Intermolecular Forces and Properties

Covalent bond

Metallic bond

Hydrogen bond

Ionic bond

Dipole-dipole forces

Hydrogen bonding

London dispersion forces

Ion-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.

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.

$CO_2$

$BF_3$

$SO_2$

$CH_4$

$CH_3Cl$ 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.

$CH_3OCH_3$

$H_2O$

$H_2S$

$CH_4$

$HF$ because fluorine is more electronegative than oxygen.

$H_2O$ because oxygen is more electronegative than fluorine.

Both form equally strong hydrogen bonds because they both contain hydrogen.

Neither forms hydrogen bonds.

Hydrogen bonding increases the kinetic energy of water molecules.

Hydrogen bonding causes water molecules to repel each other.

Hydrogen bonding creates strong cohesive forces between water molecules.

Hydrogen bonding decreases the density of water.