AP Chem Unit 2 - Molecular Geometry

2 bonds 0 lone pairs

linear

• sp

• 2 hybrid orbitals

• bond angle of 180

• nonpolar if both terminal atoms are the same, polar if not

3 bonds 0 lone pairs

trigonal planar

• sp²

• 3 hybrid orbitals

• bond angle of 120

• nonpolar if all terminal atoms are the same, polar if not

2 bonds 1 lone pair

bent

• sp²

• 3 hybrid orbitals

• bond angle of less than 120

• polar

4 bonds 0 lone pairs

tetrahedral

• sp³

• 4 hybrid orbitals

• bond angle of 109.5

• nonpolar if all terminal atoms are the same, polar if not

3 bonds 1 lone pair

trigonal pyramidal

• sp³

• 4 hybrid orbitals

• bond angle of about 109

• polar

2 bonds 2 lone pairs

bent

• sp³

• 4 hybrid orbitals

• bond angle of less than 109

• polar

5 bonds 0 lone pairs

trigonal bipyramidal

• sp³d

• 5 hybrid orbitals

• bond angle of 120 (for triangle) and 90 (for vertical and horizontal)

• nonpolar if all terminal atoms are the same, polar if not

4 bonds 1 lone pair

seesaw

• sp³d

• 5 hybrid orbitals

• bond angle of less than 120 (for “legs”) and less than 90 (for vertical and horizontal)

• polar

3 bonds 2 lone pairs

t-shaped

• sp³d

• 5 hybrid orbitals

• bond angles of less than 90

• polar

2 bonds 3 lone pairs

linear

• sp³d

• 5 hybrid orbitals

• bond angle of 180

• nonpolar if both terminal atoms are the same, polar if not

6 bonds 0 lone pairs

octahedral

• sp³d²

• 6 hybrid orbitals

• bond angle of 90

• nonpolar if all terminal atoms are the same, polar if not

5 bonds 1 lone pair

square pyramidal

• sp³d²

• 6 hybrid orbitals

• bond angle of less than 90

• polar

4 bonds 2 lone pairs

square planar

• sp³d²

• 6 hybrid orbitals

• bond angle of 90

• nonpolar if all terminal atoms are the same, polar if not