AP Chem - Molecular Geometry

Linear

number of electron pairs: 2, number of lone pairs: 0, electronic geometry: linear, bond angles: 180, hybridization: sp

Trigonal planar

number of electron pairs: 3, number of lone pairs: 0, electronic geometry: trigonal planar, bond angles: 120, hybridization: sp²

Bent

number of electron pairs: 3, number of lone pairs: 1, electronic geometry: trigonal planar, bond angles: 119, hybridization: sp²

Tetrahedral

number of electron pairs: 4, number of lone pairs: 0, electronic geometry: tetrahedral, bond angles: 109.5, hybridization: sp³

Pyramidal

number of electron pairs: 4, number of lone pairs: 1, electronic geometry: tetrahedral, bond angles: 107.5, hybridization: sp³

Bent (2)

number of electron pairs: 4, number of lone pairs: 2, electronic geometry: tetrahedral, bond angles: 105.5, hybridization: sp³

Trigonal bipyramidal

number of electron pairs: 5, number of lone pairs: 0, electronic geometry: trigonal bipyramidal, bond angles: 120; 90, hybridization: sp³d

See-saw

number of electron pairs: 5, number of lone pairs: 1, electronic geometry: trigonal bipyramidal, bond angles: 119; 90, hybridization: sp³d

T-shaped

number of electron pairs: 5, number of lone pairs: 2, electronic geometry: trigonal bipyramidal, bond angles: 90, hybridization: sp³d

Linear (expanded)

number of electron pairs: 5, number of lone pairs: 3, electronic geometry: trigonal bipyramidal, bond angles: 180, hybridization: sp³d

Octahedral

number of electron pairs: 6, number of lone pairs: 0, electronic geometry: octahedral, bond angles: 90, hybridization: sp³d²

Square pyramidal

number of electron pairs: 6, number of lone pairs: 1, electronic geometry: octahedral, bond angles: 90, hybridization: sp³d²

Square planar

number of electron pairs: 6, number of lone pairs: 2, electronic geometry: octahedral, bond angles: 90, hybridization: sp³d²