Question

The bond angles ${NO}_2^{+},{NO}_2,{NO}_2^{-}$ are respectively:

• A. ${180}^o,{134}^o,{115}^o$
• B. ${115}^o,{134}^o,{180}^o$
• C. ${134}^o,{180}^o,{130}^o$
• D. ${115}^o,{180}^o,{130}^o$

Answer 1

The correct option is A ${180}^o,{134}^o,{115}^o$

• NO₂⁺ is sp hybridized with no lone pairs and linear geometry. Thus, bond angle will be equal to the ideal bond angle of sp hybridization i.e. 180°.
  
• NO₂ is sp² hybridized with a lone electron which exerts a less repulsion than a lone pair of electrons, so two bonding oxygen atoms are able to spread out more leading to bond angle greater than the ideal of 120° i.e. bond angle will be 134°.
  
• NO₂⁻ is also sp² hybridized but we have 1 lone pair on nitrogen. Lone pair electron repulsion is more than the bonding electrons so the bond angle will be less than 120° i.e. bond angle will be 115°.

Hence, option A is correct.