Question

below is the lewis structure of the fluoramine (nh₂f) molecule. :f: h:n:h count the number of bonding pairs and the number of lone pairs around the nitrogen atom. bonding pairs: lone pairs:

Explanation:

Step1: Identify bonding pairs

In the Lewis - structure of \(NH_2F\), the nitrogen atom (\(N\)) is bonded to two hydrogen atoms (\(H\)) and one fluorine atom (\(F\)). Each bond represents a bonding pair. So, the number of bonding pairs around \(N\) is 3.

Step2: Identify lone pairs

Nitrogen has 5 valence electrons. In \(NH_2F\), it uses 3 of its valence electrons for bonding. So, the number of non - bonding (lone) electrons is \(5 - 3=2\), which forms 1 lone pair.

Answer:

bonding pairs: 3
lone pairs: 1