Which of the following molecule can in intermolecular hydrogen bonding with water?

(1) Urea
(2) CH₄
(3) CCl₄
(4) CHCl3

Molecules that Form Intermolecular Hydrogen Bonds with Water

An important intermolecular force that affects solubility, boiling points, and molecular interactions is hydrogen bonding. A molecule needs the following in order to create hydrogen bonds with water:

A donor of hydrogen (N-H or O-H bonds)

Electronegative atoms with lone pairs, such as O or N, are hydrogen acceptors.

Urea (Option 1) is the right response.

Urea (CO(NH₂)₂) is the right response among the options provided because:

It has N-H bonds, which can give water hydrogen bonds.

Its nitrogen (N) and oxygen (O) atoms are capable of taking up hydrogen bonds from water.

Urea is very soluble in water due to its potent hydrogen bonding ability.

Why Other Choices Are Wrong

CH₄ (Methane):

lacks the O or N electronegative atoms required for hydrogen bonding.

Only experiences weak van der Waals forces.

Carbon Tetrachloride, or CCl₄:

Electronegative atoms are not directly joined to hydrogen atoms.

It is non-polar and does not form hydrogen bonds with water.

Chloroform, or CHCl₃:

The hydrogen is not acidic enough to form a strong hydrogen bond with water, despite having a slightly polar C-H bond.

In conclusion, urea and water form hydrogen bonds.

The presence of electronegative acceptor atoms and N-H or O-H bonds is necessary for the formation of hydrogen bonds with water. Urea is the right response because it is the only molecule among the options that can create strong hydrogen bonds with water.