Question

draw the lewis structure of the following molecule. use it to give the information

n₂h₂

number of single bonds

number of double bonds

number of sigma bonds

number of pi bonds

number of unshared electrons

Explanation:

Step1: Calculate total valence electrons

N has 5 valence electrons, H has 1. For \(N_2H_2\), total valence electrons \(= 2\times5+2\times1=12\).

Step2: Draw the Lewis structure

The Lewis structure of \(N_2H_2\) is \(H - N=N - H\).

Step3: Analyze bonds

• Single bonds: Each \(N - H\) is a single bond. There are 2 single bonds.
• Double bonds: The \(N=N\) is a double bond. There is 1 double bond.
• Sigma (\(\sigma\)) bonds: A single bond is 1 \(\sigma\) bond, a double bond has 1 \(\sigma\) bond. So total \(\sigma\) bonds \(=2 + 1=3\).
• Pi (\(\pi\)) bonds: A double bond has 1 \(\pi\) bond. So there is 1 \(\pi\) bond.
• Unshared electrons: Each N has 1 lone pair (2 unshared electrons). Total unshared electrons \(=2\times2 = 4\).

Answer:

Number of single bonds: 2
Number of double bonds: 1
Number of sigma bonds: 3
Number of pi bonds: 1
Number of unshared electrons: 4