Identify the molecule (X) with maximum number of lone pairs of electrons (obtained using Lewis dot structure) among HNO₃, H₂SO₄, NF₃ and O₃. Choose the correct bond angle made by the central atom of the molecule (X).
Q. Identify the molecule (X) with maximum number of lone pairs of electrons (obtained using Lewis dot structure) among HNO3, H2SO4, NF3 and O3. Choose the correct bond angle made by the central atom of the molecule (X).
A. 107°
B. 102°
C. 120°
D. 116°
Correct Answer: 102°

Explanation

First, we compare the number of lone pairs on the central atom using Lewis dot structures.

In HNO3, nitrogen is the central atom. Nitrogen forms three sigma bonds and one pi bond with oxygen atoms and has no lone pair on the central atom.

In H2SO4, sulfur is the central atom. Sulfur forms four sigma bonds and two pi bonds with oxygen atoms and does not have any lone pair on the central atom.

In NF3, nitrogen is the central atom. It forms three N–F bonds and has one lone pair of electrons.

In O3, the central oxygen atom forms two sigma bonds and has two lone pairs of electrons.

Thus, O3 has the maximum number of lone pairs on the central atom.

The central oxygen in O3 has four electron pairs (2 bond pairs + 2 lone pairs), corresponding to a tetrahedral electron geometry. Due to strong lone pair–lone pair and lone pair–bond pair repulsions, the bond angle decreases from the ideal value.

The observed bond angle in ozone is approximately 102°.

Hence, the correct bond angle is 102°.

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