What is the formal charge on the oxygen atom in N₂O (with the atomic order N–N–O)?

• A. 0
• B. +1
• C. -1
• D. -2

Answer: (C)

Verified step by step guidance

1. Identify the Lewis structure of N\_2O with the atomic order N–N–O. This means the molecule is arranged as nitrogen bonded to nitrogen, which is bonded to oxygen.
2. Determine the number of valence electrons for oxygen. Oxygen has 6 valence electrons because it is in group 16 of the periodic table.
3. Count the number of lone pair electrons on the oxygen atom in the Lewis structure. These are the non-bonding electrons localized on oxygen.
4. Count the number of bonding electrons shared between oxygen and the adjacent nitrogen atom. Each bond consists of 2 electrons, but for formal charge, only half of these electrons are assigned to oxygen.
5. Use the formal charge formula for oxygen: \(\text{Formal Charge} = \text{Valence electrons} - \text{Non-bonding electrons} - \frac{1}{2} \times \text{Bonding electrons}\). Substitute the values from the Lewis structure to find the formal charge on oxygen.