Question

question 3 (2 points)
what is the formal charge on atom 1 for the following lewis structure?
-2
-1
+1
+2
0

Explanation:

Step1: Recall the formula for formal charge

The formula for formal charge is \(FC = V - N - \frac{B}{2}\), where \(V\) is the number of valence electrons of the atom in isolation, \(N\) is the number of non - bonding electrons, and \(B\) is the number of bonding electrons.
For nitrogen (atom 1), \(V = 5\) (since nitrogen is in group 15 and has 5 valence electrons).

Step2: Determine \(N\) and \(B\) for atom 1

Looking at the Lewis structure, for atom 1 (N):

• \(N=0\) (no non - bonding electrons shown as lone pairs on the N atom in the relevant part for the formula calculation).
• \(B = 8\) (4 bonds, each bond has 2 electrons, so \(4\times2=8\)).

Step3: Calculate the formal charge

Substitute into the formula: \(FC=5 - 0-\frac{8}{2}\).
First, calculate \(\frac{8}{2}=4\). Then \(FC = 5-0 - 4=+1\).

Answer:

+1