Question

Which of the following statements is true about hydrogen bonding?

• A. Cl and N have comparable electronegativities yet there is no H-bonding in HCl because size of Cl is large
• B. Intermolecular H-bonding results in decrease in m.p. and b.p.
• C. Ice has maximum density at $0^\circ $ C due to H-bonding
• D. $KHCl_{2}\left(\right.HCl_{2}^{-}\left.\right)$ exists but $KHF_{2}\left(\right.HF_{2}^{-}\left.\right)$ does not exist due to lack of H-bonding in HCl

Answer 1

Answer: (A)

For hydrogen bonding, the size of the atom should be small and electronegativity must be high for e.g. F, O, N. Although chlorine has high electronegativity but due to its larger size hydrogen bonding is not possible with it. $KHCl_{2}\left(\right.HCl_{2}^{-}\left.\right)$ don't exists but $KHF_{2}\left(\right.HF_{2}^{-}\left.\right)$ exists due to lack of H-bonding in HCl but possible in HF.