Electron/Molecular Geometry and Hybridizations

Linear

Electron group arrangement of 2 electron groups (AX2). Forms an ideal bond angle of 180 degrees (Ex. CO2, BeCl2)

Trigonal Planar

Electron group arrangement of 3 electron groups (AX3). Forms ideal bond angles of 120 degrees (Ex. NO3-, SO3)

Tetrahedral

Electron group arrangement of 4 electron groups (AX4). Forms ideal bond angles of 109.5 degrees (Ex. CH4, SiCl4, ClO4-)

Trigonal Bipyramidal

Electron group arrangement of 5 electron groups (AX5). Forms ideal bond angles of 120 degrees (equatorial) and 90 degrees (axial) (Ex. PCl5, SOF4)

Octahedral

Electron group arrangement of 6 electron groups (AX6). Forms ideal bond angles of 90 degrees (Ex. SF6, IOF5)

equal

If all of the electron groups around a central atom are bonding groups, then the electron group geometry will ____ the molecular geometry.

Bent

Molecular shape resulting from 2 bonding groups and 1 lone pair (AX2E). Forms bond angles of <120 degrees (Ex. SO2, O3)

Trigonal Pyramidal

Molecular shape resulting from 3 bonding groups and 1 lone pair (AX3E). Forms bond angles of <109.5 degrees (Ex. NH3, PF3)

Bent

Molecular shape resulting from 2 bonding groups and 2 lone pairs (AX2E2). Forms bond angles of <109.5 degrees (Ex. H2O, OF2)

Seesaw

Molecular shape resulting from 4 bonding groups and 1 lone pair (AX4E). Forms bond angles of <120 degrees (equatorial) and <90 degrees (axial) (Ex. SF4, IF4)

T-shaped

Molecular shape resulting from 3 bonding groups and 2 lone pairs (AX3E2). Forms bond angles of <120 degrees (equatorial) and <90 degrees (axial) (Ex. ClF3, BrF3)

Linear

Molecular shape resulting from 2 bonding groups and 3 lone pairs (AX2E3). Forms bond angles of <120 degrees (equatorial) and 180 degrees (axial) (Ex. XeF2, I3)

Square Pyramidal

Molecular shape resulting from 5 bonding groups and 1 lone pair (AX5E). Forms bond angles of <90 degrees (Ex. BrF5, XeOF4)

Square Planar

Molecular shape resulting from 4 bonding groups and 2 lone pairs (AX4E2). Forms bond angles of 90 degrees (Ex. XeF4, ICl4)

One s and one p

Two sp

Two p

For a hybridized molecule with linear electron geometry:

Which atomic orbitals are mixed?

Which hybrid orbitals are formed?

Which unhybridized orbitals are remaining?

One s and two p

Three sp2

One p

For a hybridized molecule with trigonal planar electron geometry:

Which atomic orbitals are mixed?

Which hybrid orbitals are formed?

Which unhybridized orbitals are remaining?

One s and three p

Four sp3

No p remaining

For a hybridized molecule with tetrahedral electron geometry:

Which atomic orbitals are mixed?

Which hybrid orbitals are formed?

Which unhybridized orbitals are remaining?

One s, three p, and one d

Five sp3d

Four d remaining

For a hybridized molecule with trigonal bipyramidal electron geometry:

Which atomic orbitals are mixed?

Which hybrid orbitals are formed?

Which unhybridized orbitals are remaining?

One s, three p, and two d

Six sp3d2

Three d remaining

For a hybridized molecule with octahedral electron geometry:

Which atomic orbitals are mixed?

Which hybrid orbitals are formed?

Which unhybridized orbitals are remaining?