morechem

Joshua F. (United States of America)
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  1. law of partial pressures
    (chemistry and physics) law stating that the pressure exerted by a mixture of gases equals the sum of the partial pressures of the gases in the mixture; the pressure of a gas in a mixture equals the pressure it would exert if it occupied the same volume alone at the same temperature
    Real gases occupy space and exert attractive forces on one another
    Likely to behave nearly ideally Likely not to behave ideally
    Gases at high temperature and low pressure Gases at low temperature and high pressure
    Small non-polar gas molecules Large, polar gas molecules
    14.4 Gases: Mixtures and Movements
    I. Dalton's Law of Partial Pressures
    A. Partial Pressure
    1.
  2. molarity
    concentration measured by molecular weight of a substance
    Molarity describes the concentration of a solution in moles of solute divided by liters of solution.
  3. endothermic reaction
    a chemical reaction accompanied by the absorption of heat
    Increasing temperature causes the reaction to shift in a way so as to use up the added energy
    (away from the side that has energy)
    Endothermic reaction
    X + Y + Energy ' Z
    
    Exothermic reaction
    A + B ' C + D + Energy
    
    b.
  4. valence electron
    an electron in the outer shell of an atom which can combine with other atoms to form molecules
    "Dope" silicon with elements such as arsenic
    (1) extra valence electron increases conductivity
    3. p-type semiconductors
    a.
  5. atomic spectrum
    (physics) a spectrum of radiation caused by electron transitions within an atom; the series of spectrum lines is characteristic of the element
    Atomic Spectra
    A. Ground State
    1.
  6. trichloromethane
    a volatile liquid haloform ; formerly used as an anesthetic
    Formulas indicating the kind, number, arrangement, and bonds but not unshared pairs of the
    atoms in a molecule 4
    D. Drawing Lewis Structures (trichloromethane, CHCl3 as an example)
    1.
  7. enthalpy
    (thermodynamics) a thermodynamic quantity equal to the internal energy of a system plus the product of its volume and pressure
    Heat of Reaction
    A. Enthalpy (H)
    1.
  8. decomposition reaction
    (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
    Decomposition Reactions
    A. Decomposition Rxns
    1.
  9. covalent
    of or relating to or characterized by covalence
    These are the
    electrons usually
    involved in the
    formation of
    covalent bonds
    B. The Octet Rule – Ionic Compounds
    1.
  10. covalent bond
    a chemical bond that involves sharing a pair of electrons between atoms in a molecule
    A covalent bond produced by the sharing of two pairs of electrons between two atoms
    2.
  11. ideal gas
    a hypothetical gas with molecules of negligible size that exert no intermolecular forces
    A mathematical expression of the relationship
    between pressure, volume and temperature of a
    fixed amount of gas (constant mass)
    (in real life experiments, pressure, volume and temperature may all change)

    2
    2 2
    1
    1 1
    T
    P V
    T
    PV
    ∴ =
    14.3 Ideal Gases
    I. Ideal Gas Law
    A. The mathematical relationship of pressure, volume, temperature, and the number of moles of a gas.
  12. activation energy
    the energy that an atomic system must acquire before a process (such as an emission or reaction) can occur
    Activation Energy and the Activated Complex
    A. Activated Complex
    1.
  13. electronegativity
    (chemistry) the tendency of an atom or radical to attract electrons in the formation of an ionic bond
    Trends in Electronegativity
    A. Electronegativity
    1.
  14. nonmetal
    not resembling shiny, malleable, conductive elements
    Metals, Nonmetals, and Metalloids
    A. Metals
    1.
  15. atomic mass
    the property of an atom that causes it to have weight
    Using Atomic Mass
    A. Average Atomic Masses
    1.
  16. dipole
    an aerial half a wavelength long consisting of two rods connected to a transmission line at the center
    Light is scattered in a colloid
    Table 11.7 Types of Colloids
    Examples
    Dispersing
    Medium
    Dispersed
    Substance
    Colloid Type
    Fog, aerosol sprays Gas Liquid Aerosol
    Smoke, airborne bacteria Gas Solid Aerosol
    Whipped cream, soap suds Liquid Gas Foam
    Milk, mayonnaise Liquid Liquid Emulsion
    Paint, clays, gelatin Liquid Solid Sol
    Marshmallow, polystyrene foam Solid Gas Solid foam
    Butter, cheese Solid Liquid Solid emulsion
    Ruby glass Solid Solid Solid sol

    1
    Chapter 10 - Liquids and Solids
    10.1 Int...
  17. solute
    the dissolved matter in a homogenous liquid mixture
    The dissolving medium in a solution
    D. Solute
    1.
  18. unit cell
    the smallest group of atoms or molecules whose repetition at regular intervals in three dimensions produces the lattices of a crystal
    The total three dimensional arrangement of particles of a crystal
    B. Unit Cell
    1.
  19. vapor pressure
    the pressure exerted by a vapor
    Vapor Pressure
    a.
  20. polyatomic
    of or relating to a molecule made up of more than two atoms
    Polyatomic Ions
    A. Oxyanions
    1.
  21. mass number
    the sum of the number of neutrons and protons in an atomic nucleus
    Short range attractive forces:
    neutron-to-neutron, proton-to-proton, proton-to-neutron
    Particle Symbols Relative charge Mass Number
    Electron
    e
    -
    e
    0
    −1
    -1 0
    Proton
    p
    +

    1
    1
    H
    +1 1
    Neutron
    n° n
    1
    0
    0 1

    4.3 Distinguishing Among Atoms
    I. Atomic Number, Mass Number, and Isotopes
    A. Atomic Number (Z)
    1.
  22. stoichiometry
    (chemistry) the relation between the quantities of substances that take part in a reaction or form a compound (typically a ratio of whole integers)
    Molecules with preferential orientation in an electric field
    + + +
    - - - 1
    Unit 4 – Conservation of Mass and Stoichiometry
    9.1 Naming Ions
    I. Monatomic Ions
    A. Monatomic ions
    1.
  23. noble gas
    any of the chemically inert gaseous elements of the helium group in the periodic table
    Noble gases have a very high ionization energy
    E. Removing Additional Electrons
    Na + 496 kJ/mol Æ Na
    +
    + e
    -
    Na
    +
    + 4562 kJ/mol Æ Na
    ++
    + e
    -
    Na
    ++
    + 6912 kJ/mol Æ Na
    +++
    + e
    -
    1.
  24. intermolecular
    existing or acting between molecules
    Overcoming intermolecular forces in the solvent to make room for the solute
    (expanding the solvent)
    a.
  25. kelvin
    the basic unit of thermodynamic temperature adopted under the Systeme International d'Unites
    T = Temperature in Kelvins
    2.
  26. trigonal
    having threefold symmetry
    Lone pairs do not cause distortion when bond angles are 120° or greater 6
    Arrangement of Electron Pairs Around an Atom Yielding Minimum
    Repulsion
    # of Electron
    Pairs
    Shape Arrangement of Electron Pairs
    2 Linear

    3 Trigonal Planar
    4 Tetrahedral
    5 Trigonal bipyramidal

    6 Octahedral

    8.4 Polar Bonds and Molecules
    I. Bond Polarity
    A. Nonpolar Covalent Bond
    1.
  27. electronegative
    having a negative charge
    Otherwise, the least electronegative element atom is central (except for hydrogen,
    which is never central).
  28. reactant
    a substance that is altered during a chemical process
    Balancing is done with coefficients - small whole numbers that appear in front of a formula
    2H2 + O2 Æ 2H2O
    D. Additional symbols used in Chemical equations
    Table 11.1 Symbols Used in Chemical Equations
    Symbol Explanation
    + Used to separate two reactants or products
    Æ "Yields," separates reactants from products
    ' Used in place of a single arrow to indicate a reversible reactions
    (s) Reactant or product in the solid state.
  29. energy state
    a definite stable energy that a physical system can have
    Gamma rays (γ) are high-energy electromagnetic waves emitted from a nucleus as it changes from an
    excited state to a ground energy state
    2.
  30. monatomic
    of or relating to an element consisting of a single atom
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  31. exothermic reaction
    a chemical reaction accompanied by the evolution of heat
    Increasing temperature causes the reaction to shift in a way so as to use up the added energy
    (away from the side that has energy)
    Endothermic reaction
    X + Y + Energy ' Z
    
    Exothermic reaction
    A + B ' C + D + Energy
    
    b.
  32. orbital point
    the craniometric point at the lowest point on the lower edge of the orbit
    Lobes of bonding orbital point toward
    each other
    c.
  33. gas constant
    (physics) the universal constant in the gas equation: pressure times volume = R times temperature; equal to 8.3143 joules per kelvin per mole
    The ideal gas law reduces to Boyle's, Charles's, or Gay-Lussac's Law if the necessary variable is held
    constant
    B. The Ideal Gas Constant
    1.
  34. nucleon
    a constituent (proton or neutron) of an atomic nucleus
    Molar mass of an element equals the average atomic mass in gram units
    25.1 Nuclear Radiation
    I. Introduction
    A. Nucleons
    1.
  35. atomic number
    quantity of protons in the nucleus of an atom of an element
    Short range attractive forces:
    neutron-to-neutron, proton-to-proton, proton-to-neutron
    Particle Symbols Relative charge Mass Number
    Electron
    e
    -
    e
    0
    −1
    -1 0
    Proton
    p
    +

    1
    1
    H
    +1 1
    Neutron
    n° n
    1
    0
    0 1

    4.3 Distinguishing Among Atoms
    I. Atomic Number, Mass Number, and Isotopes
    A. Atomic Number (Z)
    1.
  36. molal
    designating a solution containing one mole of solute per kilogram of solvent
    Freezing-Point Depression
    A. Molal Freezing-Point Constant for Water
    1.
  37. empirical formula
    a chemical formula showing the ratio of elements in a compound rather than the total number of atoms
    Empirical Formula
    A. Definition:
    The symbols for the elements combined in a compound, with subscripts showing the smallest
    whole-number ratio of the different atoms in the compound
    B. Calculation of Empirical Formula
    1.
  38. electron
    an elementary particle with negative charge
    Most of the atomic radius is due to the electron cloud
    B. Nuclear radius
    1.
  39. beta particle
    a high-speed electron or positron emitted in the decay of a radioactive isotope
    Beta particle (β) is an electron emitted from the nucleus during nuclear decay
    β
    0
    1
    1
    1
    1
    0 → + −
    n p
    2.
  40. semipermeable
    (of a membrane) selectively permeable
    The flow of solvent molecules into a solution through a semipermeable
    membrane
    B. Osmotic Pressure
    1.
  41. ground state
    the lowest energy state of an atom or other particle
    The atom achieves the ground state when atoms occupy the closest possible positions around
    the nucleus
    4.
  42. double bond
    a covalent bond in which two pairs of electrons are shared between two atoms
    Multiple Covalent Bonds
    A. Double Bonds
    1.
  43. isotonic solution
    a solution having the same osmotic pressure as blood
    Transfer of solvent molecules as well as small solute molecules and ions
    D. Isotonic Solutions
    1.
  44. endothermic
    occurring or formed with absorption of heat
    ∆H is positive for an endothermic rxn
    (1) Heat content of products is greater than the heat content of the reactants
    b.
  45. exothermic
    occurring or formed with the release of heat
    ∆H is negative for an exothermic rxn
    (1) Heat content of the reactants is greater than the heat content of the products
    C. Writing Thermochemical Equations
    1.
  46. ionic
    containing or involving electrically charged particles
    The simplest collection of atoms from which an ionic compound's formula can be established
    II.
  47. energy level
    a definite stable energy that a physical system can have
    Gamma rays are produced when nuclear particles undergo transitions in energy levels
    3.
  48. diatomic
    of or relating to a molecule made up of two atoms
    A neutral group of atoms that are held together by covalent bonds
    B. Diatomic Molecule
    1.
  49. thermochemistry
    the branch of chemistry that studies the relation between chemical action and the amount of heat absorbed or generated
    Bases are proton acceptors in solution

    1
    m T
    q
    cp
    ⋅
    ∆
    = q =
    cp
    ⋅ m ⋅
    ∆ T
    Unit 7 – Kinetics and Thermodynamics
    17-1 Thermochemistry
    Thermochemistry - The study of the changes in heat energy that accompany chemical reactions and physical changes
    I. Heat and Temperature
    A. Calorimeter
    1.
  50. solubility
    the quality of being easily dissolved in liquid
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  51. ethene
    a flammable colorless gaseous alkene
    Trigonal planar structure, 120° angle, in ethene
    (ethylene) rules out sp
    3
    hybridization
    2. sp
    2
    hybridization creates 3 identical orbitals of
    intermediate energy and length and leaves one
    unhybridized p orbital
    3.
  52. hemolysis
    lysis of erythrocytes with the release of hemoglobin
    Hemolysis
    a.
  53. exclusion principle
    no two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
    Pauli Exclusion Principle
    a.
  54. anion
    a particle with a negative electric charge
    Less shielding of electrons
    B. Anions
    1.
  55. molar
    grinding tooth with a broad crown
    Avogadro's number = 6.022 x 10
    23

    C. Molar Mass
    1.
  56. proton
    a stable particle with positive charge
    Protons
    a.
  57. cation
    a particle with a positive electric charge
    Trends in Ionic Size
    A. Cations
    1.
  58. standard pressure
    a unit of pressure: the pressure that will support a column of mercury 760 mm high at sea level and 0 degrees centigrade
    Standard Pressure = 101.3 kPa or 1 atmosphere
    B. Standard Molar Volume
    1.
  59. hybridization
    (genetics) the act of mixing different species or varieties of animals or plants and thus to produce hybrids
    Very strong s bonds between carbons in fused rings using sp
    2
    hybridization
    2. p molecular orbitals provide weaker p bonding between layers
    a.
  60. molecule
    the simplest structural unit of an element or compound
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  61. stoichiometric
    of or relating to stoichiometry
    Other Stoichiometric Calculations
    A. Gas Volume
    1.
  62. mol
    the molecular weight of a substance expressed in grams
    Units are grams/mole (or g/mol)
    b.
  63. heat energy
    a form of energy that is transferred by a difference in temperature
    Bases are proton acceptors in solution

    1
    m T
    q
    cp
    ⋅
    ∆
    = q =
    cp
    ⋅ m ⋅
    ∆ T
    Unit 7 – Kinetics and Thermodynamics
    17-1 Thermochemistry
    Thermochemistry - The study of the changes in heat energy that accompany chemical reactions and physical changes
    I. Heat and Temperature
    A. Calorimeter
    1.
  64. halogen
    any of five related nonmetallic elements (fluorine or chlorine or bromine or iodine or astatine) that are all monovalent and readily form negative ions
    Nonmetals
    (1) Halogens (Group 17) are most reactive of the nonmetals
    D. f-Block, Lanthanides and Actinides
    1.
  65. hybridize
    breed animals or plants using parents of different races and varieties
    Bonds formed by overlap of hybridized sp
    3
    orbitals
    C. Graphite
    1.
  66. colloid
    a mixture with properties between those of a solution and fine suspension
    Colloids
    A. Colloidal Dispersions (Colloids)
    1.
  67. alpha particle
    a positively charged particle that is the nucleus of the helium atom; emitted from natural or radioactive isotopes
    Alpha particles (helium nuclei) fired at a thin sheet of gold
    a.
  68. ionize
    convert into ions
    Strong acids ionize completely in solution
    2.
  69. bonding
    the act of fastening firmly together
    Electronegativity tends to decrease down a group of main-group elements 1
    Unit 3 - Chemical Bonding and Molecular Structure
    7.1 Ions
    I. Valence Electrons – Outer energy
    level electrons
    A. Electron-dot Notation
    1.
  70. radioactive decay
    the spontaneous disintegration of a radioactive substance along with the emission of ionizing radiation
    Radioactivity
    A. Radioactive Decay
    1.
  71. crystal lattice
    a 3-dimensional geometric arrangement of the atoms or molecules or ions composing a crystal
    The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice
    III.
  72. hydrophilic
    having a strong affinity for water
    Polar (hydrophilic) dissolves in polar
    a.
  73. rest mass
    (physics) the mass of a body as measured when the body is at rest relative to an observer, an inherent property of the body
    A photon is a particle of energy having a rest mass of zero and carrying a quantum of
    energy
    b.
  74. ionization
    the process of ionizing
    Trends in Ionization Energy
    A. Ion
    1.
  75. lawrencium
    a radioactive transuranic element synthesized from californium
    Plutonium (94) through Lawrencium (103) are man-made
    6.3 Periodic Trends
    I. Atomic Radii
    A. Atomic Radius
    1.
  76. STP
    standard temperature and pressure
    The Mole-Volume Relationship
    A. Standard Temperature and Pressure (STP)
    1.
  77. subscript
    character printed slightly below and to the side of another
    Indicates the relative numbers of atoms of each kind of a chemical compound by using atomic
    symbols and numerical subscripts
    E. Molecular Formula
    1.
  78. osmotic pressure
    (physical chemistry) the pressure exerted by a solution necessary to prevent osmosis into that solution when it is separated from the pure solvent by a semipermeable membrane
    Osmotic Pressure
    B. Boiling-Point Elevation
    1.
  79. melting point
    the temperature at which a solid turns into a liquid
    Soft, silvery metals of low density and low melting points
    c.
  80. line spectrum
    a spectrum in which energy is concentrated at particular wavelengths; produced by excited atoms and ions as they fall back to a lower energy level
    A state in which an atom has a higher potential energy than in its ground state
    C. Bright line spectrum
    1.
  81. chemical property
    a property used to characterize materials in reactions that change their identity
    Definite wavelength
    6.1 Organizing the Elements
    I. The Periodic Law
    A. The physical and chemical properties of the elements are periodic functions of their atomic numbers
    B. Elements on the table are arranged in order of increasing atomic number (number of protons)
    II.
  82. joule
    a unit of electrical energy
    Heat is usually measured in joules, J

    2
    2
    1
    s
    kg m
    J N m
    ⋅
    = ⋅ =
    a.
  83. kinetic energy
    the mechanical energy that a body has by virtue of motion
    They therefore possess kinetic energy, the energy of
    motion
    II.
  84. ion
    a particle that is electrically charged positive or negative
    Trends in Ionization Energy
    A. Ion
    1.
  85. electromagnetic radiation
    radiation consisting of waves of energy associated with electric and magnetic fields resulting from the acceleration of an electric charge
    The spontaneous disintegration of a nucleus into a slightly lighter and more stable nucleus, accompanied
    by emission of particles, electromagnetic radiation, or both
    B. Nuclear Radiation
    1.
  86. periodic table
    arrangement of chemical elements according to atomic number
    Periodic Table is in order of increasing atomic number
    B. Mass Number
    1.
  87. electropositive
    having a positive charge
    Electropositive hydrogen of the water molecule is attracted to negatively charged ions
    2.
  88. surface tension
    phenomenon at a liquid's surface from intermolecular forces
    The point on the graph describing simultaneously the critical temperature and the critical pressure
    P = 217.75 atm Temperature = 373.99 °C
    15.1 Water and Its Properties
    I. Liquid Water
    A. Surface Tension
    1.
  89. atom
    the smallest component of an element
    Unit 1 – Atomic Structure
    4.1 Defining the Atom
    I. Atomic Theory
    A. Modern Atomic Theory
    1.
  90. gamma ray
    electromagnetic radiation emitted during radioactive decay and having an extremely short wavelength
    Gamma rays (γ) are high-energy electromagnetic waves emitted from a nucleus as it changes from an
    excited state to a ground energy state
    2.
  91. localize
    concentrate on a particular place or spot
    Washington, N.H. 6,293 590 93
    Boulder, Colorado 5,430 610 94
    Madison, Wisconsin 900 730 99
    New York City, New York 10 760 100
    Death Valley, California -282 770 100.3
    1
    Chapter 9 - Covalent Bonding: Orbitals
    9.1 Hybridization and the Localized Electron Model
    A. Hybridization
    1.
  92. solvent
    capable of meeting financial obligations
    A homogeneous mixture of two or more substances in a single phase
    C. Solvent
    1.
  93. entropy
    a numerical measure of the uncertainty of an outcome
    Most spontaneous reactions have a negative value for ÌH
    B. Entropy (S)
    1.
  94. neutron
    a subatomic particle with zero charge
    Neutrons
    a.
  95. reverse osmosis
    a method of producing pure water
    Cells placed in a hypotonic solution gain water from the solution and
    swell, possibly bursting
    F. Reverse Osmosis
    1.
  96. law of definite proportions
    (chemistry) law stating that every pure substance always contains the same elements combined in the same proportions by weight
    Naming Bases
    A. Bases are ionic compounds and are named in the same way as other ionic compounds 3
    9.5 The Laws Governing Formulas and Names
    I. The Law of Definite Proportions
    “In samples of any chemical compound, the masses of the elements are always in the same proportions.”
  97. isotope
    atom with same atomic number, different number of neutrons
    Short range attractive forces:
    neutron-to-neutron, proton-to-proton, proton-to-neutron
    Particle Symbols Relative charge Mass Number
    Electron
    e
    -
    e
    0
    −1
    -1 0
    Proton
    p
    +

    1
    1
    H
    +1 1
    Neutron
    n° n
    1
    0
    0 1

    4.3 Distinguishing Among Atoms
    I. Atomic Number, Mass Number, and Isotopes
    A. Atomic Number (Z)
    1.
  98. aqueous solution
    a solution in water
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  99. surface area
    the extent of a 2-dimensional surface enclosed within a boundary
    Factors Affecting Gas Pressure
    A. Amount of Gas
    1. ⇑ molecules = ⇑ collisions with walls = ⇑ pressure
    2. ⇓ molecules = ⇓ collisions with walls = ⇓ pressure
    B. Volume
    1. ⇑ volume = ⇑ surface area = ⇓ collisions per unit of area = ⇓ pressure
    2. ⇓ volume = ⇓ surface area = ⇑ collisions per unit of area = ⇑ pressure
    C. Temperature
    1. ⇑ temperature = ⇑ molecule speed = ⇑ frequent (and harder) collisions = ⇑ pressure
    2. ⇓ temperature = ⇓ molecule speed = ⇓ frequent (and softer) coll...
  100. electromagnetic wave
    radiation consisting of waves of energy associated with electric and magnetic fields resulting from the acceleration of an electric charge
    Gamma rays (γ) are high-energy electromagnetic waves emitted from a nucleus as it changes from an
    excited state to a ground energy state
    2.
  101. alkali metal
    any of the monovalent metals of group I of the periodic table (lithium or sodium or potassium or rubidium or cesium or francium)
    Group 1 - The alkali metals
    a.
  102. Kelvin
    British physicist who invented the Kelvin scale of temperature and pioneered undersea telegraphy (1824-1907)
    Kelvin temperature is directly proportional to the average kinetic energy of a substance
    a.
  103. molecular
    relating to the simplest units of an element or compound
    Electronegativity tends to decrease down a group of main-group elements 1
    Unit 3 - Chemical Bonding and Molecular Structure
    7.1 Ions
    I. Valence Electrons – Outer energy
    level electrons
    A. Electron-dot Notation
    1.
  104. conservation of mass
    a fundamental principle of classical physics that matter cannot be created or destroyed in an isolated system
    Molecules with preferential orientation in an electric field
    + + +
    - - - 1
    Unit 4 – Conservation of Mass and Stoichiometry
    9.1 Naming Ions
    I. Monatomic Ions
    A. Monatomic ions
    1.
  105. chemical bond
    an electrical force linking atoms
    Chemical bonds are not being broken during phase changes
    2.
  106. nuclear reaction
    (physics) a process that alters the energy or structure or composition of atomic nuclei
    A change in the identity of a nucleus as a result of a change in the number of its protons
    B. Nuclear Reaction
    1.
  107. radio wave
    an electromagnetic wave with a wavelength between 0.5 cm to 30,000 m
    Many types of EM waves
    a. visible light
    b. x-rays
    c. ultraviolet light
    d. infrared light
    e. radio waves
    2.
  108. positively charged
    having a positive charge
    Assumed that the positively charged particles were bounced back if they approached a
    positively charged atomic nucleus head-on (Like charges repel one another)
    2.
  109. chemical equilibrium
    a chemical reaction and its reverse proceed at equal rates
    A chemical reaction in which the products can react to re-form the reactants
    B. Chemical Equilibrium
    1.
  110. half-life
    the time required for something to fall to half its initial value (in particular, the time for half the atoms in a radioactive substance to disintegrate)
    Half-Life
    A. Half-Life (t1/2)
    1.
  111. hypotonic
    (of living tissue) lacking normal tone or tension
    Cells placed in a hypotonic solution gain water from the solution and
    swell, possibly bursting
    F. Reverse Osmosis
    1.
  112. carboxyl group
    the univalent radical -COOH
    Covalent molecular substances containing a carboxyl group
    a.
  113. wavelength
    a way of thinking or coming to mutual understanding
    Speed is equal to the frequency times the wavelength c = νλ
    (1).
  114. aerosol
    a cloud of solid or liquid particles in a gas
    Light is scattered in a colloid
    Types of Colloids
    Examples
    Dispersing
    Medium
    Dispersed
    Substance
    Colloid Type
    Fog, aerosol sprays Gas Liquid Aerosol
    Smoke, airborne bacteria Gas Solid Aerosol
    Whipped cream, soap suds Liquid Gas Foam
    Milk, mayonnaise Liquid Liquid Emulsion
    Paint, clays, gelatin Liquid Solid Sol
    Marshmallow, polystyrene foam Solid Gas Solid foam
    Butter, cheese Solid Liquid Solid emulsion
    Ruby glass Solid Solid Solid sol
    16.1 Properties of Solutions
    I. F...
  115. octet
    eight performers or singers who perform together
    These are the
    electrons usually
    involved in the
    formation of
    covalent bonds
    B. The Octet Rule – Ionic Compounds
    1.
  116. orbital
    relating to the path of one body around another
    Atomic Orbitals
    A. Atomic orbital
    1.
  117. structural formula
    an expanded molecular formula showing the arrangement of atoms within the molecule
    Formulas in which atomic symbols represent nuclei and inner-shell
    electrons, dot pairs or dashes between two atomic symbols
    represent electron pairs in covalent bonds, and dots adjacent to only
    one atomic symbol represent unshared electrons
    C. Structural Formula
    1.
  118. particle
    (nontechnical usage) a tiny piece of anything
    All matter is made up of very tiny particles called atoms
    2.
  119. cathode ray
    a beam of electrons emitted by the cathode of an electrical discharge tube
    Cathode ray tube produces a ray with a constant charge to mass ratio
    b.
  120. Avogadro
    Italian physicist noted for his work on gases
    The amount of substance that contains the Avogadro number of particles
    B. Avogadro's Number
    1.
  121. H2O
    binary compound that occurs at room temperature as a clear colorless odorless tasteless liquid; freezes into ice below 0 degrees centigrade and boils above 100 degrees centigrade; widely used as a solvent
    This is done with a formula equation
    H2 + O2 Æ H2O
    C. The law of conservation of atoms must be satisfied
    1.
  122. sulfide
    a compound of sulphur and some other element that is more electropositive
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  123. kinetic
    relating to the motion of material bodies and their forces
    The ratio of the actual yield to the theoretical yield, multiplied by 100
    x 100
    theoretical yield
    actual yield
    percent yield =
    1
    Unit 5 – Gases and Gas Laws
    13.1 The Nature of Gases
    I. The Kinetic Theory and a Model for Gases
    A. Assumptions of the Kinetic-Molecular Theory
    1.
  124. photon
    a tiny bundle of matter that transmits light
    Radiant energy is transferred in units (or quanta) of energy called photons
    a.
  125. torr
    a unit of pressure equal to 0.001316 atmosphere
    Gas molecules exert force,
    and therefore pressure, on
    any surface with which they
    collide
    B. Units of Pressure
    Units of Pressure
    Unit Symbol Definition/Relationship
    Pascal Pa SI pressure unit
    1 Pa =
    2
    1
    m
    N
    Millimeter of mercury mm Hg Pressure that supports a 1 mm column of mercury in a
    barometer
    Atmosphere atm Average atmospheric pressure at sea level and 0 °C
    Torr torr 1 torr = 1 mm Hg
    C. Standard Pressure
    1.
  126. alkaline earth
    any of the bivalent metals of group II of the periodic table
    Group 2 - The alkaline earth metals
    a.
  127. boiling point
    the temperature at which a liquid boils at sea level
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  128. chemical reaction
    a process in which substances are changed into others
    = 34.02)
    (HO weight)x = 34.02
    HO = 17.01 (1.01 + 16.00)
    (17.01)x = 34.02
    x = 2
    Molecular formula is (HO)2
    ∴ Molecular formula is H2O25
    11.1 Describing Chemical Reactions
    I. Introduction
    A. Reactants
    1.
  129. low density
    a rarified quality
    Soft, silvery metals of low density and low melting points
    c.
  130. immiscible
    (chemistry, physics) incapable of mixing
    Immiscible - Liquid solutes and solvents that are not soluble in each other
    a.
  131. benzene ring
    a closed chain of 6 carbon atoms with hydrogen atoms attached
    Localized model
    2. p bonds are a result of remaining p orbitals above and below the plane of
    the benzene ring
  132. valence
    the capacity of something or someone to react with or affect others
    Electronegativity tends to decrease down a group of main-group elements 1
    Unit 3 - Chemical Bonding and Molecular Structure
    7.1 Ions
    I. Valence Electrons – Outer energy
    level electrons
    A. Electron-dot Notation
    1.
  133. equation
    a mathematical statement that two expressions are the same
    B. Regions of probability in which electrons may be found in an atom are determined by mathematical
    equations.
  134. capillary action
    a phenomenon associated with surface tension and resulting in the elevation or depression of liquids in capillaries
    Capillary Action
    a.
  135. nucleus
    a part of the cell responsible for growth and reproduction
    The Nucleus
    A. The Rutherford Experiment (1911)
    1.
  136. binary compound
    chemical compound composed of only two elements
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    A. B...
  137. freezing point
    the temperature below which a liquid turns into a solid
    Freezing and Melting
    A. Freezing Point
    1.
  138. isotonic
    of two or more muscles; having equal tension
    Transfer of solvent molecules as well as small solute molecules and ions
    D. Isotonic Solutions
    1.
  139. hypertonic
    (of living tissue) in a state of abnormally high tension
    Cells placed in a hypertonic solution lose water to the solution, and
    shrink
    2.
  140. vapor
    a visible suspension in the air of particles of a substance
    Molecules with sufficient kinetic energy escape as vapor from the surface of the liquid
    2.
  141. hydrogen chloride
    a colorless corrosive gas (HCl)
    Example - Hydrogen Chloride
    H
    1s
    Cl
    1s 2s 2p 3s
    II.
  142. specific heat
    the heat required to raise the temperature of one gram of a substance one degree centigrade
    Heat Capacity and Specific Heat
    A. Specific Heat
    1.
  143. chemical compound
    (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
    A measure of the ability of an atom in a chemical compound to attract electrons
    2.
  144. polystyrene
    a polymer of styrene; a rigid transparent thermoplastic
    Light is scattered in a colloid
    Types of Colloids
    Examples
    Dispersing
    Medium
    Dispersed
    Substance
    Colloid Type
    Fog, aerosol sprays Gas Liquid Aerosol
    Smoke, airborne bacteria Gas Solid Aerosol
    Whipped cream, soap suds Liquid Gas Foam
    Milk, mayonnaise Liquid Liquid Emulsion
    Paint, clays, gelatin Liquid Solid Sol
    Marshmallow, polystyrene foam Solid Gas Solid foam
    Butter, cheese Solid Liquid Solid emulsion
    Ruby glass Solid Solid Solid sol
    16.1 Properties of Solutions
    I. F...
  145. solid solution
    a homogeneous solid that can exist over a range of component chemicals; a constituent of alloys that is formed when atoms of an element are incorporated into the crystals of a metal
    Solid solutions
    a.
  146. attractive force
    the force by which one object attracts another
    Short range attractive forces:
    neutron-to-neutron, proton-to-proton, proton-to-neutron
    Particle Symbols Relative charge Mass Number
    Electron
    e
    -
    e
    0
    −1
    -1 0
    Proton
    p
    +

    1
    1
    H
    +1 1
    Neutron
    n° n
    1
    0
    0 1

    4.3 Distinguishing Among Atoms
    I. Atomic Number, Mass Number, and Isotopes
    A. Atomic Number (Z)
    1.
  147. le Chatelier
    French chemist who formulated Le Chatelier's principle
    Catalysts provide an alternate
    reaction mechanism or pathway
    with a lower activation energy 4
    18.1 – 18.2 Equilibrium and Le Chatelier’s Principle
    A. Reversible Reactions
    1.
  148. negatively charged
    having a negative charge
    All cathode rays are composed of identical negatively charged particles (electrons)
    B. Inferences from the properties of electrons
    1.
  149. negative charge
    the state of having a surplus of electrons
    An atom or a group of atoms that has a positive or negative charge
    B. Ionization
    1.
  150. positive charge
    the state of having a deficiency of electrons
    Atoms are neutral, so there must be positive charges to balance the negatives
    2.
  151. compound
    a whole formed by a union of two or more elements or parts
    A measure of the ability of an atom in a chemical compound to attract electrons
    2.
  152. nuclear fusion
    a nuclear reaction in which nuclei combine to form more massive nuclei with the simultaneous release of energy
    Nuclear Fusion
    A. Nuclear Fusion
    1.
  153. liquid
    fluid matter having no fixed shape but a fixed volume
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  154. reactivity
    responsive to stimulation
    Lanthanides are shiny metals similar in reactivity to the Group 2 metals
    2.
  155. nuclear fission
    a nuclear reaction in which a massive nucleus splits into smaller nuclei with the simultaneous release of energy
    Total atomic numbers and mass numbers must be equal on both sides
    Be He C n
    1
    0
    12
    6
    4
    2
    9
    4
    + → +
    25.3 Fission and Fusion of Atomic Nuclei
    I. Nuclear Fission
    A. Nuclear Fission
    1.
  156. Protium
    genus of chiefly tropical American trees having fragrant wood and yielding gum elemi
    Hydrogen as an example:

    Protium (hydrogen-1) Deuterium (hydrogen-2) Tritium (hydrogen-3)

    D. Designating Isotopes
    1.
  157. activation
    causing something to take effect or to have energy
    Activation Energy and the Activated Complex
    A. Activated Complex
    1.
  158. atomic
    relating to the smallest component of an element
    Unit 1 – Atomic Structure
    4.1 Defining the Atom
    I. Atomic Theory
    A. Modern Atomic Theory
    1.
  159. nitride
    a compound containing nitrogen and a more electropositive element (such as phosphorus or a metal)
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  160. carbon tetrachloride
    a colorless nonflammable liquid used as a solvent for fats and oils; because of its toxicity its use as a cleaning fluid or fire extinguisher has declined
    Benzene and carbon tetrachloride (both nonpolar)
    b.
  161. ammeter
    a meter that measures the flow of electrical current in amperes
    Lamp glows brightly, ammeter registers a substantial current
    2.
  162. aqueous
    similar to or containing or dissolved in water
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  163. gaseous state
    the state of matter distinguished from the solid and liquid states by: relatively low density and viscosity; relatively great expansion and contraction with changes in pressure and temperature; the ability to diffuse readily; and the spontaneous tendency to become distributed uniformly throughout any container
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  164. sulfate
    a salt or ester of sulphuric acid
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  165. sterling silver
    a silver alloy with no more than 7.5% copper
    Sterling silver
    a.
  166. carboxyl
    the univalent radical -COOH
    Covalent molecular substances containing a carboxyl group
    a.
  167. periodic law
    (chemistry) the principle that chemical properties of the elements are periodic functions of their atomic numbers
    Definite wavelength
    6.1 Organizing the Elements
    I. The Periodic Law
    A. The physical and chemical properties of the elements are periodic functions of their atomic numbers
    B. Elements on the table are arranged in order of increasing atomic number (number of protons)
    II.
  168. computerize
    provide with computers
    Diffractometer
    a. computerized device to rotate crystal samples in an x-ray field, gather
    incidence and reflection data, and construct models of crystal
    structure3
    C. Types of Crystalline Solids
    1.
  169. configuration
    an arrangement of parts or elements
    Two possible values for spin, +1/2, -1/2
    5.2 Electron Arrangement in Atoms
    I. Writing Electrons Configurations
    A. Rules
    1.
  170. quark
    fundamental subatomic particle that has a fractional charge
    Can be broken into simpler substances by chemical means, not
    by physical means
    The Organization of Matter
    (Slightly different than your book)
    Matter
    Mixtures:
    a) Homogeneous
    (Solutions)
    b) Heterogeneous
    Pure Substances
    Compounds
    s
    Elements
    Atoms
    Nucleus Electrons
    Protons Neutrons
    Quarks Quarks

    1
    A B
    A
    A
    n n
    n
    Mole fraction of componentA x
    +
    = =
    Chapter 11 – Properties of Solutions
    11.1 Solution Composition
    A. Molarity
    1.
    liters of solution
    moles solute
    Molarity(M ) =
    B. Mas...
  171. worksheet
    a sheet of paper with multiple columns
    Refer to the “Naming Acids” worksheet
    II.
  172. hydrophobic
    lacking affinity for water
    Nonpolar (hydrophobic) in nonpolar
    a.
  173. dissociation
    the act of removing from association
    A substance combines with oxygen, releasing a large amount of energy in the form of light and heat
    2H2(g) + O2(g) Æ 2H2O(g)
    B. Hydrocarbon combustion always produces carbon dioxide and water
    2C2H6(g) + 7O2(g) Æ 4CO2(g) + 6H2O(g)
    11.3 Reactions in Aqueous Solution
    I. Dissociation
    A. Dissociation
    1.
  174. chlorate
    any salt of chloric acid
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  175. perchlorate
    a salt of perchloric acid
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  176. hydration
    the process of combining with water
    Hydration
    1.
  177. conductivity
    the property of transmitting heat, electricity, or sound
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  178. formula
    a group of symbols that make a mathematical statement
    Examples include NaCl, MgBr2, Na2O
    B. Formula Unit
    1.
  179. hydrogen
    a colorless, odorless gas; the lightest chemical element
    Hydrogen as an example:

    Protium (hydrogen-1) Deuterium (hydrogen-2) Tritium (hydrogen-3)

    D. Designating Isotopes
    1.
  180. temperature
    the degree of hotness or coldness of a body or environment
    The Mole-Volume Relationship
    A. Standard Temperature and Pressure (STP)
    1.
  181. reactive
    participating in processes changing substances into others
    Highly reactive, never found pure in nature
    2.
  182. liquid state
    the state in which a substance exhibits a characteristic readiness to flow with little or no tendency to disperse and relatively high incompressibility
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  183. Celsius
    Swedish astronomer who devised the centigrade thermometer
    The amount of heat required to raise the temperature of one gram of substance by one Celsius degree
    (1°C) or one Kelvin (1 K)
    B. Calculating Specific Heat
    1.
  184. viscosity
    resistance of a liquid to flowing
    Oxygen in glass is attracted to hydrogen in water
    C. Viscosity
    1.
  185. vaporize
    turn into gas
    The amount of heat energy required to vaporize one mole of a liquid at its boiling point
    2.
  186. half life
    the time required for something to fall to half its initial value (in particular, the time for half the atoms in a radioactive substance to disintegrate)
    Less stable nuclides decay rapidly
    Table 22-2 Representative Radioactive Nuclides and Their Half Lives
    Nuclide Half-life Nuclide Half-life
    H
    3
    1
    12.32 years
    Po
    214
    84
    163.7 µseconds
    C
    14
    6
    5715 years
    Po
    218
    84
    3.0 minutes
    P
    32
    15
    14.28 days
    At
    218
    85
    1.6 seconds
    K
    40
    19
    1.3 x 109 years U
    238
    92
    4.46 x 10
    9
    years
    Co
    60
    27
    10.47 minutes
    Pu
    239
    94
    2.41 x 10
    4
    years III.
  187. sublimation
    a change directly from the solid to the gaseous state
    Temperature remains constant during a phase change
    B. Sublimation and Deposition
    1.
  188. thermodynamic
    of or concerned with thermodynamics
    Bases are proton acceptors in solution

    1
    m T
    q
    cp
    ⋅
    ∆
    = q =
    cp
    ⋅ m ⋅
    ∆ T
    Unit 7 – Kinetics and Thermodynamics
    17-1 Thermochemistry
    Thermochemistry - The study of the changes in heat energy that accompany chemical reactions and physical changes
    I. Heat and Temperature
    A. Calorimeter
    1.
  189. amorphous
    having no definite form or distinct shape
    Amorphous Solids - substances in which the particles are arranged randomly
    B. Definite Shape and Volume
    C. Definite Melting Point
    1.
  190. miscible
    capable of being mixed, in chemistry
    Miscible - Liquids that dissolve freely in one another in any proportion
    a.
  191. tetrachloride
    any compound that contains four chlorine atoms per molecule
    Benzene and carbon tetrachloride (both nonpolar)
    b.
  192. radioactive
    exhibiting or caused by emissions in nuclear decay
    Radioactivity
    A. Radioactive Decay
    1.
  193. digit
    a finger or toe, or a corresponding body part
    Record all digits that are certain
    2.
  194. reaction
    an idea evoked by some experience
    Transmutation Reactions
    A. Transmutations
    1.
  195. electromagnetic
    pertaining to or exhibiting magnetism produced by electric charge in motion
    The spontaneous disintegration of a nucleus into a slightly lighter and more stable nucleus, accompanied
    by emission of particles, electromagnetic radiation, or both
    B. Nuclear Radiation
    1.
  196. kinetics
    the science concerned with the forces that cause motion
    Bases are proton acceptors in solution

    1
    m T
    q
    cp
    ⋅
    ∆
    = q =
    cp
    ⋅ m ⋅
    ∆ T
    Unit 7 – Kinetics and Thermodynamics
    17-1 Thermochemistry
    Thermochemistry - The study of the changes in heat energy that accompany chemical reactions and physical changes
    I. Heat and Temperature
    A. Calorimeter
    1.
  197. saturate
    infuse or fill completely
    Saturated solution
    a.
  198. dry ice
    solidified carbon dioxide
    Dry ice Æ Gaseous CO2
    2.
  199. solid state
    the state in which a substance has no tendency to flow under moderate stress; resists forces (such as compression) that tend to deform it; and retains a definite size and shape
    Balancing is done with coefficients - small whole numbers that appear in front of a formula
    2H2 + O2 Æ 2H2O
    D. Additional symbols used in Chemical equations
    Table 11.1 Symbols Used in Chemical Equations
    Symbol Explanation
    + Used to separate two reactants or products
    Æ "Yields," separates reactants from products
    ' Used in place of a single arrow to indicate a reversible reactions
    (s) Reactant or product in the solid state.
  200. electrolyte
    a solution that conducts electricity
    Solutes: Electrolytes vs.
  201. decompose
    break down
    Metallic hydroxides , when heated, decompose into metallic oxides and water
    Ca(OH)2(s) Æ CaO(s) + H2O(g)
    3.
  202. atmospheric pressure
    the pressure exerted by the atmosphere
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  203. hydroxide
    a compound of an oxide with water
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  204. acceptor
    the person (or institution) who accepts a check or draft and becomes responsible for paying the party named in the draft when it matures
    Bases are proton acceptors in solution

    1
    m T
    q
    cp
    ⋅
    ∆
    = q =
    cp
    ⋅ m ⋅
    ∆ T
    Unit 7 – Kinetics and Thermodynamics
    17-1 Thermochemistry
    Thermochemistry - The study of the changes in heat energy that accompany chemical reactions and physical changes
    I. Heat and Temperature
    A. Calorimeter
    1.
  205. soluble
    capable of being dissolved in some solvent
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  206. osmosis
    diffusion of molecules through a semipermeable membrane
    Kf
    is the molal freezing point depression constant of the solvent
    c. msolute is the molality of the solute in the solution4
    11.6 Osmotic Pressure
    A. Osmosis
    1.
  207. Arrhenius
    Swedish chemist and physicist noted for his theory of chemical dissociation (1859-1927)
    Arrhenius Acids and Basees
    A. Acids
    1.
  208. benzene
    a colorless liquid hydrocarbon
    Nonpolar solvents include CCl4 and toluene (methyl benzene), C6H5CH3
    D. Liquid Solutes and Solvents
    1.
  209. emulsion
    a mixture of liquids that do not normally stay mixed
    Light is scattered in a colloid
    Types of Colloids
    Examples
    Dispersing
    Medium
    Dispersed
    Substance
    Colloid Type
    Fog, aerosol sprays Gas Liquid Aerosol
    Smoke, airborne bacteria Gas Solid Aerosol
    Whipped cream, soap suds Liquid Gas Foam
    Milk, mayonnaise Liquid Liquid Emulsion
    Paint, clays, gelatin Liquid Solid Sol
    Marshmallow, polystyrene foam Solid Gas Solid foam
    Butter, cheese Solid Liquid Solid emulsion
    Ruby glass Solid Solid Solid sol
    16.1 Properties of Solutions
    I. F...
  210. fission
    reproduction of a unicellular organism by cell division
    Total atomic numbers and mass numbers must be equal on both sides
    Be He C n
    1
    0
    12
    6
    4
    2
    9
    4
    + → +
    25.3 Fission and Fusion of Atomic Nuclei
    I. Nuclear Fission
    A. Nuclear Fission
    1.
  211. gaseous
    existing as or having the qualities of a gas
    Most are gaseous
    3.
  212. density
    the amount per unit size
    0.001 pm
    2. density is 2x10
    8
    metric tons/cm
    3
    a.
  213. equilibrium
    a stable situation in which forces cancel one another
    It occurs when the
    equilibrium vapor pressure of the liquid equals the atmospheric pressure
    B. Boiling Point
    1.
  214. absolute zero
    the lowest temperature theoretically attainable
    0 Kelvin = absolute zero = NO kinetic energy 2
    14.1 Properties of Gases
    I. Properties of Gases
    A. Expansion
    1.
  215. kinetic theory
    (physics) a theory that gases consist of small particles in random motion
    The ratio of the actual yield to the theoretical yield, multiplied by 100
    x 100
    theoretical yield
    actual yield
    percent yield =
    1
    Unit 5 – Gases and Gas Laws
    13.1 The Nature of Gases
    I. The Kinetic Theory and a Model for Gases
    A. Assumptions of the Kinetic-Molecular Theory
    1.
  216. hypochlorite
    any salt or ester of hypochlorous acid
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  217. element
    a substance that cannot be separated into simpler substances
    Atoms of the same element are chemically alike
    3.
  218. quantum
    the smallest discrete quantity of some physical property
    The Quantum Mechanical Model
    A. Probability and the Electron
    1.
  219. binary
    of or pertaining to a number system having 2 as its base
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  220. emission
    the act of causing to flow forth
    The spontaneous disintegration of a nucleus into a slightly lighter and more stable nucleus, accompanied
    by emission of particles, electromagnetic radiation, or both
    B. Nuclear Radiation
    1.
  221. butyric acid
    an unpleasant smelling fatty acid found especially in butter
    Butyric acid - in rancid butter
    b.
  222. silicate
    a salt or ester derived from silicic acid
    Most carbonates, phosphates, and silicates, are insoluble, except those of sodium,
    potassium, and ammonium
    6.
  223. reducing agent
    a substance capable of bringing about the reduction of another substance as it itself is oxidized; used in photography to lessen the density of a negative or print by oxidizing some of the loose silver
    Equivalents of oxidizing and reducing agents
    a.
  224. chemical
    produced by reactions involving atomic or molecular changes
    Atoms are not subdivided, created, or destroyed in chemical rxns
    II.
  225. atomic theory
    a theory of the structure of the atom
    Unit 1 – Atomic Structure
    4.1 Defining the Atom
    I. Atomic Theory
    A. Modern Atomic Theory
    1.
  226. sodium chloride
    a white crystalline solid consisting mainly of sodium chloride (NaCl)
    Formation of sodium chloride
    a.
  227. trioxide
    an oxide containing three atoms of oxygen in the molecule
    Second element ALWAYS gets a prefix, and an “-ide” ending
    Examples: N2O3 = dinitrogen trioxide
    CO = carbon monoxide, not monocarbon monoxide
    Numerical Prefixes
    Number 1 2 3 4 5 6 7 8 9 10
    Prefix mono di tri tetra penta hexa hepta octa nona deca
    9.4 Naming and Writing Formulas for Acids and Bases
    I. Naming Acids
    A. Binary Acids
    1.
  228. speed of light
    the speed at which light travels in a vacuum
    Travel at speeds close to the speed of light
    b.
  229. crystalline
    consisting of or containing or of the nature of crystals
    Most are crystalline solids
    b.
  230. tetra
    brightly colored tropical freshwater fishes
    Second element ALWAYS gets a prefix, and an “-ide” ending
    Examples: N2O3 = dinitrogen trioxide
    CO = carbon monoxide, not monocarbon monoxide
    Numerical Prefixes
    Number 1 2 3 4 5 6 7 8 9 10
    Prefix mono di tri tetra penta hexa hepta octa nona deca
    9.4 Naming and Writing Formulas for Acids and Bases
    I. Naming Acids
    A. Binary Acids
    1.
  231. catalyst
    substance that initiates or accelerates a chemical reaction
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  232. strontium
    a soft silver-white or yellowish metallic element of the alkali metal group; turns yellow in air; occurs in celestite and strontianite
    Most sulfates are soluble, except those of barium, strontium, and lead
    5.
  233. magnetic field
    the lines of force surrounding a permanent magnet or a moving charged particle
    Could produce energy for human use if a way can be found to contain a fusion rxn (magnetic field?)
  234. metal
    a chemical element or alloy that is usually a shiny solid
    Metals, Nonmetals, and Metalloids
    A. Metals
    1.
  235. chemical change
    process determined by substances' composition and structure
    An equation that includes only those compounds and ions that undergo a chemical change in a
    reaction in an aqueous solution
    B. Writing a Net Ionic Equation
    1.
  236. semiconductor
    a substance as germanium or silicon whose electrical conductivity is intermediate between that of a metal and an insulator; its conductivity increases with temperature and in the presence of impurities
    Metalloids
    (1) Brittle solids with some metallic and some nonmetallic properties
    (2) Semiconductors
    c.
  237. polar
    of or existing within the Arctic or Antarctic Circles
    Lone pairs do not cause distortion when bond angles are 120° or greater 6
    Arrangement of Electron Pairs Around an Atom Yielding Minimum
    Repulsion
    # of Electron
    Pairs
    Shape Arrangement of Electron Pairs
    2 Linear

    3 Trigonal Planar
    4 Tetrahedral
    5 Trigonal bipyramidal

    6 Octahedral

    8.4 Polar Bonds and Molecules
    I. Bond Polarity
    A. Nonpolar Covalent Bond
    1.
  238. hydrogen atom
    an atom of hydrogen
    Add unshared pairs of electrons so that each hydrogen atom shares a pair of electrons and each
    other nonmetal is surrounded by eight electrons

    6.
  239. coefficient
    a constant number that serves as a measure of some property
    Balancing is done with coefficients - small whole numbers that appear in front of a formula
    2H2 + O2 Æ 2H2O
    D. Additional symbols used in Chemical equations
    Table 11.1 Symbols Used in Chemical Equations
    Symbol Explanation
    + Used to separate two reactants or products
    Æ "Yields," separates reactants from products
    ' Used in place of a single arrow to indicate a reversible reactions
    (s) Reactant or product in the solid state.
  240. unsaturated
    used of a compound (especially of carbon) containing atoms sharing more than one valence bond
    Unsaturated solutions
    a.
  241. chlorite
    a generally green or black mineral
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  242. oxidize
    enter into a combination with oxygen
    Equivalents of oxidizing and reducing agents
    a.
  243. fusion
    the act of melding or melting together
    Total atomic numbers and mass numbers must be equal on both sides
    Be He C n
    1
    0
    12
    6
    4
    2
    9
    4
    + → +
    25.3 Fission and Fusion of Atomic Nuclei
    I. Nuclear Fission
    A. Nuclear Fission
    1.
  244. acid
    a sour water-soluble compound with a pH of less than 7
    Second element ALWAYS gets a prefix, and an “-ide” ending
    Examples: N2O3 = dinitrogen trioxide
    CO = carbon monoxide, not monocarbon monoxide
    Numerical Prefixes
    Number 1 2 3 4 5 6 7 8 9 10
    Prefix mono di tri tetra penta hexa hepta octa nona deca
    9.4 Naming and Writing Formulas for Acids and Bases
    I. Naming Acids
    A. Binary Acids
    1.
  245. lattice
    an arrangement of points in a regular periodic pattern
    The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice
    III.
  246. periodic
    happening or recurring at regular intervals
    Periodic Table is in order of increasing atomic number
    B. Mass Number
    1.
  247. toluene
    a colorless flammable liquid obtained from petroleum or coal tar; used as a solvent for gums and lacquers and in high-octane fuels
    Nonpolar solvents include CCl4 and toluene (methyl benzene), C6H5CH3
    D. Liquid Solutes and Solvents
    1.
  248. carbon
    an abundant nonmetallic element in all organic compounds
    The amount of substance that contains as many particles are there are in exactly 12 grams of carbon-12
    2.
  249. electric current
    a flow of electricity through a conductor
    Some decomposition rxns are produced by an electric current
    2NaCl(s) Æ 2Na(s) + Cl2 (g)
    III.
  250. oxide
    any compound of oxygen with another element or a radical
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  251. deuterium
    an isotope of hydrogen which has one neutron
    Hydrogen as an example:

    Protium (hydrogen-1) Deuterium (hydrogen-2) Tritium (hydrogen-3)

    D. Designating Isotopes
    1.
  252. chain reaction
    a series of chemical reactions in which the product of one is a reactant in the next
    Small amounts of missing mass are converted to HUGE amounts of energy (E = mc
    2
    )
    B. Nuclear Chain Reaction
    1.
  253. insoluble
    incapable of being dissolved
    No compound is completely insoluble
    2.
  254. visible light
    (physics) electromagnetic radiation that can produce a visual sensation
    Many types of EM waves
    a. visible light
    b. x-rays
    c. ultraviolet light
    d. infrared light
    e. radio waves
    2.
  255. molecular weight
    (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
    Calculations
    a. (empirical formula wt.)x = molecular weight
    b. (empirical formula)x = molecular formula
    Example : (empirical formula = HO molecular wt.
  256. erg
    a cgs unit of work or energy
    E = hν (h is Planck’s constant, 6.62554 x 10
    -27
    erg sec)
    10
    -12
    10
    -10
    10
    -8
    4 to 7x10
    -7
    10
    -4
    10
    -2
    1 10
    2
    10
    4
    Wavelength increases
    Frequency decreases
    Energy decreases
    II.
  257. tritium
    a radioactive isotope of hydrogen
    Hydrogen as an example:

    Protium (hydrogen-1) Deuterium (hydrogen-2) Tritium (hydrogen-3)

    D. Designating Isotopes
    1.
  258. CO2
    a colorless, odorless greenhouse gas essential for photosynthesis
    Nonmetals react with oxygen to form oxides
    C(s) + O2(g) Æ CO2(g)
    4.
  259. gamma
    the 3rd letter of the Greek alphabet
    Protection requires shielding with thick layers of lead, cement, or both
    C. Penetrating ability of radiation
    Increasing penetrating ability Æ
    ALPHA BETA GAMMA
    Least harmful most harmful
    C. Radioactive Elements
    1.
  260. sucrose
    a complex carbohydrate found in many plants and used as a sweetening agent
    Ice and sucrose are examples
    3.
  261. chloride
    any compound containing a chlorine atom
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  262. dilute
    lessen the strength or flavor of a solution or mixture
    Parts per million (ppm), is a ratio of parts of solute to one million parts of solution, and is usually applied to very dilute
    solutions.
  263. dissociate
    break away from; stop having a relationship with
    Ionic bases dissociate to some extent when placed in water
    ( ) ( ) ( )
    2
    NaOH s Na aq OH aq
    H O + −
     → +
    2.
  264. absolute value
    a real number regardless of its sign
    Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other
    ion
    3.
  265. alpha
    the 1st letter of the Greek alphabet
    Alpha particles (helium nuclei) fired at a thin sheet of gold
    a.
  266. phosphorous
    containing or characteristic of phosphorus
    SF6 is an example
    Question: Why doesn't carbon undergo dsp
    3
    or d
    2
    sp
    3
    hybridization, while phosphorous
    and sulfur do undergo this type of hybridization?
  267. calibration
    the act of checking or adjusting (by comparison with a standard) the accuracy of a measuring instrument
    Caused by poor measurement calibration
    1) gun sight set too high/low
    2) balance improperly zeroed
    3) thermometer improperly marked3
    1.5 Significant Figures and Calculations
    A. Rules for Counting Significant Figures
    Number Rule Example
    Nonzero integers Always significant 6.34 m (3 sig figs)
    Leading zeroes Never significant 0.00634 m ( 3 sig figs)
    Captive zeroes Always significant 6.0034 (5 sig figs)
    Trailing zeroes Significant if after a decimal 63400 (3 sig figs)
    0.63400 (5 sig figs)...
  268. electric field
    a field of force surrounding a charged particle
    Molecules with preferential orientation in an electric field
    + + +
    - - - 1
    Unit 4 – Conservation of Mass and Stoichiometry
    9.1 Naming Ions
    I. Monatomic Ions
    A. Monatomic ions
    1.
  269. alloy
    a mixture containing two or more metallic elements
    Metallic bonding is the same in all directions, so metals tend not to be brittle
    E. Metals atoms organized in compact, orderly crystalline patterns
    F. Different metallic elements (and carbon) can be mixed to form alloys
    1.
  270. ultraviolet light
    radiation lying in the ultraviolet range
    Many types of EM waves
    a. visible light
    b. x-rays
    c. ultraviolet light
    d. infrared light
    e. radio waves
    2.
  271. radiation
    the act of spreading outward from a central source
    Molar mass of an element equals the average atomic mass in gram units
    25.1 Nuclear Radiation
    I. Introduction
    A. Nucleons
    1.
  272. gelatin
    a sticky, colorless protein obtained from animal tissue
    Light is scattered in a colloid
    Types of Colloids
    Examples
    Dispersing
    Medium
    Dispersed
    Substance
    Colloid Type
    Fog, aerosol sprays Gas Liquid Aerosol
    Smoke, airborne bacteria Gas Solid Aerosol
    Whipped cream, soap suds Liquid Gas Foam
    Milk, mayonnaise Liquid Liquid Emulsion
    Paint, clays, gelatin Liquid Solid Sol
    Marshmallow, polystyrene foam Solid Gas Solid foam
    Butter, cheese Solid Liquid Solid emulsion
    Ruby glass Solid Solid Solid sol
    16.1 Properties of Solutions
    I. F...
  273. critical point
    a crisis situation or point in time when a critical decision must be made
    For water, the critical pressure is 217.75 atm
    E. Critical Point
    1.
  274. dispersion
    spreading widely or driving off
    Colloids
    A. Colloidal Dispersions (Colloids)
    1.
  275. cathode
    a negatively charged electrode that is the source of electrons entering an electrical device
    Cathode ray tube produces a ray with a constant charge to mass ratio
    b.
  276. reversible
    capable of being returned to the original condition
    Balancing is done with coefficients - small whole numbers that appear in front of a formula
    2H2 + O2 Æ 2H2O
    D. Additional symbols used in Chemical equations
    Table 11.1 Symbols Used in Chemical Equations
    Symbol Explanation
    + Used to separate two reactants or products
    Æ "Yields," separates reactants from products
    ' Used in place of a single arrow to indicate a reversible reactions
    (s) Reactant or product in the solid state.
  277. ammonium
    an ion of nitrogen and hydrogen found in many salts and fertilizers
    Most sodium, potassium, and ammonium compounds are soluble in water.
  278. diffraction
    process by which light changes passing through a narrow slit
    Structure of crystalline solids can be determined by xray diffraction
    a. waves in parallel beams that are "in phase" produce constructive
    interference
    b. waves in parallel beams that are "out of phase" produce destructive
    interference
    q = angle of incidence and reflection
    d = distance between atoms
    n = integer
    l = wavelength
    2.
  279. thermodynamics
    physics concerned with heat and other forms of energy
    Bases are proton acceptors in solution

    1
    m T
    q
    cp
    ⋅
    ∆
    = q =
    cp
    ⋅ m ⋅
    ∆ T
    Unit 7 – Kinetics and Thermodynamics
    17-1 Thermochemistry
    Thermochemistry - The study of the changes in heat energy that accompany chemical reactions and physical changes
    I. Heat and Temperature
    A. Calorimeter
    1.
  280. hydrate
    any compound that contains water of crystallization
    The percentage by mass of each element in a compound
    x element in compound
    molar mass of compound
    Mass of element in mol of compound
    100 %
    1
    =
    B. Hydrates
    1.
  281. barium
    a soft silvery metallic element of the alkali earth group
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  282. ethylene
    a flammable colorless gaseous alkene
    Trigonal planar structure, 120° angle, in ethene
    (ethylene) rules out sp
    3
    hybridization
    2. sp
    2
    hybridization creates 3 identical orbitals of
    intermediate energy and length and leaves one
    unhybridized p orbital
    3.
  283. latent heat
    heat absorbed or radiated during a change of phase at a constant temperature and pressure
    Specific Heat(cp)
    2. q = heat m = mass ∆T = change in temperature (in Celsius or Kelvin)



    12.3 Latent Heat of Phase Change
    I. Boiling and Condensation
    A. Molar Heat of Vaporization
    1.
  284. monoxide
    an oxide containing just one atom of oxygen in the molecule
    Second element ALWAYS gets a prefix, and an “-ide” ending
    Examples: N2O3 = dinitrogen trioxide
    CO = carbon monoxide, not monocarbon monoxide
    Numerical Prefixes
    Number 1 2 3 4 5 6 7 8 9 10
    Prefix mono di tri tetra penta hexa hepta octa nona deca
    9.4 Naming and Writing Formulas for Acids and Bases
    I. Naming Acids
    A. Binary Acids
    1.
  285. lithium
    a soft silver-white univalent element of the alkali metal group; the lightest metal known; occurs in several minerals
    The number of electrons in a sublevel is indicated by adding a superscript to the sublevel
    designation
    Hydrogen = 1s
    1
    Helium = 1s
    2
    Lithium = 1s
    2
    2s
    1
    D. Exceptional Electron Configurations
    1.
  286. radius
    a straight line from the center to the perimeter of a circle
    Sizes of Atoms
    A. Atomic radius
    1.
  287. helium
    a light colorless element that is one of the six inert gases
    Alpha particles (helium nuclei) fired at a thin sheet of gold
    a.
  288. sigma
    the 18th letter of the Greek alphabet
    Sigma bonds (s bond)
    a.
  289. nitrite
    the radical -NO2 or any compound containing it
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  290. sodium
    a silvery soft waxy metallic element of the alkali metal group; occurs abundantly in natural compounds (especially in salt water); burns with a yellow flame and reacts violently in water; occurs in sea water and in the mineral halite (rock salt)
    Formation of a sodium ion
    Na = 1s
    2
    2s
    2
    2p
    6
    3s
    1
    Æ Na
    +
    = 1s
    2
    2s
    2
    2p
    6
    3.
  291. citric acid
    a weak water-soluble acid found in many fruits
    Citric acid - in citrus fruit
    d.
  292. decomposition
    the organic phenomenon of rotting
    Decomposition Reactions
    A. Decomposition Rxns
    1.
  293. interstitial
    of or relating to small spaces between things
    Interstitial alloys
    a.
  294. oxygen
    a colorless, odorless gas that is essential for respiration
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  295. silica
    a white or colorless vitreous insoluble solid
    Delocalized electrons make graphite an electrical conductor
    D. Silica
    1.
  296. hydrogen bomb
    a nuclear weapon that releases atomic energy by union of light (hydrogen) nuclei at high temperatures to form helium
    Source of energy of the hydrogen bomb
    3.
  297. repulsion
    the act of successfully defending against an attack
    Greater electron-electron repulsion
    C. Trends
    1.
  298. polarity
    a relation between two opposite attributes or tendencies
    Lone pairs do not cause distortion when bond angles are 120° or greater 6
    Arrangement of Electron Pairs Around an Atom Yielding Minimum
    Repulsion
    # of Electron
    Pairs
    Shape Arrangement of Electron Pairs
    2 Linear

    3 Trigonal Planar
    4 Tetrahedral
    5 Trigonal bipyramidal

    6 Octahedral

    8.4 Polar Bonds and Molecules
    I. Bond Polarity
    A. Nonpolar Covalent Bond
    1.
  299. component
    one of the individual parts making up a larger entity
    The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component
    gases
    ...
  300. diffusion
    the act of dispersing something
    Graham’s Law
    A. Diffusion
    1.
  301. silicon
    a tetravalent nonmetallic element
    10.5 Carbon and Silicon: Network Atomic Solids
    A. Network Solids
    1.
  302. condensation
    process of changing from a gas to a liquid or solid state
    Obsidian
    13.4 Changes of State
    I. Boiling and Condensation
    A. Boiling
    1.
  303. interaction
    mutual or reciprocal dealings or influence
    Maximizes (+) ----- ( - ) interactions
    b.
  304. boron
    a trivalent metalloid element
    "Dope" silicon with elements such as boron
    (1) shortage of valence electrons creates a "hole" that electrons fill
    as they move (conduct)
    10.6 Molecular Solids
    A. Examples
    1.
  305. acetate
    a fabric made from fibers of cellulose acetate
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  306. graphite
    a soft, dark gray mineral made of carbon
    Bonds formed by overlap of hybridized sp
    3
    orbitals
    C. Graphite
    1.
  307. crystallization
    the formation of crystals
    The physical state in which the opposing processes of dissolution and crystallization of a solute occur
    at equal rates
    B. Saturation Levels
    1.
  308. potential energy
    energy stored by a body or system by virtue of its position
    A state in which an atom has a higher potential energy than in its ground state
    C. Bright line spectrum
    1.
  309. lactic acid
    a clear odorless hygroscopic syrupy carboxylic acid found in sour milk and in many fruits
    Lactic acid - in sour milk
    c.
  310. meniscus
    a lens that is concave on one side and convex on the other
    Water's adhesive forces are greater than its cohesive forces, thus
    the increase in surface area (concave meniscus)
    b.
  311. citric
    of or related to citric acid
    Citric acid - in citrus fruit
    d.
  312. angle of incidence
    the angle that a line makes with a line perpendicular to the surface at the point of incidence
    Structure of crystalline solids can be determined by xray diffraction
    a. waves in parallel beams that are "in phase" produce constructive
    interference
    b. waves in parallel beams that are "out of phase" produce destructive
    interference
    q = angle of incidence and reflection
    d = distance between atoms
    n = integer
    l = wavelength
    2.
  313. dioxide
    an oxide containing two atoms of oxygen in the molecule
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2 Formul...
  314. fluorine
    a nonmetallic univalent element belonging to the halogens
    Example – Diatomic fluorine
    F
    1s 2s 2p

    F
    1s 2s 2p
    b.
  315. heterogeneous
    consisting of elements not of the same kind or nature
    Lamp does not glow, ammeter may not register a current at all 5
    15.3 Heterogeneous Aqueous Systems
    I. Suspensions
    A. A mixture from which particles settle out upon standing
    II.
  316. carbon dioxide
    a colorless, odorless greenhouse gas essential for photosynthesis
    Metallic carbonates, when heated, form metallic oxides and carbon dioxide
    CaCO3(s) Æ CaO(s) + CO2(g)
    2.
  317. micro
    extremely small in scale or scope or capability
    Some properties of metals, some of nonmetals
    gamma xrays UV visible IR micro Radio waves
    FM short AM 6.2 Classifying the Elements
    I. Periods and the Blocks of the Periodic Table
    A. Periods
    1.
  318. critical mass
    the minimum amount required to start or maintain a venture
    A reaction in which the material that starts the reaction is also one of the products and can start another
    reaction
    C. Critical Mass
    1.
  319. directional
    relating to or indicating directions in space
    Atomic solids with strong directional covalent bonds
    B. Diamond
    1.
  320. calorimeter
    a measuring instrument that determines quantities of heat
    Bases are proton acceptors in solution

    1
    m T
    q
    cp
    ⋅
    ∆
    = q =
    cp
    ⋅ m ⋅
    ∆ T
    Unit 7 – Kinetics and Thermodynamics
    17-1 Thermochemistry
    Thermochemistry - The study of the changes in heat energy that accompany chemical reactions and physical changes
    I. Heat and Temperature
    A. Calorimeter
    1.
  321. effusion
    an unrestrained expression of emotion
    Rate of diffusion is dependent upon:
    a. speed of particles
    b. diameter of particles
    c. attractive forces between the particles
    B. Effusion
    1.
  322. Planck
    German physicist whose explanation of blackbody radiation in the context of quantized energy emissions initiated quantum theory (1858-1947)
    E = hν (h is Planck’s constant, 6.62554 x 10
    -27
    erg sec)
    10
    -12
    10
    -10
    10
    -8
    4 to 7x10
    -7
    10
    -4
    10
    -2
    1 10
    2
    10
    4
    Wavelength increases
    Frequency decreases
    Energy decreases
    II.
  323. activate
    put in motion
    Activation Energy and the Activated Complex
    A. Activated Complex
    1.
  324. capillary
    a minute blood vessel connecting arterioles with venules
    Capillary Action
    a.
  325. conduction
    the transmission of heat or electricity or sound
    Molecular orbitals occupied by conducting electrons are called
    conduction bands
    C. Metal Alloys
    1.
  326. carbonate
    treat with carbon dioxide
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  327. Pauli
    United States physicist who proposed the exclusion principle
    Pauli Exclusion Principle
    a.
  328. potassium
    a light soft silver-white metallic element of the alkali metal group; oxidizes rapidly in air and reacts violently with water; is abundant in nature in combined forms occurring in sea water and in carnallite and kainite and sylvite
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  329. linear
    involving a single dimension
    Lone pairs do not cause distortion when bond angles are 120° or greater 6
    Arrangement of Electron Pairs Around an Atom Yielding Minimum
    Repulsion
    # of Electron
    Pairs
    Shape Arrangement of Electron Pairs
    2 Linear

    3 Trigonal Planar
    4 Tetrahedral
    5 Trigonal bipyramidal

    6 Octahedral

    8.4 Polar Bonds and Molecules
    I. Bond Polarity
    A. Nonpolar Covalent Bond
    1.
  330. transmutation
    an act that changes the form or character or substance of something
    Transmutation Reactions
    A. Transmutations
    1.
  331. fluoride
    a chemical used to help prevent tooth decay
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  332. methane
    a colorless, odorless gas used as a fuel
    Orbitals of equal energy produced by the combination of two or more
    orbitals on the same atom
    C. Evidence for hybridization of carbon - Methane and sp
    3
    1.
  333. baking soda
    a white soluble compound (NaHCO3) used in effervescent drinks and in baking powders and as an antacid
    I look around my kitchen (I have a BIG kitchen!) and find 40 lbs. of
    butter, two lbs. of salt, 1 gallon of vanilla extract, 80 lbs. of chocolate chips, 200 lbs. of flour, 150 lbs. of sugar,
    150 lbs. of brown sugar, ten lbs. of baking soda and TWO eggs.
  334. nuclear
    constituting the core or central part
    Most of the atomic radius is due to the electron cloud
    B. Nuclear radius
    1.
  335. atmospheric
    relating to or located in the mass of air surrounding Earth
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  336. acid rain
    precipitation with toxic gas emissions combined with water
    Nonmetal oxides react with water to form oxyacids (acid rain)
    SO2(g) + H2O Æ H2SO3(aq)
    II.
  337. glucose
    a monosaccharide sugar that has several forms
    The sum of the average atomic masses of all the atoms represented in the formula of a molecule,
    formula unit, or ion
    Formula Mass of glucose, C6H12O6 :
    C = 12.01 amu 6 x 12.01 amu = 72.06 amu
    H = 1.01 amu 12 x 1.01 amu = 12.12 amu
    O = 16.00 amu 6 x 16.00 amu = 96.00 amu
    Formula Mass = 180.18 amu
    B. Molar Masses
    1.
  338. mercury
    a heavy silvery toxic univalent and bivalent metallic element; the only metal that is liquid at ordinary temperatures
    Solids (except mercury)
    4.
  339. dialysis
    separation of mixed substances using a special filter
    T is the Kelvin temperature
    C. Dialysis
    1.
  340. Death Valley
    a desert area that is part of the Mojave Desert in eastern California and southwestern Nevada; contains the lowest point in North America
    Washington, N.H. 6,293 590 93
    Boulder, Colorado 5,430 610 94
    Madison, Wisconsin 900 730 99
    New York City, New York 10 760 100
    Death Valley, California -282 770 100.3
    1
    Chapter 9 - Covalent Bonding: Orbitals
    9.1 Hybridization and the Localized Electron Model
    A. Hybridization
    1.
  341. carbon monoxide
    an odorless very poisonous gas that is a product of incomplete combustion of carbon
    Second element ALWAYS gets a prefix, and an “-ide” ending
    Examples: N2O3 = dinitrogen trioxide
    CO = carbon monoxide, not monocarbon monoxide
    Numerical Prefixes
    Number 1 2 3 4 5 6 7 8 9 10
    Prefix mono di tri tetra penta hexa hepta octa nona deca
    9.4 Naming and Writing Formulas for Acids and Bases
    I. Naming Acids
    A. Binary Acids
    1.
  342. hydrocarbon
    an organic compound containing only carbon and hydrogen
    A substance combines with oxygen, releasing a large amount of energy in the form of light and heat
    2H2(g) + O2(g) Æ 2H2O(g)
    B. Hydrocarbon combustion always produces carbon dioxide and water
    2C2H6(g) + 7O2(g) Æ 4CO2(g) + 6H2O(g)
    11.3 Reactions in Aqueous Solution
    I. Dissociation
    A. Dissociation
    1.
  343. beta
    the second letter of the Greek alphabet
    Protection requires shielding with thick layers of lead, cement, or both
    C. Penetrating ability of radiation
    Increasing penetrating ability Æ
    ALPHA BETA GAMMA
    Least harmful most harmful
    C. Radioactive Elements
    1.
  344. methyl
    the univalent radical CH3- derived from methane
    Nonpolar solvents include CCl4 and toluene (methyl benzene), C6H5CH3
    D. Liquid Solutes and Solvents
    1.
  345. crystallize
    cause to form crystals or assume crystalline form
    Not all metals crystallize in closest packing
    B. Bonding Models for Metals
    1.
  346. sea level
    level of the ocean's surface
    Gas molecules exert force,
    and therefore pressure, on
    any surface with which they
    collide
    B. Units of Pressure
    Units of Pressure
    Unit Symbol Definition/Relationship
    Pascal Pa SI pressure unit
    1 Pa =
    2
    1
    m
    N
    Millimeter of mercury mm Hg Pressure that supports a 1 mm column of mercury in a
    barometer
    Atmosphere atm Average atmospheric pressure at sea level and 0 °C
    Torr torr 1 torr = 1 mm Hg
    C. Standard Pressure
    1.
  347. radioactivity
    the discharge of particles or rays in nuclear decay
    Radioactivity
    A. Radioactive Decay
    1.
  348. alkaline
    relating to or containing an alkali
    Group 2 - The alkaline earth metals
    a.
  349. incidence
    the relative frequency of occurrence of something
    Structure of crystalline solids can be determined by xray diffraction
    a. waves in parallel beams that are "in phase" produce constructive
    interference
    b. waves in parallel beams that are "out of phase" produce destructive
    interference
    q = angle of incidence and reflection
    d = distance between atoms
    n = integer
    l = wavelength
    2.
  350. saturated
    unable to dissolve still more of a substance
    Saturated solution
    a.
  351. hybrid
    the offspring of genetically dissimilar parents or stock
    The mixing of two or more atomic orbitals of similar energies on the
    same atom to produce new orbitals of equal energies
    B. Hybrid Orbitals
    1.
  352. spectroscope
    an optical instrument for spectrographic analysis
    A spectroscope reveals lines of particular colors
    410nm 434nm 486nm 656nm
    a.
  353. infrared
    having or employing wavelengths longer than light but shorter than radio waves; lying outside the visible spectrum at its red end
    Many types of EM waves
    a. visible light
    b. x-rays
    c. ultraviolet light
    d. infrared light
    e. radio waves
    2.
  354. inhalation
    the act of drawing in air or other gases
    Can cause harm through ingestion or inhalation
    2.Beta
  355. mono
    an acute disease characterized by fever and swollen lymph nodes and an abnormal increase of mononuclear leucocytes or monocytes in the bloodstream; not highly contagious; some believe it can be transmitted by kissing
    Second element ALWAYS gets a prefix, and an “-ide” ending
    Examples: N2O3 = dinitrogen trioxide
    CO = carbon monoxide, not monocarbon monoxide
    Numerical Prefixes
    Number 1 2 3 4 5 6 7 8 9 10
    Prefix mono di tri tetra penta hexa hepta octa nona deca
    9.4 Naming and Writing Formulas for Acids and Bases
    I. Naming Acids
    A. Binary Acids
    1.
  356. scientific method
    a systematic way of investigating to test a hypothesis
    Scientific Method
    A. General Framework
    1.
  357. combustion
    a reaction of a substance with oxygen to give heat and light
    Formation of Water
    NaOH(aq) + HCl(aq) Æ NaCl(aq) + H2O(l)
    V. Combustion Reactions
    A. Combustion Rxns
    1.
  358. ultraviolet
    having wavelengths shorter than light but longer than X-rays
    Many types of EM waves
    a. visible light
    b. x-rays
    c. ultraviolet light
    d. infrared light
    e. radio waves
    2.
  359. bismuth
    a heavy brittle diamagnetic trivalent metallic element
    All isotopes of all elements beyond bismuth (atomic #83) are radioactive Unit 2 - Electrons and Periodic Behavior
    5.1 Models of the Atom
    I. The Bohr Model of the Atom
    A. Electron Orbits, or Energy Levels
    1.
  360. metric
    based on a decimal unit of measurement
    0.001 pm
    2. density is 2x10
    8
    metric tons/cm
    3
    a.
  361. ceramic
    an artifact made of clay baked at a high temperature
    Other compounds added to molten silica prior to cooling produce
    glass with varying properties (see table 10.5)
    E. Ceramics
    1.
  362. iodide
    a salt or ester of hydriodic acid
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  363. molten
    reduced to liquid form by heating
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  364. bromide
    a trite or obvious remark
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  365. titanium
    a light strong grey lustrous corrosion-resistant metallic element used in strong lightweight alloys (as for airplane parts); the main sources are rutile and ilmenite
    Everyone knows that REAL
    racing bikes are made out of TITANIUM!
  366. phosphate
    a salt of phosphoric acid
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  367. ethanol
    colorless flammable liquid used as a solvent or intoxicant
    Water and ethanol (both polar)
    E. Effects of Pressure on Solubility
    1.
  368. saturation
    the process of totally infusing something with a substance
    The physical state in which the opposing processes of dissolution and crystallization of a solute occur
    at equal rates
    B. Saturation Levels
    1.
  369. indicator
    a device for showing the operating condition of some system
    Acids change the color of acid-base indicators
    3.
  370. chromium
    a hard brittle multivalent metallic element
    Irregularity of Chromium
    a.
  371. magnetic
    of or relating to or caused by attraction for iron
    Could produce energy for human use if a way can be found to contain a fusion rxn (magnetic field?)
  372. nitrate
    any compound containing the nitrate group
    Polyatomic anions that contain oxygen
    Formula Name
    NO2
    -
    Nitrite
    NO3
    -
    Nitrate
    SO3
    2-
    Sulfite
    SO4
    2-
    Sulfate
    OH
    -
    Hydroxide
    PO4
    3-
    Phosphate
    CO3
    2-
    Carbonate
    ClO3
    -
    Chlorate
    C2H3O2
    -
    Acetate
    B. Naming a series of similar polyatomic ions
    ClO
    -
    ClO2
    -
    ClO3
    -
    ClO4
    -
    Hypochlorite Chlorite Chlorate Perchlorate 2
    9.2 Naming and Writing Formulas for Ionic Compounds
    I. Binary Ionic Compounds
    ...
  373. acetic acid
    a colorless pungent liquid widely used in manufacturing plastics and pharmaceuticals
    Acetic acid - in vinegar
    II.
  374. vitamin
    an organic substance essential to normal metabolism
    Water soluble vitamins
    2.
  375. plutonium
    a solid silvery grey radioactive transuranic element whose atoms can be split when bombarded with neutrons; found in minute quantities in uranium ores but is usually synthesized in nuclear reactors; 13 isotopes are known with the most important being plutonium 239
    Plutonium (94) through Lawrencium (103) are man-made
    6.3 Periodic Trends
    I. Atomic Radii
    A. Atomic Radius
    1.
  376. synthesis
    the combination of ideas into a complex whole
    Balancing Chemical Equations
    A. Identify the names of reactants and products, and write a word equation
    B. Write a formula equation by substituting correct formulas for the names of the reactants and the products
    C. Balance the formula equation according to the law of conservation of atoms
    D. Count atoms to be sure that the equation is balanced 6
    11.2 Types of Chemical Reactions
    I. Combination Reactions (Synthesis Rxns)
    A. Two or more substances combine to form a more complex subs...
  377. diffuse
    spread out; not concentrated in one place
    The volume of liquids doesn't change appreciably when pressure is applied
    D. Liquids have the Ability to Diffuse
    1.
  378. calcium
    a white metallic element that burns with a brilliant light
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  379. meter
    a basic unit of length (approximately 1.094 yards)
    They have a range of a few meters in air.
  380. condense
    cause a gas or vapor to change into a liquid
    The amount of heat energy released when one mole of a vapor condenses to a liquid at its
    condensation point
    3.
  381. experimentally
    in an experimental fashion
    Actual effect of concentration change must be determined experimentally for each rxn
    E. Presence of Catalysts
    1.
  382. volatile
    liable to lead to sudden change or violence
    Volatile substances
    a.
  383. strong force
    (physics) the interaction that binds protons and neutrons together in the nuclei of atoms; mediated by gluons
    Solute and solvent are similar, with strong forces of attraction
    b.
  384. rotate
    turn on or around an axis or a center
    Diffractometer
    a. computerized device to rotate crystal samples in an x-ray field, gather
    incidence and reflection data, and construct models of crystal
    structure3
    C. Types of Crystalline Solids
    1.
  385. variable
    something that is likely to change
    The ideal gas law reduces to Boyle's, Charles's, or Gay-Lussac's Law if the necessary variable is held
    constant
    B. The Ideal Gas Constant
    1.
  386. X-ray
    electromagnetic radiation of short wavelength produced when high-speed electrons strike a solid target
    Components "frozen in place" and lacking orderly arrangement
    (1) glass
    (2) plastic
    B. X-ray Analysis of Solids
    1.
  387. chemically
    with respect to chemistry
    Atoms of the same element are chemically alike
    3.
  388. magnesium
    a light, malleable, silver-white metallic element
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  389. lobe
    a rounded projection that is part of a larger structure
    Lobes of bonding orbital point toward
    each other
    c.
  390. chemistry
    the science of matter
    This is the most widely used unit for concentration when
    preparing solutions in chemistry and biology.
  391. instantaneous
    occurring with no delay
    Instantaneous dipoles
    a.
  392. conservation
    careful management of the environment and natural resources
    Molecules with preferential orientation in an electric field
    + + +
    - - - 1
    Unit 4 – Conservation of Mass and Stoichiometry
    9.1 Naming Ions
    I. Monatomic Ions
    A. Monatomic ions
    1.
  393. indeterminate
    not fixed or known in advance
    Random Errors (indeterminate errors)
    a.
  394. unstable
    subject to change; variable
    Particles or electromagnetic radiation emitted from the nucleus during radioactive decay
    C. Unstable Nuclides
    1.
  395. orbit
    the path of a celestial body in its revolution about another
    All isotopes of all elements beyond bismuth (atomic #83) are radioactive Unit 2 - Electrons and Periodic Behavior
    5.1 Models of the Atom
    I. The Bohr Model of the Atom
    A. Electron Orbits, or Energy Levels
    1.
  396. radium
    an intensely radioactive metallic element that occurs in minute amounts in uranium ores
    Atoms identified by the number of protons and neutrons in the nucleus
    a. radium-228 or Ra
    228
    88
    II.
  397. theory
    a belief that can guide behavior
    Unit 1 – Atomic Structure
    4.1 Defining the Atom
    I. Atomic Theory
    A. Modern Atomic Theory
    1.
  398. citrus
    a tropical tree cultivated for its juicy edible fruits
    Citric acid - in citrus fruit
    d.
  399. orientation
    the act of determining one's position
    Molecules with preferential orientation in an electric field
    + + +
    - - - 1
    Unit 4 – Conservation of Mass and Stoichiometry
    9.1 Naming Ions
    I. Monatomic Ions
    A. Monatomic ions
    1.
  400. magnetism
    attraction for iron
    Magnetism can be induced in some nonmagnetic materials when in the
    presence of a magnetic field
    a.
  401. Fahrenheit
    of or relating to a temperature scale proposed by the inventor of the mercury thermometer
    Size of the temperature unit (degree) is the same
    B. Fahrenheit
    1.
  402. isolate
    place or set apart
    Four bonds of equal length and strength
    Carbon's isolated configuration Carbon's hybridized configuration
    2.
  403. resonance
    the characteristic of having a loud deep sound
    There is no universally accepted molecular orbital energy order
    9.5 Combining the Localized Electron and Molecular Orbital Models
    A. Resonance
    1.
  404. membrane
    a sheet of tissue that lines or connects organs or cells
    The flow of solvent molecules into a solution through a semipermeable
    membrane
    B. Osmotic Pressure
    1.
  405. distortion
    a shape resulting from being deformed
    Lone pairs do not cause distortion when bond angles are 120° or greater 6
    Arrangement of Electron Pairs Around an Atom Yielding Minimum
    Repulsion
    # of Electron
    Pairs
    Shape Arrangement of Electron Pairs
    2 Linear

    3 Trigonal Planar
    4 Tetrahedral
    5 Trigonal bipyramidal

    6 Octahedral

    8.4 Polar Bonds and Molecules
    I. Bond Polarity
    A. Nonpolar Covalent Bond
    1.
  406. spectrum
    a broad range of related objects, values, or qualities
    Atomic Spectra
    A. Ground State
    1.
  407. manganese
    a hard brittle grey polyvalent metallic element that resembles iron but is not magnetic; used in making steel; occurs in many minerals
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2 Formul...
  408. natural law
    a body of inherent rules governing human conduct in society
    Natural Law
    a.
  409. mechanism
    device consisting of a piece of machinery
    There is a tendency for the disorder of the system to increase
    17-3 The Reaction Process
    I. Reaction Mechanisms
    A. Reaction Mechanism
    1.
  410. displacement
    the act of moving something from its natural environment
    Pressure of the vapor present at equilibrium (also called equilibrium vapor
    pressure)
    ***remember vapor pressure corrections made in gas law problems
    involving water displacement
    2.
  411. bacteria
    single-celled organisms that can cause disease
    Light is scattered in a colloid
    Types of Colloids
    Examples
    Dispersing
    Medium
    Dispersed
    Substance
    Colloid Type
    Fog, aerosol sprays Gas Liquid Aerosol
    Smoke, airborne bacteria Gas Solid Aerosol
    Whipped cream, soap suds Liquid Gas Foam
    Milk, mayonnaise Liquid Liquid Emulsion
    Paint, clays, gelatin Liquid Solid Sol
    Marshmallow, polystyrene foam Solid Gas Solid foam
    Butter, cheese Solid Liquid Solid emulsion
    Ruby glass Solid Solid Solid sol
    16.1 Properties of Solutions
    I. F...
  412. disintegration
    separation into component parts
    The spontaneous disintegration of a nucleus into a slightly lighter and more stable nucleus, accompanied
    by emission of particles, electromagnetic radiation, or both
    B. Nuclear Radiation
    1.
  413. concave
    curving inward
    Water's adhesive forces are greater than its cohesive forces, thus
    the increase in surface area (concave meniscus)
    b.
  414. alkali
    any of various water-soluble compounds capable of turning litmus blue and reacting with an acid to form a salt and water
    Group 1 - The alkali metals
    a.
  415. electric
    using or providing the flow of charge through a conductor
    Molecules with preferential orientation in an electric field
    + + +
    - - - 1
    Unit 4 – Conservation of Mass and Stoichiometry
    9.1 Naming Ions
    I. Monatomic Ions
    A. Monatomic ions
    1.
  416. cell
    the basic structural and functional unit of all organisms
    The total three dimensional arrangement of particles of a crystal
    B. Unit Cell
    1.
  417. precipitation
    the falling to earth of any form of water
    Most sulfides are insoluble, except those of calcium, strontium, sodium, potassium, and
    ammonium
    B. Precipitation Reactions
    1.
  418. arsenic
    a very poisonous metallic element
    "Dope" silicon with elements such as arsenic
    (1) extra valence electron increases conductivity
    3. p-type semiconductors
    a.
  419. solar system
    the sun with the celestial bodies that revolve around it
    There is 1 star at the
    center of our solar system.
  420. electricity
    a physical phenomenon that can produce light, heat and power
    Good conductors of heat and electricity
    2.
  421. vanilla
    any of numerous climbing plants having fleshy leaves
    I look around my kitchen (I have a BIG kitchen!) and find 40 lbs. of
    butter, two lbs. of salt, 1 gallon of vanilla extract, 80 lbs. of chocolate chips, 200 lbs. of flour, 150 lbs. of sugar,
    150 lbs. of brown sugar, ten lbs. of baking soda and TWO eggs.
  422. atmosphere
    the envelope of gases surrounding any celestial body
    Standard Pressure = 101.3 kPa or 1 atmosphere
    B. Standard Molar Volume
    1.
  423. physical
    involving the body as distinguished from the mind or spirit
    Definite wavelength
    6.1 Organizing the Elements
    I. The Periodic Law
    A. The physical and chemical properties of the elements are periodic functions of their atomic numbers
    B. Elements on the table are arranged in order of increasing atomic number (number of protons)
    II.
  424. barometer
    an instrument that measures atmospheric pressure
    Gas molecules exert force,
    and therefore pressure, on
    any surface with which they
    collide
    B. Units of Pressure
    Units of Pressure
    Unit Symbol Definition/Relationship
    Pascal Pa SI pressure unit
    1 Pa =
    2
    1
    m
    N
    Millimeter of mercury mm Hg Pressure that supports a 1 mm column of mercury in a
    barometer
    Atmosphere atm Average atmospheric pressure at sea level and 0 °C
    Torr torr 1 torr = 1 mm Hg
    C. Standard Pressure
    1.
  425. electrical
    relating to or concerned with electricity
    Cu = 60%, Zn = 40%
    Ionic Compounds
    Structure Crystalline solids
    Melting point Generally high
    Boiling Point Generally high
    Electrical Conductivity Excellent conductors, molten and aqueous
    Solubility in water Generally soluble 3
    8.1 Molecular Compounds
    I. Important Definitions
    A. Molecule
    1.
  426. elevate
    raise from a lower to a higher position
    Nonvolatile solutes elevate the boiling point of the solvent
    DT = Kbmsolut e
    a.
  427. DNA
    material that carries genetic information in a cell
    Important in the bonding of molecules such as water and DNA
    C. London Dispersion Forces
    1.
  428. platinum
    a heavy precious metallic element
    Also a precipitate
    (l) Reactant or product in the liquid state.
    (aq) Reactant or product in an aqueous solution (dissolved in water)
    (g) Reactant or product in the gaseous state
    ∆ Reactants are heated
    Pt A formula written above or below the yield sign indicates its use as a
    catalyst (in this case, platinum)
    Pressure Pressure at which rxn is carried out exceeds normal atmospheric pressure
    25 °C Temperature at which the rxn is carried out, in this case 25 °C
    MnO2...
  429. biology
    the science that studies living organisms
    This is the most widely used unit for concentration when
    preparing solutions in chemistry and biology.
  430. aluminum
    a silvery, flexible, metallic element
    Formation of chloride ion
    Cl = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    5
    Æ Cl
    -
    = 1s
    2
    2s
    2
    2p
    6
    3s
    2
    3p
    6

    Common Ions and Their Charges
    Monatomic Cations Name Monatomic Anions Name
    H
    +
    Hydrogen F
    -
    Fluoride
    Li
    +
    Lithium Cl
    -
    Chloride
    Na
    +
    Sodium Br
    -
    Bromide
    K
    +
    Potassium I
    -
    Iodide
    Mg
    2+
    Magnesium O
    2-
    Oxide
    Ca
    2+
    Calcium S
    2-
    Sulfide
    Ba
    2+
    Barium N
    3-
    Nitride
    Al
    3+
    Aluminum P
    3-
    Phosphide 2
    7.2 Ionic Bonds and Ionic Compounds
    I. Introduction
    A...
  431. latent
    potentially existing but not presently evident or realized
    Specific Heat(cp)
    2. q = heat m = mass ∆T = change in temperature (in Celsius or Kelvin)



    12.3 Latent Heat of Phase Change
    I. Boiling and Condensation
    A. Molar Heat of Vaporization
    1.
  432. elastic
    capable of resuming shape after stretching or compression
    Gas particles undergo elastic collisions
    a.
  433. thermometer
    measuring instrument for measuring temperature
    Caused by poor measurement calibration
    1) gun sight set too high/low
    2) balance improperly zeroed
    3) thermometer improperly marked3
    1.5 Significant Figures and Calculations
    A. Rules for Counting Significant Figures
    Number Rule Example
    Nonzero integers Always significant 6.34 m (3 sig figs)
    Leading zeroes Never significant 0.00634 m ( 3 sig figs)
    Captive zeroes Always significant 6.0034 (5 sig figs)
    Trailing zeroes Significant if after a decimal 63400 (3 sig figs)
    0.63400 (5 sig figs)...
  434. physics
    the science of matter and energy and their interactions
    Numerous transition and rare-earth elements transfer electrons from smaller sublevels in order
    to half-fill, or fill, larger sublevels
    5.3 Physics and the Quantum Mechanical Model
    I. Properties of Light
    A. Electromagnetic Radiation
    1.
  435. mechanical
    using tools or devices
    The Quantum Mechanical Model
    A. Probability and the Electron
    1.
  436. experimental
    of the nature of or undergoing a trial
    Molar mass of a solute can be calculated from experimental results for vapor
    pressure lowering
    C. Ionic solutes
    1.
  437. analysis
    abstract separation of something into its various parts
    1.6 Dimensional Analysis
    A. Examine examples
    1. pages 18 - 21
    B. Unit Conversions Questions
    1.
  438. copper
    a ductile malleable reddish-brown corrosion-resistant diamagnetic metallic element; occurs in various minerals but is the only metal that occurs abundantly in large masses; used as an electrical and thermal conductor
    Irregularity of Copper
    c.
  439. skeleton
    the structure providing a frame for the body of an animal
    Arrange the atoms to form a skeleton structure for the molecule.
  440. precision
    the quality of being exact
    The agreement of a particular value with the accepted value
    C. Precision
    1.
  441. fluid
    continuous amorphous matter that tends to flow
    Rate of effusion is dependent upon:
    a. speed of particles (small molecules have greater speed than large molecules at the same
    temperature, so the effuse more rapidly)
    C. Graham’s Mathematical Law

    Molar Mass of Gas A
    Molar Mass of Gas B
    rate of effusion of B
    rate of effusion of A


    1
    Unit 6 – Solids, Liquids and Solutions
    13.2 The Nature of Liquids
    I. A Model for Liquids
    A. Liquids are Fluids
    1.
  442. petroleum
    a dark oil consisting mainly of hydrocarbons
    Fats, oils and many petroleum products are soluble in nonpolar solvents
    3.
  443. solar
    relating to the sun or utilizing the energies of the sun
    There is 1 star at the
    center of our solar system.
Created on Sun Jan 22 20:03:32 EST 2012

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