Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force. Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force. CCl4 C5H12 CH3NH2 NaF CH2I2

CH3NH2

Explanation:

Hydrogen bonding is a bond that occurs between hydrogen and a highly electronegative element. It is a kind of dipole - dipole interaction. Hydrogen bonding only occurs when hydrogen is bonded to a highly electronegative element.

If we look at the options stated, it is only in CH3NH2  that hydrogen is bonded to a very electronegative element (nitrogen). Hence, CH3NH2  exhibits hydrogen bonding as its strongest intermolecular force among other intermolecular forces.

CH3NH2

Explanation:

To form hydrogen bondings between the molecules, the compound needs a highly electronegative atom (usually N, O, or F) bonded with a hydrogen atom;

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.