Question

The correct bond angle in the compound which has maximum number of lone pair of electrons among the following compounds H$_2$SO$_4$, HNO$_3$, O$_3$, NF$_3$ is:

• A. 102$^\circ$
• B. 107$^\circ$
• C. 112$^\circ$
• D. 126$^\circ$

Hint:

The presence of lone pairs generally reduces the bond angle due to electron-electron repulsion. The more lone pairs on the central atom, the smaller the bond angle.

Answer 1

The Correct Option is A

To determine the correct bond angle in the compound with the maximum number of lone pair of electrons among the given compounds (H₂SO₄, HNO₃, O₃, NF₃), let's analyze each compound:

1. H₂SO₄ (Sulfuric acid):
   • It has a central sulfur atom surrounded by four double-bonded oxygens, with two of these oxygens being protonated (attached to hydrogen).
   • Sulfur forms a tetrahedral arrangement and has no lone pairs on the sulfur atom.
2. HNO₃ (Nitric acid):
   • Consists of a nitrogen atom bonded to three oxygen atoms, with one of these oxygens being protonated.
   • Nitrogen has a resonance structure that involves the sharing of electrons, but there are no lone pairs on the nitrogen.
3. O₃ (Ozone):
   • Contains three oxygen atoms arranged in a bent conformation due to lone pairs on the central oxygen.
   • The central oxygen has one lone pair, leading to a bond angle of approximately 117°.
4. NF₃ (Nitrogen trifluoride):
   • Comprises a central nitrogen atom bonded to three fluorine atoms.
   • Nitrogen has one lone pair, which affects the bond angle, making it approximately 102°.

The compound with the maximum number of lone pairs influencing the bond angle is NF₃. The presence of one lone pair on the nitrogen atom reduces the bond angle from the ideal tetrahedral angle (109.5°) to about 102°.

Thus, the correct bond angle of the compound with the maximum number of lone pair of electrons is 102°.

Hence, the correct answer is:

102°