Respuesta :
Explanation:
Formula to calculate hybridization is as follows.
Hybridization = [tex]\frac{1}{2}[V+N-C+A][/tex]
where,
V = number of valence electrons present in central atom
N = number of monovalent atoms bonded to central atom
C = charge of cation
A = charge of anion
So, hybridization of [tex]BeCl_{2}[/tex] is as follows.
Hybridization = [tex]\frac{1}{2}[V + N - C + A][/tex]
= [tex]\frac{1}{2}[2 + 2][/tex]
= 2
Hybridization of [tex]BeCl_{2}[/tex] is sp. Therefore, [tex]BeCl_{2}[/tex] is a linear molecule. There will be only two electron groups through which Be is attached.
Similarly, hybridization of [tex]XeF_{2}[/tex] is calculated as follows.
Hybridization = [tex]\frac{1}{2}[V + N - C + A][/tex]
= [tex]\frac{1}{2}[8 + 2][/tex]
= 5
Therefore, hybridization of [tex]XeF_{2}[/tex] is [tex]sp^{3}d. Therefore, [tex]XeF_{2}[/tex] is also a linear molecule. Though there are three lone pair of electrons present on a xenon atom and it is further attached with fluorine atoms through two electron pairs. Hence, there are in total five electron groups.
Thus, we can conclude that out of the given options [tex]XeF_{2}[/tex] is the correct examples of linear molecules for five electron groups.
