part 2 of 3\nselect the single best geometry of no₂⁻ ion.\ntrigonal planar\ntetrahedral\ntrigonal…

part 2 of 3\nselect the single best geometry of no₂⁻ ion.\ntrigonal planar\ntetrahedral\ntrigonal pyramidal\nbent\npart 3 of 3\nenter the hybridization of the n atom in the no₂⁻ ion.

part 2 of 3\nselect the single best geometry of no₂⁻ ion.\ntrigonal planar\ntetrahedral\ntrigonal pyramidal\nbent\npart 3 of 3\nenter the hybridization of the n atom in the no₂⁻ ion.

Answer

Explanation:

Step1: Determine the Lewis - structure of $NO_{2}^{-}$

N has 5 valence electrons, each O has 6 valence electrons, and there is an extra electron due to the - 1 charge. So the total number of valence electrons is $5 + 2\times6+1=18$. The Lewis - structure has N as the central atom with a double - bond to one O and a single - bond to the other O, and a lone pair on N.

Step2: Use VSEPR theory for geometry

The steric number of the central N atom is the sum of the number of bonding pairs and lone pairs. There are 2 bonding pairs and 1 lone pair around N. According to VSEPR theory, a steric number of 3 with 1 lone pair gives a bent molecular geometry.

Step3: Determine the hybridization of N

The steric number of N is 3. When the steric number is 3, the hybridization is $sp^{2}$.

Answer:

Part 2 of 3: D. Bent Part 3 of 3: $sp^{2}$