Lewis structure of NO₂⁺
16 valence electrons. Two N=O double bonds, with no lone pair on N.
Lewis structure
16 valence electronsFormal charges: N +1
Why this shape
- N has 5 valence electrons. In the Lewis structure it makes two double bonds to O and keeps no lone pair, which leaves it a formal charge of +1.
- Steric number = two sigma bonds + no lone pairs = 2, so N is sp hybridised. A double or triple bond counts once: only its sigma bond uses a hybrid orbital.
- Two electron pairs point in opposite directions, along a line (linear electron geometry). With no lone pairs the atoms take the same shape: linear.
- All the bond pairs repel each other equally, so the angle is the ideal 180°.
- NO₂⁺ is an ion with an overall charge of +1, so it is not described as polar or non-polar.
How to draw it
- Count the valence electrons: N 5 + 2 × O 6 − 1 for the ⁺ charge = 16 valence electrons, 8 pairs.
- Put N in the middle and join it to the two outer atoms with single bonds.
- Give each outer atom lone pairs until it has an octet (H needs only two electrons), then put any electrons left over on the central atom.
- Where an atom is still short of an octet, turn a lone pair of its neighbour into a shared pair: that makes a double or triple bond.
- Result: two N=O double bonds, with no lone pair on N.
- Formal charge = valence electrons − lone pair electrons − number of bonds. Here: N +1.
Class 11, Chapter 4 Chemical Bonding and Molecular Structure.
Lewis structure of NO2+: quick answers
How many valence electrons are in NO2+?
N 5 + 2 × O 6 − 1 for the ⁺ charge = 16 valence electrons, 8 pairs.
What are the formal charges in the Lewis structure of NO2+?
N +1; every other atom is zero. Formal charge = valence electrons - lone pair electrons - number of bonds.
How many lone pairs are in the Lewis structure of NO2+?
4 in all, none on the central N.