Question

Match the column I with column II and mark the appropriate choice.

Column I	Column II
(A) $Xe{F}_4$	(i) $s{p}^3{d}^2$
(B) $Xe{F}_6$	(ii) $s{p}^3{d}^3$
(C) $XeO{F}_2$	(iii) $s{p}^{3}d$
(D) $Xe{O}_3$	(iv) $s{p}^3$

• A. (A) $\to$ (i); (B) $\to$ (ii); (C) $\to$ (iii); (D) $\to$ (iv)
• B. (A) $\to$ (iv); (B) $\to$ (iii); (C) $\to$ (ii); (D) $\to$ (i)
• C. (A) $\to$ (iii); (B) $\to$ (iv); (C) $\to$ (i); (D) $\to$ (ii)
• D. (A) $\to$ (ii); (B) $\to$ (iii); (C) $\to$ (iv); (D) $\to$ (i)

Answer 1

The correct option is A (A) $\to$ (i); (B) $\to$ (ii); (C) $\to$ (iii); (D) $\to$ (iv)

Hybridization of an atom is identified by caliculating the sum of sigma bonds and lone pairs.

If sum of sigma bonds and lone pairs is 2. $sp$ hybridization

If sum of sigma bonds and lone pairs is 3. $s{p}^2$ hybridization

If sum of sigma bonds and lone pairs is 4. $s{p}^3$ hybridization.$Xe{O}_3$ has 3 sigma bonds and 1 lone pair.So the sum is 4.So it is $s{p}^3$

If sum of sigma bonds and lone pairs is 5. $s{p}^{3}d$ hybridization.$XeO{F}_2$ has 3 sigma bonds and two lone pairs ,the sum is 5.So it is $S{P}^{3}d$.

If sum of sigma bonds and lone pairs is 6 .$s{p}^3{d}^2$ hybridization.$Xe{F}_4$ has 4 sigma bonds and 2 lone pair.So the sum is 6.So it is $s{p}^3{d}^2$

If sum of sigma bonds and lone pairs is 7. $s{p}^3{d}^2$ hybridization.$Xe{F}_6$ has 6 sigma bonds and 1 lone pair.So the sum is 7.So it is $s{p}^3{d}^3$

So the option A is correct match.

Hence option A is correct.