Question

Find the total number of planar molecules among the following.
$C{O}_3^{2-},\stackrel{.}{C}{H}_3,\stackrel{.}{C}{F}_3,BeC{l}_2,B_2{H}_6,H_{3}P{O}_2,S{O}_3,B{F}_3,Xe{F}_4$

Answer 1

$C{O}_3^{2-}$ - Here the central atom $C$ is $s{p}^2$ hybridised and hence it is planar.

$\stackrel{.}{C}{H}_3$ - Here the central atom $C$ is $s{p}^2$ hybridised and hence it is also planar.

$\stackrel{.}{C}{F}_3$ - Here the central atom $C$ is $s{p}^3$ hybridised. Hence, its shape is pyramidal.

$BeC{l}_2$ - Here the central atom $Be$ is $sp$ hybridised. So, its shape is linear and also planar.

$B_2{H}_6$ - Here both the $B$ atoms are in $s{p}^3$ hybridization state and each boron contains two types of boron-hydrogen bond. The bridging hydrogen atoms are not in the plane of the molecule.

$H_{3}P{O}_2$ - Here the central atom $P$ is $s{p}^3$ hybridised. Thus, it is tetrahedral.

$S{O}_3$ - Here the central atom $S$ is $s{p}^2$ hybridised. So, it is also planar.

$B{F}_3$ - Here also the central atom $B$ is $s{p}^2$ hybridised. Thus, it is also planar.

$Xe{F}_4$ - Here the central atom $Xe$ is $s{p}^3{d}^2$ hybridised. But, it has two lone pairs of electrons. Thus, its shape is square planar.