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antibonding orbital
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molecular orbital located outside of the region between two nuclei; electrons in an antibonding orbital destabilize the molecule
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bond order
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number of pairs of electrons between two atoms; it can be found by the number of bonds in a Lewis structure or by the difference between the number of bonding and antibonding electrons divided by two
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bonding orbital
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molecular orbital located between two nuclei; electrons in a bonding orbital stabilize a molecule
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degenerate orbitals
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orbitals that have the same energy
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diamagnetism
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phenomenon in which a material is not magnetic itself but is repelled by a magnetic field; it occurs when there are only paired electrons present
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homonuclear diatomic molecule
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molecule consisting of two identical atoms
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hybrid orbital
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orbital created by combining atomic orbitals on a central atom
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hybridization
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model that describes the changes in the atomic orbitals of an atom when it forms a covalent compound
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linear combination of atomic orbitals
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technique for combining atomic orbitals to create molecular orbitals
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molecular orbital
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region of space in which an electron has a high probability of being found in a molecule
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molecular orbital diagram
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visual representation of the relative energy levels of molecular orbitals
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molecular orbital theory
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model that describes the behavior of electrons delocalized throughout a molecule in terms of the combination of atomic wave functions
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node
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plane separating different lobes of orbitals, where the probability of finding an electron is zero
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overlap
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coexistence of orbitals from two different atoms sharing the same region of space, leading to the formation of a covalent bond
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paramagnetism
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phenomenon in which a material is not magnetic itself but is attracted to a magnetic field; it occurs when there are unpaired electrons present
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pi bond (π bond)
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covalent bond formed by side-by-side overlap of atomic orbitals; the electron density is found on opposite sides of the internuclear axis
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s-p mixing
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change that causes σ
p
orbitals to be less stable than π
p
orbitals due to the mixing of
s
and
p
-based molecular orbitals of similar energies.
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sigma bond (σ bond)
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covalent bond formed by overlap of atomic orbitals along the internuclear axis
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sp
hybrid orbital
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one of a set of two orbitals with a linear arrangement that results from combining one
s
and one
p
orbital
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sp
2
hybrid orbital
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one of a set of three orbitals with a trigonal planar arrangement that results from combining one
s
and two
p
orbitals
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sp
3
hybrid orbital
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one of a set of four orbitals with a tetrahedral arrangement that results from combining one
s
and three
p
orbitals
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sp
3
d
hybrid orbital
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one of a set of five orbitals with a trigonal bipyramidal arrangement that results from combining one
s
, three
p
, and one
d
orbital
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sp
3
d
2
hybrid orbital
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one of a set of six orbitals with an octahedral arrangement that results from combining one
s
, three
p
, and two
d
orbitals
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valence bond theory
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description of bonding that involves atomic orbitals overlapping to form σ or π bonds, within which pairs of electrons are shared
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π bonding orbital
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molecular orbital formed by side-by-side overlap of atomic orbitals, in which the electron density is found on opposite sides of the internuclear axis
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π* bonding orbital
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antibonding molecular orbital formed by out of phase side-by-side overlap of atomic orbitals, in which the electron density is found on both sides of the internuclear axis, and there is a node between the nuclei
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σ bonding orbital
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molecular orbital in which the electron density is found along the axis of the bond
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σ* bonding orbital
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antibonding molecular orbital formed by out-of-phase overlap of atomic orbital along the axis of the bond, generating a node between the nuclei
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