Question

The correct order towards bond angle is
A) \[sp < s{p^2} < s{p^3}\]
B) \[s{p^2} < sp < s{p^3}\]
C) \[s{p^3} < s{p^2} < sp\]
D) Bond angle does not depend on hybridization

Answer 1

Hint: The bond angle is dependent on the hybridization of the centrally placed atom. Here, we will first discuss \[sp,s{p^2}\]and \[s{p^3}\]hybridization first and then try to understand the bond angle of each other hybridization.

Complete step by step solution:The \[sp\] hybridized molecules are those that have two electron groups surrounding the centrally placed atom. For example, the carbon dioxide molecule is \[sp\] hybridized because two oxygen atoms surround the Carbon atom. And the bond angle in a \[sp\]hybridized molecule is \[180^\circ \] .
The \[s{p^2}\]hybridized molecules are those that have three electron groups surrounding the centrally placed atom. For example, the \[{\rm{B}}{{\rm{F}}_3}\] molecule is \[s{p^2}\] hybridized because three fluorine atoms surround the centrally placed boron atom. And the bond angle observed in a\[s{p^2}\]hybridized molecule is \[120^\circ \] .
Let's discuss the \[s{p^3}\]hybridization in detail. In this type of molecule, four electron groups surround the centrally placed atom. For example, in the methane (\[{\rm{C}}{{\rm{H}}_{\rm{4}}}\] ) molecule, four hydrogen surrounds the centrally place carbon atom. And the bond angle observed in this type of molecule is \[109^\circ 28'\] .
Therefore, the increasing order of their bond angle is \[s{p^3} < s{p^2} < sp\].

Hence, option C is right

Note: It is to be noted that, according to the VSEPR theory, an \[sp\]hybridized molecule has a linear shape. The shape acquired by a \[s{p^2}\]hybridized molecule is trigonal planar and the shape of a \[s{p^3}\]hybridized molecule is tetrahedral. The presence of lone pairs in these molecules changes the shapes of these molecules.