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Chemistry 161
Chapter 7
Term | Definition |
---|---|
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 |