Question

\[s{p^3}\] hybridization leads to which shape of the molecule
A) Tetrahedral
B) Octahedral
C) Linear
D) Plane triangle

Answer 1

Hint: The VSEPR theory tells the molecular shapes of molecules based on the count of lone pairs and bond pairs around the central atom.

Complete step by step solution:Let’s discuss the molecular shape acquired by an \[s{p^3}\]hybridized molecule according to VSEPR theory. A\[s{p^3}\]hybridized molecule has four surrounding groups around the central atom. The surrounding groups are bonded atoms and the lone pairs present at the central atom. The shape of an \[s{p^3}\]hybridized molecule is tetrahedral and the bond angle is \[109^\circ 28'\] . Some molecules which exhibit this type of hybridization are methane, ammonia etc.
Let’s discuss other molecular shapes given in the options.
Option B is octahedral shape which is exhibited by molecules possessing \[s{p^3}{d^2}\] hybridization and the bond angle in this type of molecule is \[90^\circ \] . Example, \[{\rm{S}}{{\rm{F}}_{\rm{6}}}\]
Option C is a linear shape which is exhibited by molecules possessing \[sp\] hybridization and the bond angle in this type of molecule is \[180^\circ \] . Example, carbon dioxide
Option D is a plane triangle shape which is exhibited by molecules possessing \[s{p^2}\] hybridization. The bond angle in this type of hybridization is\[120^\circ \] . Some molecules of this type of hybridization are \[{\rm{B}}{{\rm{F}}_{\rm{3}}}\].

Therefore, option A is right.

Note: It is to be noted that, if the count of electron groups is four and there is the presence of lone pair, then the shape of the molecule differs. If three bond pairs and one lone pair are present, the shape of the molecule is pyramidal.