Question

$\large\red{Neet\:Jee}$

⏺️⏺️ Explain option 2 & 3⏺️​⏺️​

Answer 1

Answer :

Nitrate ion = NO₃ˉ

Structure : Refer to the attachment$.$

(I) Formal charge on N :

➝ FC = V - L - 1/2(S)

• Valence eˉ of N = 5
• Lone pair eˉ = 0
• Shared eˉ in bonding = 8

➝ FC = 5 - 0 - 1/2(8)

➝ FC = 5 - 4

➝ FC = +1

(II) Bond order of NO bond :

➝ BO = bond pairs/no. of bonds

➝ BO = 4/3 = 1.33

(III) Average formal charge of O :

• Formal charge of O₁ :

➝ V - L - 1/2(S)

➝ 6 - 4 - 1/2(4)

➝ 6 - 4 - 2

➝ 0

• Formal charge of O₂ :

➝ V - L - 1/2(S)

➝ 6 - 6 - 1/2(2)

➝ 0 - 1

➝ -1

• Formal charge of O₃ :

➝ V - L - 1/2(S)

➝ 6 - 6 - 1/2(2)

➝ 0 - 1

➝ -1

• Average FC of O :

➝ Avg. = net charge/total atom

➝ Avg. = -2/3

(IV) π Bond :

It is clear from the structure that, there is only 1π bond.

Option (II) is correct.