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.
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.
(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.
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.
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.
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 ...
(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 ...
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...
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...
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.
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.
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 ...
ExamplePredicting 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...
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...
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...
a planet (usually Venus) 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...
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...
a flammable colorless gaseous alkene; obtained from petroleum and natural gas and used in manufacturing many other chemicals; sometimes used as an anesthetic
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.
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...
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...
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.
(physics and chemistry) 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.
the molecular weight of a substance expressed in grams; the basic unit of amount of substance adopted under the Systeme International d'Unites
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...
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 ...
an abundant nonmetallic tetravalent element occurring in three allotropic forms: amorphous carbon and graphite and diamond; occurs in all organic compounds
Carbon dioxide, CO2, has two polar bonds but, because of its geometry, is a nonpolar molecule.
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...
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 ...
having a surplus of electrons; having a lower electric potential
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.
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.
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.
(chemistry) a property of atoms or radicals; their combining power given in terms of the number of hydrogen atoms (or the equivalent)
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...
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.
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 ...
(physics and chemistry) the smallest component of an element having the chemical properties of the 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.
a light volatile flammable poisonous liquid alcohol; used as an antifreeze and solvent and fuel and as a denaturant for ethyl 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...
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...
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.
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...
a nonmetallic bivalent element that is normally a colorless odorless tasteless nonflammable diatomic gas; constitutes 21 percent of the atmosphere by volume; the most abundant element in the earth's crust
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.
relating to or produced by or consisting of 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
Bo...
a light volatile flammable poisonous liquid alcohol; used as an antifreeze and solvent and fuel and as a denaturant for ethyl 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...
of or existing at or near a geographical pole or 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.
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...
a chemical substance that is present at the start of a chemical reaction
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...
ExamplePredicting 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...
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.
having a deficiency of electrons; having a higher electric potential
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.
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...
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 ...
a part of the cell containing DNA and RNA and 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...
ExamplePredicting 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...
ExamplePredicting 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...
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...
characterized by asymmetry in the spatial arrangement or placement of parts or components
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 ...
an exercising weight; two spheres connected by a short bar that serves as a handle
ExamplePredicting 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...
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...
representation of something (sometimes 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...
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...
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...
a thing constructed; a complex entity constructed 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 ...
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 ...
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.
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...
ExamplePredicting 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...
the pure 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.
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...
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...
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 ...
a heavy odorless colorless gas formed during respiration and by the decomposition of organic substances; absorbed from the air by plants in photosynthesis
Carbon dioxide, CO2, has two polar bonds but, because of its geometry, is a nonpolar 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.
adjusted or located in relation to surroundings or circumstances; sometimes used in combination
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 ...
a nonmetallic univalent element that is normally a colorless and odorless highly flammable diatomic gas; the simplest and lightest and most abundant element in the universe
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...
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 ...
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 ...
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...
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 Orbitalsand 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...
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.
the hemisphere that includes Eurasia and Africa and Australia
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 ...
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.
of or made from or using substances produced by or used in 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...
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...
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...
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...
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 ...
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 ...
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 ...
pertaining to biology or 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...
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...
covering with a design in which one element covers a part of another (as with tiles or shingles)
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...
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...
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.
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 ...
ExamplePredicting 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...
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...
a heavy odorless colorless gas formed during respiration and by the decomposition of organic substances; absorbed from the air by plants in photosynthesis
Carbon dioxide, CO2, has two polar bonds but, because of its geometry, is a nonpolar molecule.
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.
ExamplePredicting 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...
characterized by or displaying negation or denial or opposition or resistance; having no positive features
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.
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 Orbitalsand 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...
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...
the act of repulsing or repelling an attack; a successful defensive stand
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...
assets belonging to or due to or contributed by 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.
the cardinal number that is the sum of one and one or a numeral representing this number
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.
exhibiting equivalence or correspondence among constituents of an entity or between different entities
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...
a compound obtained from, or regarded as derived 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...
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...
(biology) 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...
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 ...
being or relating to or derived from or having properties characteristic of living organisms
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 ...
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...
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...
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...
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...
characterized by or displaying affirmation or acceptance or certainty etc.
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.
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 ...
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...
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...
(microbiology) single-celled or noncellular spherical or spiral or rod-shaped organisms lacking chlorophyll that reproduce by fission; important as pathogens and for biochemical properties; taxonomy is difficult; often considered to be plants
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...
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.
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...
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.
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 Orbitalsand 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 ...
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...
a drawing intended to explain how something works; a drawing showing the relation between the parts
ExamplePredicting 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...
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...
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...
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.
of or pertaining to or of the nature of mathematics
ExamplePredicting 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...
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...
ExamplePredicting 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...
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 ...
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 ...
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 Orbitalsand 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...
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...
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...
a projectile with a straight thin shaft and an arrowhead on one end and stabilizing vanes on the other; 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.
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 ...
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...
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...
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...
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...
the natural physical world including plants and animals and landscapes 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...
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...
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...
any of a series of volatile hydroxyl compounds that are made from hydrocarbons 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...
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.
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 ...
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 Orbitalsand 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 ...
ExamplePredicting 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...
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...
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.
part of an organism consisting of an aggregate of cells having a similar structure and function
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...
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 ...
(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...
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 ...
following the third position; number four in a countable series
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.
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 ...
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.
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...
(used of count nouns) every one considered individually
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...
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...
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 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 ...
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...
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.
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...
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.
a specific identifiable position in a continuum or series or especially in a process
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.
the property of being physically or mentally strong
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...
the linear extent in space from one end to the other; the longest dimension of something that is fixed in place
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...
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...
the property created by the space between two objects or points
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...
worthy of or requiring responsibility or trust; or 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...
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...
a homogeneous mixture of two or more substances; frequently (but not necessarily) a liquid solution
ExamplePredicting 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...
ExamplePredicting 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...
violent or severe weather (viewed as caused by the action of the four elements)
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...
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 ...
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...
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 ...
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...
a marking that consists of lines that cross 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.
ExamplePredicting 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...
of a particle or body or system; having a net amount of positive or negative electric 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...
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...
a perceptible indication of something not immediately apparent (as a visible clue that something has happened)
ExamplePredicting 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...
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.
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.
exert a force on (a body) causing it to approach or prevent it from moving away
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...
an act that exploits or victimizes someone (treats them unfairly)
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...
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.
the material that forms the hard outer covering of many animals
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...
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...
ExamplePredicting 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...
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...
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
ExamplePredicting 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...
in equal amounts or shares; 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.
bonding
