Question

drag the electrons and bonds to the correct place in arrangement of atoms to construct the correct lewis structure for $n_{2}h_{2}$. use lines for bonds and pairs of dots for unbonded pairs.

Explanation:

Step1: Calculate the total valence electrons

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

Step2: Determine the bonding

Each N - H bond uses 2 electrons. Let's assume the structure \(H - N=N - H\). The N - N double bond uses 4 electrons. Each N - H bond (2 bonds) uses \(2\times2 = 4\) electrons. So far, \(4 + 4=8\) electrons are used.

Step3: Add lone pairs

We have \(12-8 = 4\) electrons left. Each N atom gets one lone pair (2 electrons per lone pair)

Answer:

The Lewis structure is \(H-\dot{N}=\dot{N}-H\) (where the dots represent the lone pairs on each N atom)