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
$AB_2 E_2$	2	P	Bent	$H_2O$
$AB_3 E_2$	3	2	Q	$ClF_3$
$AB_5 E$	5	R	S	$BrF_5$
$AB_4E_2$	4	2	T	U

	P	Q	R	S	T	U
(a)	2	Square pyramidal	2	T- Shaped	Square planar	$H_2O_2$
(b)	4	T -Shaped	5	Square palnar	Square pyramidal	$SO_3$
(c)	2	T - shaped	1	Square pyramidal	Square planar	$XeF_4$
(d)	3	Square planar	2	T- Shaped	Square pyramidal	$BaCl_3$

• A. a
• B. b
• C. c
• D. d

Answer 1

Answer: (C)

$- H _{2} O$ has 2 lone pairs so $P$ will be 2,
$- ClF _{3}$ has $T$-shape so $Q$ will be $T$-shaped,
$- BrF _{5}$ has one lone pair so $R$ will be 1 ,
$- BrF _{5}$ 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 $XeF _{4}$.