Question

Observe the following structure:
 
The formal charges on the atoms 1, 2, 3 respectively are:

• A. \( +1, 0, -1 \)
• B. \( 0, 0, -1 \)
• C. \( -1, 0, +1 \)
• D. \( 0, 0, 0 \)

Hint:

To determine formal charges, use the formula: \[ FC = \text{Valence electrons} - \text{Non-bonding electrons} - \frac{\text{Bonding electrons}}{2} \] Correct calculation ensures proper Lewis structure interpretation.

Answer 1

The Correct Option is B

To determine the formal charges on atoms in the molecule, we use the following formula:

Formal Charge = Valence electrons - (Bonding electrons / 2) - Non-bonding electrons

For the given structure:

   :O: = N - O:

Formal Charge on Atom 1 (Oxygen, 1st atom):

Oxygen normally has 6 valence electrons. It forms two bonds with nitrogen, so it has 2 bonding electrons, and there are 6 non-bonding electrons (3 lone pairs).

Formal charge on Atom 1 = 6 - (2 / 2) - 6 = 6 - 1 - 6 = 0.

Formal Charge on Atom 2 (Nitrogen):

Nitrogen normally has 5 valence electrons. It is bonded to 2 oxygens with a double bond, so it has 4 bonding electrons, and it has 0 non-bonding electrons.

Formal charge on Atom 2 = 5 - (4 / 2) - 0 = 5 - 2 - 0 = 0.

Formal Charge on Atom 3 (Oxygen, 3rd atom):

Oxygen normally has 6 valence electrons. It is bonded to nitrogen with a single bond and has 6 non-bonding electrons (3 lone pairs).

Formal charge on Atom 3 = 6 - (2 / 2) - 6 = 6 - 1 - 6 = -1.

Thus, the formal charges on atoms 1, 2, and 3 are 0, 0, and -1 respectively.