Which of the following statements correctly describes the Lewis dot structure of the NO_2^+ ion?

• A. NO_2^+ has a bent structure with one N–O single bond and one N–O double bond.
• B. NO_2^+ has a trigonal planar structure with three N–O bonds.
• C. NO_2^+ has a linear structure with both N–O bonds equivalent and no lone pairs on nitrogen.
• D. NO_2^+ has a linear structure with a lone pair on nitrogen.

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the NO_2^+ ion. Nitrogen (N) has 5 valence electrons, each oxygen (O) has 6 valence electrons, and since the ion has a +1 charge, subtract one electron from the total count.
2. Step 2: Draw a skeletal structure with nitrogen as the central atom bonded to two oxygen atoms. Connect the atoms with single bonds initially.
3. Step 3: Distribute the remaining valence electrons to satisfy the octet rule for oxygen atoms first, then place any leftover electrons on nitrogen.
4. Step 4: Check the formal charges on each atom. Adjust the bonding by forming double bonds if necessary to minimize formal charges and achieve resonance structures if applicable.
5. Step 5: Determine the molecular geometry using VSEPR theory. Count the regions of electron density around nitrogen (bonding and lone pairs) to predict the shape and bond equivalency.