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Pearson Chemistry - Chapter 8.3

Terms in this set (15)

Molecular orbital
An orbital that applies to the entire molecule. When two atoms combine, this model assumes that their atomic orbitals overlap to produce molecular orbitals, or orbitals that apply to the entire molecule.
Bonding orbital
A molecular orbital that can be occupied by two electrons of a covalent bond.
Sigma bond
A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei.
Pi bond
A covalent bond in which the bonding electrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded atoms.
Tetrahedral angle
A bond angle of 109.5 that results when a central atom forms four bonds directed toward the center of a regular tetrahedron.
VSEPR theory
Valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible.
Hybridization
The mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals.
trigonal planar shape and angle
120 degrees
linear shape and angle
180 degrees
bent shape and angle
105 degrees
pyramidal shape and angle
107 degrees
trigonal bipyramidal shape and angle
90 degrees and 120 degrees
octahedral shape and angle
90 degrees
square planar shape and angle
90 degrees
t- shaped shape and angle
90 degrees
THIS SET IS OFTEN IN FOLDERS WITH...