Question

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part a

what is the formal charge of nitrogen in this structure?

0
+2
-1
+1

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 its neutral state, \( N \) is the number of non - bonding (lone pair) electrons, and \( B \) is the number of bonding electrons.
For nitrogen (\( N \)), \( V=5 \) (since nitrogen is in group 15 of the periodic table and has 5 valence electrons).

Step2: Determine \( N \) and \( B \) for nitrogen in the given structure

In the structure \( H - C-\ddot{N}=\ddot{O}: \), for the nitrogen atom:

• The number of non - bonding electrons \( N = 2 \) (one lone pair).
• The number of bonding electrons \( B = 6 \) (a double bond (\( 4 \) electrons) and a single bond (\( 2 \) electrons) to carbon).

Step3: Calculate the formal charge

Substitute the values into the formula:

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Answer:

0