Question

How many of the following has hydrogen
bonding
NH3, CH4 H2O HI, HF, HCOOH,
B(OH)3, CH3COOH, HCO, ion​

Answer 1

All have hydrogen bonding. without B(OH)3

Answer 2

Answer:

All compounds have hydrogen bonding except $CH_{4}$ and $HI$.

Explanation:

• Hydrogen bonding is a very special kind of dipole-dipole attraction between molecules.
• It is the electrostatic force of attraction between a hydrogen atom, which is bonded to a highly electronegative atom, and another highly electronegative around it.
• The higher the electronegativity of an atom, the greater the polarization.  
• The size of the electronegative atom should be small so that there is greater force of attraction.
• The examples of electronegative atoms that can establish hydrogen bondings are-

1. Nitrogen
2. Oxygen
3. Fluorine

• In each compound: $NH_{3}, H_{2}O, HF, HCOOH, B(OH)_{3}, CH_{3}COOH, HCO_{3}^{-2}$, there exist hydrogen bondings amongst its molecules.
• In $HI$ and $CH_{4}$ there are no electronegative atoms; hence, no hydrogen bonding exists.