Lewis Structures

Step 1: Understanding the electron configuration.
The Lewis structure of NO F shows that nitrogen (N) forms a single bond with oxygen (O) and fluorine (F). Nitrogen has one lone pair of electrons, while oxygen and fluorine both have three lone pairs each.
Step 2: Counting the lone pairs.
- Nitrogen: 1 lone pair - Oxygen: 3 lone pairs - Fluorine: 3 lone pairs
So the total number of lone pairs is .
Step 3: Conclusion.
The total number of lone pairs of electrons in NO F is 8.

Step 1: Understanding BF reactivity.
BF is a Lewis acid and reacts with Lewis bases like amines (C H N), which can donate electron pairs.
Step 2: Analyzing the options.
(A) C H N: Correct — BF reacts readily with amines like C H N (an amine), forming a Lewis acid-base complex.
(B) SnCl : Incorrect — SnCl is a reducing agent, not a Lewis base.
(C) SO : Incorrect — SO is a strong Lewis acid but does not readily react with BF .
(D) (C H N)–SnCl : Incorrect — This is not a common reaction.
Step 3: Conclusion.
The correct answer is (A) C H N, as BF readily reacts with amines to form complexes.