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Chemistry 161

Chapter 7

Linear 2 electron pairs
Trigonal planar 3 electron pairs
Tetrahedral 4 electron pairs
Trigonal bipyramidal 5 electron pairs
Octahedral 6 electron pairs
Pentagonal bipyramidal 7 electron pairs
Valence Shell Electron Pair Repulsion (VSEPR) Model that account for electron pairs in the valence shell of an atom repelling one another
Electron domain A lone pair or a bond, regardless the bond is a single, double or triple
Electron domain geometry Arrangement of electron domains (bonds and lone pairs) around the central atom
Molecular geometry The arrangement of bonded atoms
Bond angle Angle between two adjacent bonds A--B
Equatorial The three bonds that are arranged in a trigonal plane in a triennial bypiramidal geometry
Axial Two bond that form an axis perpendicular to the trigonal plane
Sigma bond Results by head on overlap by atomic orbitals
Pi bonds Results by side on overlap of atomic orbitals, weaker than sigma bonds
Hybridization The icing of atomic orbitals in an atom to generate a set of new orbitals called hybrid orbitals
Hybrid orbitals Used to form covalent bonds, Have different shapes than pure atomic orbitals
Valence bond theory Atoms share electrons when an atomic orbital on one atom overlaps with an atomic orbital on the other
Bonding molecular orbital A molecular orbital that is lower in energy than the atomic orbitals that combined to produce it
Antibonding molecular orbital A molecular orbital that is higher in energy than the atomic orbitals that combined to produce it
Created by: cynthiaf1021