Intermolecular Forces and Properties

Covalent bond

Metallic bond

Hydrogen bond

Ionic bond

Dipole-dipole forces

Hydrogen bonding

London dispersion forces

Ion-dipole forces

$CO_2$

$BF_3$

$SO_2$

$CH_4$

n-pentane has stronger dipole-dipole forces.

n-pentane has stronger hydrogen bonds.

n-pentane has a more linear shape, allowing for greater London Dispersion Forces.

Neopentane has a more linear shape, allowing for greater London Dispersion Forces.

$CH_3Cl$ because chlorine is more electronegative than bromine.

$CH_3Br$ because bromine is more electronegative than chlorine.

Both have equal dipole-dipole forces because they are both halogens.

Neither exhibits dipole-dipole forces.

Butane has stronger hydrogen bonds.

Acetone has stronger London Dispersion Forces.

Acetone has dipole-dipole forces, while butane only has London Dispersion Forces.

Butane only has dipole-dipole forces.

$CH_4$ because it is smaller.

$C_{10}H_{22}$ because it has more electrons and is more polarizable.

$CH_4$ because it is more polarizable.

Both have equal LDFs because they are both hydrocarbons.

$CH_3OCH_3$

$H_2O$

$H_2S$

$CH_4$

$Na^+$ ions are attracted to the negative oxygen end of water molecules.

$Na^+$ ions are repelled by the negative oxygen end of water molecules.

$Na^+$ ions are attracted to the positive hydrogen end of water molecules.

There is no interaction between $Na^+$ ions and water molecules.

Dipole-dipole forces

Hydrogen bonding

Ion-ion attractions

London dispersion forces