Question

Find the formal charge of \( O \), \( O \), \( O \), and \( N \) respectively.

• A. 0, +1, -1, +2
• B. -1, -1, 0, +1
• C. -1, 0, +2, +1
• D. +1, -1, 0, -1

Hint:

When calculating formal charges, keep track of the valence electrons, lone pairs, and bonds for each atom involved.

Answer 1

The Correct Option is C

Step 1: Formal charge calculation.
The formal charge is calculated as: \[ \text{Formal charge} = V - (L + \frac{B}{2}) \] where \( V \) is the valence electrons of the atom, \( L \) is the number of lone pair electrons, and \( B \) is the number of bonding electrons. - For \( O_1 \) (the leftmost oxygen): The formal charge is -1. - For \( O_2 \) (the oxygen in the middle): The formal charge is 0. - For \( O_3 \) (the rightmost oxygen): The formal charge is +2. - For \( N \) (the nitrogen): The formal charge is +1. Step 2: Conclusion.
The formal charges are: \( O_1 = -1 \), \( O_2 = 0 \), \( O_3 = +2 \), \( N = +1 \). Final Answer: \[ \boxed{-1, 0, +2, +1} \]