Question

Which of the following shows hydrogen bonding?
(A) $N{H_3}$
(B) $P$
(C) $As$
(D) $Sb$

Answer 1

Hint: In order for a hydrogen atom to form a hydrogen bond, a highly electronegative atom must also be present in the molecule. The degree of polarisation of the molecule increases with increasing electronegativity. The electronegative atom should have a tiny size.

Complete step by step solution:
Hydrogen bonding is a unique kind of dipole-dipole interaction between molecules. It originates from the attraction between two extremely electronegative atoms, one of which is a hydrogen atom covalently bound to an extremely electronegative atom such an N, O, or F atom.
As we go through the above options there is no N, O or F in the below three options from which we get the answer as,
As from which we can say that the correct answer is $N{H_3}$.

Additional Information: Fluorine (F) is the most electronegative element having a value of electronegativity of 3.98. The hydrogen bond is strongest in Fluorine.

Hence, the correct option is (A)

Note: Hydrogen bonds play a crucial role in a variety of chemical reactions. The special solvent properties of water are due to hydrogen bonding. The three-dimensional structure of folded proteins, such as enzymes and antibodies, is determined by hydrogen bonds, which bind complementary DNA strands together.