Question

Consider the following compounds
I. $HCl$
II. $HF$
III.$C{H}_{3}COOH$
IV. $C{H}_4$
V. $C{H}_{3}OH$
VI. $C{H}_{3}COO$

$H-$ bonding is not present in

• A. $I,III,andIV$
• B. $I,IV,andVI$
• C. $II,III,andV$
• D. $III,III,andIV$

Answer 1

The correct option is B $I,IV,andVI$

The conditions for hydrogen bonding are:

• The molecule must contain a highly electronegative atom $(F,O,N)$ linked to the hydrogen atom. The higher the electronegativity more is the polarization of the molecule.
• The size of the electronegative atom should be small. The smaller the size, the greater is the electrostatic attraction.

1. In molecule, $HCl$ molecule does not possess any hydrogen bonding due to the large size and low electron density of chlorine atom.
2. In molecule IV there is no electronegative element present.
3. In compound VI no proton attached to the electronegative atom is present.

So the correct option is B