Molecular Geometry and VSEPR Theory

Flashcards covering common molecular geometries based on VSEPR theory, detailing electron groups, bonding groups, lone pairs, electron geometry, approximate bond angles, and examples.

Linear Molecular Geometry (2 Electron Groups)

Occurs with 2 electron groups, 2 bonding groups, and 0 lone pairs. The electron geometry is Linear, and bond angles are 180°. Example: CO2.

Trigonal Planar Molecular Geometry (3 Electron Groups)

Occurs with 3 electron groups, 3 bonding groups, and 0 lone pairs. The electron geometry is Trigonal planar, and bond angles are 120°. Example: BF3.

Bent Molecular Geometry (3 Electron Groups, 1 Lone Pair)

Occurs with 3 electron groups, 2 bonding groups, and 1 lone pair. The electron geometry is Trigonal planar, and bond angles are <120°. Example: H2O.

Tetrahedral Molecular Geometry (4 Electron Groups)

Occurs with 4 electron groups, 4 bonding groups, and 0 lone pairs. The electron geometry is Tetrahedral, and bond angles are 109.5°. Example: CH4.

Trigonal Pyramidal Molecular Geometry (4 Electron Groups, 1 Lone Pair)

Occurs with 4 electron groups, 3 bonding groups, and 1 lone pair. The electron geometry is Tetrahedral, and bond angles are <109.5°. Example: NH3.

Bent Molecular Geometry (4 Electron Groups, 2 Lone Pairs)

Occurs with 4 electron groups, 2 bonding groups, and 2 lone pairs. The electron geometry is Tetrahedral, and bond angles are <109.5°. Example: H2O.

Trigonal Bipyramidal Molecular Geometry (5 Electron Groups)

Occurs with 5 electron groups, 5 bonding groups, and 0 lone pairs. The electron geometry is Trigonal bipyramidal, and bond angles are 120° (equatorial) and 90° (axial). Example: PCl5.

Seesaw Molecular Geometry (5 Electron Groups, 1 Lone Pair)

Occurs with 5 electron groups, 4 bonding groups, and 1 lone pair. The electron geometry is Trigonal bipyramidal, and bond angles are <120° (equatorial) and <90° (axial). Example: SF4.

T-shaped Molecular Geometry (5 Electron Groups, 2 Lone Pairs)

Occurs with 5 electron groups, 3 bonding groups, and 2 lone pairs. The electron geometry is Trigonal bipyramidal, and bond angles are <90°. Example: ClF3.

Linear Molecular Geometry (5 Electron Groups, 3 Lone Pairs)

Occurs with 5 electron groups, 2 bonding groups, and 3 lone pairs. The electron geometry is Trigonal bipyramidal, and bond angles are 180°. Example: XeF2.

Octahedral Molecular Geometry (6 Electron Groups)

Occurs with 6 electron groups, 6 bonding groups, and 0 lone pairs. The electron geometry is Octahedral, and bond angles are 90°. Example: SF6.

Square Pyramidal Molecular Geometry (6 Electron Groups, 1 Lone Pair)

Occurs with 6 electron groups, 5 bonding groups, and 1 lone pair. The electron geometry is Octahedral, and bond angles are <90°. Example: BrF5.

Square Planar Molecular Geometry (6 Electron Groups, 2 Lone Pairs)

Occurs with 6 electron groups, 4 bonding groups, and 2 lone pairs. The electron geometry is Octahedral, and bond angles are 90°. Example: XeF4.