che 200 ch1

Anisa T. (United States of America)
221 words 1 learner

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  1. electronegative
    having a negative charge
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  2. nonpolar
    not ionic
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  3. electronegativity
    (chemistry) the tendency of an atom or radical to attract electrons in the formation of an ionic bond
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  4. covalent bond
    a chemical bond that involves sharing a pair of electrons between atoms in a molecule
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  5. covalent
    of or relating to or characterized by covalence
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  6. hybridize
    breed animals or plants using parents of different races and varieties
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  7. hybridization
    (genetics) the act of mixing different species or varieties of animals or plants and thus to produce hybrids
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  8. valence electron
    an electron in the outer shell of an atom which can combine with other atoms to form molecules
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  9. chemical bond
    an electrical force linking atoms
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  10. double bond
    a covalent bond in which two pairs of electrons are shared between two atoms
    VSEPR Model
    Predict the shape of formaldehyde, CH2O
    The Lewis structure shows carbon surrounded by three regions of electron density; two regions contain single pairs of electrons and the third contains two pairs of electrons forming the double bond to oxygen.
  11. planar
    involving two dimensions
    According to the VSEPR model, the three regions radiate from carbon at angles of 120°, and the shape of the molecule is planar (trigonal planar).
  12. trigonal
    having threefold symmetry
    According to the VSEPR model, the three regions radiate from carbon at angles of 120°, and the shape of the molecule is planar (trigonal planar).
  13. electron
    an elementary particle with negative charge
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  14. orbital
    relating to the path of one body around another
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  15. subtractive
    constituting or involving subtraction
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  16. unshared
    not shared
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  17. bonding
    the act of fastening firmly together
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  18. Phosphorus
    a planet seen just before sunrise in the eastern sky
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  19. organophosphate
    an insecticide that interferes with an insect's nervous system
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  20. ethylene
    a flammable colorless gaseous alkene
    VSEPR Model
    Predict the shape of ethylene, C2H4
    The Lewis structure shows carbon surrounded by three regions of electron density; two regions contain single pairs of electrons and the third contains two pairs of electrons forming the double bond to the other carbon.
  21. sulfide
    a compound of sulphur and some other element that is more electropositive
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  22. ethane
    a colorless odorless alkane gas used as fuel
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  23. bond
    a connection that fastens things together
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  24. molecule
    the simplest structural unit of an element or compound
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  25. carbon atom
    an atom of carbon
    Draw the line-bond structure of formaldehyde, and indicate the hybridization of the carbon atom.
  26. mol
    the molecular weight of a substance expressed in grams
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  27. hybrid
    the offspring of genetically dissimilar parents or stock
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  28. carbon
    an abundant nonmetallic element in all organic compounds
    Carbon dioxide, CO2, has two polar bonds but, because of its geometry, is a nonpolar molecule.
  29. sulfur
    an abundant tasteless odorless multivalent nonmetallic element; best known in yellow crystals; occurs in many sulphide and sulphate minerals and even in native form (especially in volcanic regions)
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  30. methane
    a colorless, odorless gas used as a fuel
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  31. negative charge
    the state of having a surplus of electrons
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  32. polarity
    a relation between two opposite attributes or tendencies
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  33. formaldehyde
    a colorless poisonous gas; made by the oxidation of methanol
    VSEPR Model
    Predict the shape of formaldehyde, CH2O
    The Lewis structure shows carbon surrounded by three regions of electron density; two regions contain single pairs of electrons and the third contains two pairs of electrons forming the double bond to oxygen.
  34. valence
    the capacity of something or someone to react with or affect others
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  35. 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
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  36. lobe
    a rounded projection that is part of a larger structure
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  37. atom
    the smallest component of an element
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  38. radiate
    send out rays or waves
    According to the VSEPR model, the four regions radiate from carbon at angles of 109.5°, and the shape of the molecule is tetrahedral.
  39. methyl alcohol
    a light volatile flammable poisonous liquid alcohol
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  40. density
    the amount per unit size
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  41. acetylene
    a colorless flammable gas used chiefly in welding and in organic synthesis
    VSEPR Model
    Predict the shape of acetylene, C2H2
    The Lewis structure shows carbon surrounded by two regions of electron density; one region contains a single pair of electron, and the second contains three pairs of electrons forming the triple bond to carbon.
  42. overlap
    extend over and cover a part of
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  43. oxygen
    a colorless, odorless gas that is essential for respiration
    VSEPR Model
    Predict the shape of water, H2O
    The Lewis structure shows oxygen surrounded by four regions of electron density; two regions contain single pairs of electrons, and the third and fourth contain unshared pairs of electrons.
  44. molecular
    relating to the simplest units of an element or compound
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  45. methanol
    a light volatile flammable poisonous liquid alcohol
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  46. polar
    of or existing within the Arctic or Antarctic Circles
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  47. negatively charged
    having a negative charge
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  48. reactant
    a substance that is altered during a chemical process
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  49. algebraic
    of or relating to algebra
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  50. nitrogen
    a common nonmetallic element that is normally a colorless odorless tasteless inert diatomic gas; constitutes 78 percent of the atmosphere by volume; a constituent of all living tissues
    VSEPR Model
    Predict the shape of ammonia, NH3
    The Lewis structure shows nitrogen surrounded by four regions of electron density; three regions contain single pairs of electrons, and the fourth contains an unshared pair of electrons.
  51. angle
    the space between two lines or planes that intersect
    According to the VSEPR model, the four regions radiate from carbon at angles of 109.5°, and the shape of the molecule is tetrahedral.
  52. positive charge
    the state of having a deficiency of electrons
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  53. methyl
    the univalent radical CH3- derived from methane
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  54. Linus Pauling
    United States chemist who studied the nature of chemical bonding (1901-1994)
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  55. nucleus
    a part of the cell responsible for growth and reproduction
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  56. additive
    characterized or produced by addition
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combinatio...
  57. node
    any thickened enlargement
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  58. Bond
    United States civil rights leader who was elected to the legislature in Georgia but was barred from taking his seat because he opposed the Vietnam War (born 1940)
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  59. asymmetrical
    characterized by an imbalance in spatial arrangement
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  60. dumbbell
    an exercising weight held in one hand
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  61. head-on
    meeting front to front
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  62. model
    a representation of something, often on a smaller scale
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  63. region
    the extended spatial location of something
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  64. atomic
    relating to the smallest component of an element
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  65. structure
    a complex entity made of many parts
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  66. Pauling
    United States chemist who studied the nature of chemical bonding (1901-1994)
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  67. pair
    a set of two similar things considered as a unit
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  68. dissociation
    the act of removing from association
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  69. elongate
    lengthen
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  70. linear
    involving a single dimension
    According to the VSEPR model, the two regions radiate from carbon at an angle of 180°, and the shape of the molecule is linear.
  71. geometry
    the mathematics of points and lines and curves and surfaces
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  72. predict
    make a guess about what will happen in the future
    VSEPR Model
    Predict the shape of methane, CH4
    The Lewis structure shows carbon surrounded by four regions of electron density.
  73. phosphorus
    a multivalent nonmetallic element of the nitrogen family that occurs commonly in inorganic phosphate rocks and as organic phosphates in all living cells; is highly reactive and occurs in several allotropic forms
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  74. formation
    the act of establishing or creating something
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  75. ammonia
    a strong-smelling gas compounded of nitrogen and hydrogen
    Polarity of Molecules
    Ammonia, NH3, has three polar bonds and, because of its geometry, is a polar molecule.
  76. combination
    the act of bringing things together to form a new whole
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  77. measured
    having notes of fixed rhythmic value
    The measured H-C-H bond angles are 109.5°.
  78. shape
    a perceptual structure
    VSEPR Model
    Predict the shape of methane, CH4
    The Lewis structure shows carbon surrounded by four regions of electron density.
  79. CO2
    a colorless, odorless greenhouse gas essential for photosynthesis
    Carbon dioxide, CO2, has two polar bonds but, because of its geometry, is a nonpolar molecule.
  80. sharing
    unselfishly willing to partake with others
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  81. oriented
    adjusted or located in relation to surroundings
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  82. hydrogen
    a colorless, odorless gas; the lightest chemical element
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  83. Lewis
    English critic and novelist
    VSEPR Model
    Predict the shape of methane, CH4
    The Lewis structure shows carbon surrounded by four regions of electron density.
  84. mathematically
    with respect to mathematics
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  85. combine
    put or add together
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  86. negatively
    in a harmful manner
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  87. Lowry
    English painter (1887-1976)
    VSEPR Model



    sp2 Hybrid Orbitals and the Structure of Ethylene
    σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
    Two non-hybridized 2p orbitals overlap sideways forming a  bond
    Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond








    sp Hybrid Orbitals and the Structure of Acetylene
    sp hybridized orbital
    A hybrid orbital derived from the combination of one s and one p atomic orbital
    The two sp hybrids are oriented at an angle of 180º...
  88. pyramidal
    resembling a pyramid
    According to the VSEPR model, the four regions radiate from nitrogen at angles of 109.5°, and the shape of the molecule is pyramidal.
  89. partial
    being or affecting only a segment
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  90. orient
    the eastern hemisphere
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  91. contain
    hold or have within
    VSEPR Model
    Predict the shape of ammonia, NH3
    The Lewis structure shows nitrogen surrounded by four regions of electron density; three regions contain single pairs of electrons, and the fourth contains an unshared pair of electrons.
  92. chemical
    produced by reactions involving atomic or molecular changes
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  93. preservative
    tending or having the power to protect or prevent decay
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  94. triple
    having three units or components or elements
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  95. paired
    used of gloves, socks, etc.
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  96. sigma
    the 18th letter of the Greek alphabet
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  97. generate
    bring into existence
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  98. orientation
    the act of determining one's position
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  99. biological
    pertaining to life and living things
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  100. energy
    forceful exertion
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  101. overlapping
    with a design in which one element covers a part of another
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  102. conversely
    with the terms of the relation reversed
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  103. surrounded
    confined on all sides
    VSEPR Model
    Predict the shape of methane, CH4
    The Lewis structure shows carbon surrounded by four regions of electron density.
  104. shared
    have in common; held or experienced in common
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  105. subtract
    deduct; calculate the difference between two numbers
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  106. combining
    the act of combining things to form a new whole
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  107. theory
    a belief that can guide behavior
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  108. draw the line
    reasonably object (to) or set a limit (on)
    Draw the line-bond structure of formaldehyde, and indicate the hybridization of the carbon atom.
  109. carbon dioxide
    a colorless, odorless greenhouse gas essential for photosynthesis
    Carbon dioxide, CO2, has two polar bonds but, because of its geometry, is a nonpolar molecule.
  110. fraction
    a small part or item forming a piece of a whole
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  111. elongated
    drawn out or made longer spatially
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  112. negative
    characterized by denial or opposition or resistance
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  113. chemist
    a scientist who studies elements that make up matter
    VSEPR Model



    sp2 Hybrid Orbitals and the Structure of Ethylene
    σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
    Two non-hybridized 2p orbitals overlap sideways forming a  bond
    Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond








    sp Hybrid Orbitals and the Structure of Acetylene
    sp hybridized orbital
    A hybrid orbital derived from the combination of one s and one p atomic orbital
    The two sp hybrids are oriented at an angle of 180º...
  114. form
    a perceptual structure
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  115. repulsion
    the act of successfully defending against an attack
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  116. share
    assets belonging to an individual person or group
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  117. two
    the cardinal number that is the sum of one and one
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  118. symmetrical
    exhibiting equivalence or correspondence among constituents
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  119. derivative
    a compound obtained from another compound
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  120. phosphate
    a salt of phosphoric acid
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  121. surround
    extend on all sides of simultaneously; encircle
    VSEPR Model
    Predict the shape of methane, CH4
    The Lewis structure shows carbon surrounded by four regions of electron density.
  122. 180
    being ten more than one hundred seventy
    According to the VSEPR model, the two regions radiate from carbon at an angle of 180°, and the shape of the molecule is linear.
  123. dioxide
    an oxide containing two atoms of oxygen in the molecule
    Carbon dioxide, CO2, has two polar bonds but, because of its geometry, is a nonpolar molecule.
  124. rotting
    the process of decay caused by bacterial or fungal action
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rottin...
  125. derive
    come from
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  126. organic
    having properties characteristic of living beings
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  127. commonly
    under normal conditions
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  128. formed
    having or given a form or shape
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  129. single
    existing alone or consisting of one entity or part or aspect or individual
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  130. double
    consisting of or involving two parts or components usually in pairs
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  131. positive
    characterized by or displaying affirmation or acceptance
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  132. four
    the cardinal number that is the sum of three and one
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  133. biology
    the science that studies living organisms
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  134. measure
    determine the dimensions of something or somebody
    The measured H-C-H bond angles are 109.5°.
  135. 120
    the cardinal number that is the product of ten and twelve
    According to the VSEPR model, the three regions radiate from carbon at angles of 120°, and the shape of the molecule is planar (trigonal planar).
  136. singly
    apart from others
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  137. bacteria
    single-celled organisms that can cause disease
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  138. acquire
    come into the possession of something concrete or abstract
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  139. occupied
    held or filled or in use
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  140. involve
    contain as a part
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  141. sideways
    toward one side
    VSEPR Model



    sp2 Hybrid Orbitals and the Structure of Ethylene
    σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
    Two non-hybridized 2p orbitals overlap sideways forming a  bond
    Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond








    sp Hybrid Orbitals and the Structure of Acetylene
    sp hybridized orbital
    A hybrid orbital derived from the combination of one s and one p atomic orbital
    The two sp hybrids are oriented at an angle ...
  142. according
    in agreement with
    According to the VSEPR model, the four regions radiate from carbon at angles of 109.5°, and the shape of the molecule is tetrahedral.
  143. equilibrium
    a stable situation in which forces cancel one another
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  144. accord
    concurrence of opinion
    According to the VSEPR model, the four regions radiate from carbon at angles of 109.5°, and the shape of the molecule is tetrahedral.
  145. diagram
    a drawing intended to explain how something works
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  146. dynamic
    characterized by action or forcefulness of personality
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  147. occupy
    live in (a certain place)
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  148. charge
    assign a duty, responsibility or obligation to
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  149. mathematical
    of or pertaining to or of the nature of mathematics
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combinatio...
  150. encounter
    come together
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  151. shaped
    having the shape of
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  152. derived
    formed or developed from something else; not original
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  153. show
    make visible or noticeable
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  154. Danish
    a Scandinavian language that is the official language of Denmark
    VSEPR Model



    sp2 Hybrid Orbitals and the Structure of Ethylene
    σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
    Two non-hybridized 2p orbitals overlap sideways forming a  bond
    Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond








    sp Hybrid Orbitals and the Structure of Acetylene
    sp hybridized orbital
    A hybrid orbital derived from the combination of one s and one p atomic orbital
    The two sp hybrids are oriented at an angle of 180º...
  155. simple
    having few parts; not complex or complicated or involved
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  156. example
    an item of information that is typical of a class or group
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  157. arrow
    projectile with a thin shaft intended to be shot from a bow
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  158. effectively
    in a manner producing an intended result
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  159. lone
    being the only one; single and isolated from others
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  160. rot
    break down
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rottin...
  161. repel
    force or drive back
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  162. odor
    any property detected by the sense of smell
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  163. three
    the cardinal number that is the sum of one and one and one
    Polarity of Molecules
    Ammonia, NH3, has three polar bonds and, because of its geometry, is a polar molecule.
  164. nature
    the physical world including plants and animals
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  165. describe
    give a statement representing something
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  166. minimum
    the smallest possible quantity
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  167. alcohol
    a volatile compound made by distillation
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  168. lesser
    of smaller size or importance
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  169. promotion
    the act of raising in rank or position
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  170. non
    negation of a word or group of words
    VSEPR Model



    sp2 Hybrid Orbitals and the Structure of Ethylene
    σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
    Two non-hybridized 2p orbitals overlap sideways forming a  bond
    Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond








    sp Hybrid Orbitals and the Structure of Acetylene
    sp hybridized orbital
    A hybrid orbital derived from the combination of one s and one p atomic orbital
    The two sp hybrids are oriented at an angle ...
  171. lead
    take somebody somewhere
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  172. result
    something that follows as a consequence
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  173. crossed
    placed crosswise
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  174. tissue
    part of an organism consisting of an aggregate of cells
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  175. larger
    large or big relative to something else
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  176. close to
    (of quantities) imprecise but fairly close to correct
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  177. add to
    have an increased effect
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  178. fourth
    following the third position
    VSEPR Model
    Predict the shape of ammonia, NH3
    The Lewis structure shows nitrogen surrounded by four regions of electron density; three regions contain single pairs of electrons, and the fourth contains an unshared pair of electrons.
  179. equivalent
    being essentially comparable to something
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  180. third
    one of three equal parts of a divisible whole
    VSEPR Model
    Predict the shape of water, H2O
    The Lewis structure shows oxygen surrounded by four regions of electron density; two regions contain single pairs of electrons, and the third and fourth contain unshared pairs of electrons.
  181. responsible for
    being the agent or cause
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  182. each
    separately for every person or thing
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  183. compound
    a whole formed by a union of two or more elements or parts
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of rotting f...
  184. between
    in the interval
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between
  185. indicate
    designate a place, direction, person, or thing
    Draw the line-bond structure of formaldehyde, and indicate the hybridization of the carbon atom.
  186. one
    smallest whole number or a numeral representing this number
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  187. stable
    resistant to change of position or condition
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  188. depend on
    be contingent on
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  189. various
    having great diversity or variety
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  190. differ
    be dissimilar or unlike
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  191. degree
    a specific identifiable position in a continuum or series
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  192. strength
    the property of being physically or mentally powerful
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond s...
  193. length
    the linear extent in space from one end to the other
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  194. starting
    appropriate to the beginning or start of an event
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  195. distance
    the property created by the space between two objects
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  196. responsible
    worthy of or requiring trust; held accountable
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  197. create
    bring into existence
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  198. solution
    a homogeneous mixture of two or more substances
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combinatio...
  199. function
    what something is used for
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combinatio...
  200. elements
    violent or severe weather
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  201. strongly
    with power
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  202. involved
    connected by participation or association or use
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  203. smaller
    small or little relative to something else
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
  204. substance
    the real physical matter of which a person or thing consists
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  205. cross
    a marking that consists of lines that intersect each other
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  206. low
    less than normal in degree or intensity or amount
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  207. charged
    of a particle or body or system
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  208. characteristic
    typical or distinctive
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  209. sign
    a visible clue that something has happened or is present
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  210. tail
    the posterior part of the body of a vertebrate especially when elongated and extending beyond the trunk or main part of the body
    Polarity of Covalent Bonds
    In a polar covalent bond,
    the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
    the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow

    Polarity of Molecules
    Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
  211. relative
    not absolute or complete
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
  212. attract
    exert a force on
    The Nature of Chemical Bonds: Valence Bond Theory
    Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals

    Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
    H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
    H-H bond is cylindrically symmetrical
    Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
  213. using
    an act that exploits or victimizes someone
    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Oxygen
    Methanol CH3OH
    Methyl alcohol
    Bonds are close to the109.5º tetrahedral angle
    Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs


    Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
    Covalent bonds formed by other elements can also be described using hybrid orbitals
    Nitrogen
    Methylamine CH3NH2
    Organic derivative of ammonia and the substance responsible for the odor of ro...
  214. different
    unlike in nature, quality, form, or degree
    Polarity of Molecules
    A molecule will be polar if:
    it has polar bonds, and
    its centers of partial positive and partial negative charges lie at different places within the molecule.
  215. bent
    stooped (used of the back and knees)
    According to the VSEPR model, the four regions radiate from oxygen at angles of 109.5°, and the shape of the molecule is bent.
  216. shell
    the outer covering of an animal
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  217. other
    not the same one or ones already mentioned or implied
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bo...
  218. description
    the act of depicting something
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combinatio...
  219. product
    an artifact that has been created by someone or some process
    Bonding In Methane CH4
    The formation of molecular orbitals in ethane
    The formation of molecular orbitals in ethane

    The Nature of Chemical Bonds: Valence Bond Theory
    Bond length
    The distance between nuclei at the minimum energy point
    Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
    The Nature of Chemical Bonds: Valence Bond Theory
    Bond stre...
  220. egg
    animal reproductive body consisting of an ovum or embryo together with nutritive and protective envelopes; especially the thin-shelled reproductive body laid by e.g. female birds
    Example Predicting the Structures of Simple Molecules
    Solution
    There is only one way that two hydrogens, one carbon, and one oxygen can combine





    Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
    The Nature of Chemical Bonds: Molecular Orbital Theory
    Molecular Orbital Theory (MO)
    A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
    Additive combination of tw...
  221. equally
    in a balanced or impartial way
    Polarity of Covalent Bonds
    Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
    nonpolar covalent bond: electrons are shared equally
    polar covalent bond: electron sharing is not equal

    the degree of sharing depends on the relative electronegativities of the bonded atoms.
Created on Wed Sep 23 07:17:19 EDT 2009

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