Question

Given below is the table showing shapes of some molecules having lone pairs of electrons. Fill up the blanks left in it.

Molecular type	$bp$	$lp$	Shape	Example
$A{B}_2{E}_2$	2	P	Bent	$H_{2}O$
$A{B}_3{E}_2$	3	2	Q	$Cl{F}_3$
$A{B}_{5}E$	5	R	S	$Br{F}_5$
$A{B}_4{E}_2$	4	2	T	U

	P	Q	R	S	T	U
(a)	2	Square pyramidal	2	T- Shaped	Square planar	$H_2{O}_2$
(b)	4	T -Shaped	5	Square palnar	Square pyramidal	$S{O}_3$
(c)	2	T - shaped	1	Square pyramidal	Square planar	$Xe{F}_4$
(d)	3	Square planar	2	T- Shaped	Square pyramidal	$BaC{l}_3$

• A. a
• B. b
• C. c
• D. d

Answer 1

Answer: (C)

$-H_{2}O$ has 2 lone pairs so $P$ will be 2,
$-Cl{F}_3$ has $T$-shape so $Q$ will be $T$-shaped,
$-Br{F}_5$ has one lone pair so $R$ will be 1 ,
$-Br{F}_5$ has the Square pyramidal shape so $S$ will be pyramidal shape,
$-4$ bond pairs and 2 lone pairs means shape will be the square planner and one of the examples of this type is $Xe{F}_4$.