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

Step 1: Identify lone pairs in the given compounds.
- H$_2$SO$_4$ has no lone pairs on the central atom.
- HNO$_3$ has one lone pair on the central nitrogen atom.
- O$_3$ has one lone pair on the central oxygen atom.
- NF$_3$ has one lone pair on the central nitrogen atom.

Step 2: Identify the compound with the most lone pairs.
Among the given compounds, NF$_3$ has the highest number of lone pairs on the central atom.
Step 3: Determine the bond angle.
In NF$_3$, with three bonding pairs and one lone pair, the bond angle is approximately 102$^\circ$.
Step 4: Conclusion.
The correct bond angle is 102$^\circ$, which corresponds to option (1).