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CHEM: Exam 4

Molecular Geometires

Electron GeometryMolecular Geometry
Linear (0 lone pairs) Linear
Trigonal Planar (0 lone pairs) Trigonal Planar
Trigonal Planar (1 lone pair) Bent
Tetrahedral (0 lone pairs) Tetrahedral
Tetrahedral (1 lone pair) Trigonal Pyramidal
Tetrahedral (2 lone pairs) Bent
Trigonal Bipyramidal (0 lone pairs) Trigonal Bipyramidal
Trigonal Bipyramidal (1 lone pair) Seesaw
Trigonal Bipyramidal (2 lone pairs) T-shaped
Trigonal Bipyramidal (3 lone pairs) Linear
Octahedral (0 lone pairs) Octahedral
Octahedral (1 lone pair) Square Pyramidal
Octahedral (2 lone pairs) Square Planar
What do lone pairs do to the shape? They cause the bond angles to be smaller. Lone pair has more space than bonding pairs, and bonding pairs are closer together than with the lone pair.
Created by: emily.zegarra
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