Numford
Hybridisation

Hybridisation of NO₂⁺

N is sp hybridised (hybridization by the VSEPR count): 2 sigma bonds and no lone pairs give a linear shape, bond angle 180°.

ONO
  • N
  • O

NO₂⁺Nitronium ion

Linear

AB₂: 2 bond pairs, no lone pairs

  • Hybridisationsp
  • Bond angle180°
  • Polarityion, charge +1

Why this shape

  1. 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.
  2. 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.
  3. Two electron pairs point in opposite directions, along a line (linear electron geometry). With no lone pairs the atoms take the same shape: linear.
  4. All the bond pairs repel each other equally, so the angle is the ideal 180°.
  5. NO₂⁺ is an ion with an overall charge of +1, so it is not described as polar or non-polar.

Lewis structure

16 valence electrons
NOO+

Formal charges: N +1

Working

Why this hybridisation and shape

  1. 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.
  2. 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.
  3. Two electron pairs point in opposite directions, along a line (linear electron geometry). With no lone pairs the atoms take the same shape: linear.
  4. All the bond pairs repel each other equally, so the angle is the ideal 180°.
  5. NO₂⁺ is an ion with an overall charge of +1, so it is not described as polar or non-polar.

Class 11, Chapter 4 Chemical Bonding and Molecular Structure.

Questions

Hybridisation of NO2+: quick answers

What is the hybridisation of NO2+?

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.

What is the shape of NO2+ and its bond angle?

Linear, with a bond angle of 180 degrees. 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°.

How many lone pairs are on the central atom of NO2+?

None. 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.

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