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OpenStax Chem 8
This content is available for free at http://cnx.org/content/col11760/1.9
| Term | Definition |
|---|---|
| antibonding orbital | molecular orbital located outside of the region between two nuclei; electrons in an antibonding orbital destabilize the molecule |
| 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 |
| bonding orbital | molecular orbital located between two nuclei; electrons in a bonding orbital stabilize a molecule |
| degenerate orbitals | orbitals that have the same energy |
| 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 |
| homonuclear diatomic molecule | molecule consisting of two identical atoms |
| hybrid orbital | orbital created by combining atomic orbitals on a central atom |
| hybridization | model that describes the changes in the atomic orbitals of an atom when it forms a covalent compound |
| linear combination of atomic orbitals | technique for combining atomic orbitals to create molecular orbitals |
| molecular orbital | region of space in which an electron has a high probability of being found in a molecule |
| molecular orbital diagram | visual representation of the relative energy levels of molecular orbitals |
| molecular orbital theory | model that describes the behavior of electrons delocalized throughout a molecule in terms of the combination of atomic wave functions |
| node | plane separating different lobes of orbitals, where the probability of finding an electron is zero |
| overlap | coexistence of orbitals from two different atoms sharing the same region of space, leading to the formation of a covalent bond |
| 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 |
| 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 |
| 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. |
| sigma bond (σ bond) | covalent bond formed by overlap of atomic orbitals along the internuclear axis |
| sp hybrid orbital | one of a set of two orbitals with a linear arrangement that results from combining one s and one p orbital |
| 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 |
| sp3 hybrid orbital | one of a set of four orbitals with a tetrahedral arrangement that results from combining one s and three p orbitals |
| 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 |
| 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 |
| valence bond theory | description of bonding that involves atomic orbitals overlapping to form σ or π bonds, within which pairs of electrons are shared |
| 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 |
| 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 |
| σ bonding orbital | molecular orbital in which the electron density is found along the axis of the bond |
| 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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