Which of the following best describes the correct Lewis structure for the $NO+$ ion?

• A. A single bond between $N$ and $O$, with a formal positive charge on $N$
• B. A triple bond between $N$ and $O$, with a formal positive charge on $N$
• C. A triple bond between $N$ and $O$, with a formal positive charge on $O$
• D. A double bond between $N$ and $O$, with a formal positive charge on $N$

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the NO⁺ ion. Nitrogen (N) has 5 valence electrons, oxygen (O) has 6, and since the ion has a positive charge, subtract 1 electron. So, total valence electrons = 5 + 6 - 1 = 10 electrons.
2. Step 2: Draw possible Lewis structures for NO⁺ with different bond orders (single, double, triple bonds) between N and O, and distribute the electrons to satisfy the octet rule as much as possible.
3. Step 3: Calculate the formal charges for each atom in each Lewis structure using the formula: \(\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}\).
4. Step 4: Identify the Lewis structure where the sum of formal charges equals the overall charge (+1) and where the formal charges are minimized and placed on the most appropriate atoms (consider electronegativity).
5. Step 5: Conclude that the correct Lewis structure for NO⁺ is the one with a triple bond between N and O, with the formal positive charge located on the oxygen atom, as this arrangement best satisfies the octet rule and formal charge distribution.