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| antibonding orbital | molecular orbital located outside of the region between two nuclei; electrons in an antibonding orbital destabilize the molecule
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| bond order | 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 | molecular orbital located between two nuclei; electrons in a bonding orbital stabilize a molecule
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| degenerate orbitals | orbitals that have the same energy
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| diamagnetism | 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 | molecule consisting of two identical atoms
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| hybrid orbital | orbital created by combining atomic orbitals on a central atom
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| hybridization | 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 | technique for combining atomic orbitals to create molecular orbitals
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| molecular orbital | region of space in which an electron has a high probability of being found in a molecule
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| molecular orbital diagram | visual representation of the relative energy levels of molecular orbitals
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| molecular orbital theory | 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 | plane separating different lobes of orbitals, where the probability of finding an electron is zero
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| overlap | 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 | 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) | 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 | change that causes σp orbitals to be less stable than πp orbitals due to the mixing of s and p-based molecular orbitals of similar energies.
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| sigma bond (σ bond) | covalent bond formed by overlap of atomic orbitals along the internuclear axis
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| sp hybrid orbital | 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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| sp2 hybrid orbital | 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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| sp3 hybrid orbital | 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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| sp3d hybrid orbital | 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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| sp3d2 hybrid orbital | 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 | 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 | 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 | 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 | molecular orbital in which the electron density is found along the axis of the bond
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| σ* bonding orbital | 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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