Chapter 8, Problem 110A

Interpretation Introduction

Interpretation:

The following table needs to be completed.

Formula	Hybrid orbital	Lewis structure
${\text{XeF}}_{\text{4}}$
${\text{TeF}}_{\text{4}}$
${\text{KrF}}_2$
${\text{OF}}_2$

Concept introduction:

Lewis structure is also called as Lewis dot structure. In this structure valance electrons are represented by dot symbol around the central atom. This structure shows the Bonding between molecule and the lone pairs which may occur in the molecule.

Answer to Problem 110A

Formula	Hybrid orbital	Lewis structure
${\text{XeF}}_{\text{4}}$	$s{p}^3{d}^2$
${\text{TeF}}_{\text{4}}$	$s{p}^{3}d$
${\text{KrF}}_2$	$s{p}^{3}d$
${\text{OF}}_2$	$s{p}^3$

Explanation of Solution

Determine the valence electrons which are available for bonding in ${\text{XeF}}_{\text{4}}$. It contains one Xe (8 valence electrons) and 4 fluorine atoms (7 valence electrons). Total number of valance electron is $8+7\times 4=36$. Total number of bonding pair is $\frac{36\text{electrons}}{2\text{electrons}}=16\text{pairs}$. Hence, 16 pairs of electrons are available for bonding. Central atom Xe contains two non bonding pairs of electrons and 4 pairs of binding electrons with four F atoms.

Lewis structure of ${\text{XeF}}_{\text{4}}$ as follows:

The central atom Xe comprises of two lone pairs and four bond pairs. The hybrid orbital of ${\text{XeF}}_{\text{4}}$ is $s{p}^3{d}^2$.

Total valance electrons in ${\text{TeF}}_{\text{4}}$ is $6+7\times 4=34$. Total number of bonding pair is $\frac{34\text{electrons}}{2\text{electrons}}=17\text{pairs}$. Hence, 17 pairs of electrons are available for bonding. Central atom Te contains one non bonding pair of electrons and 4 pairs of bonding electrons with four F atoms. The hybrid orbital of ${\text{TeF}}_{\text{4}}$ is $s{p}^{3}d$.

Lewis structure of ${\text{TeF}}_{\text{4}}$ as follows:

In ${\text{KrF}}_2$ total valance electrons is $8+7\times 2=22$. Total number of bonding pair is $\frac{22\text{electrons}}{2\text{electrons}}=11\text{pairs}$. Hence, 11 pairs of electrons are available for bonding. Central atom Kr contains three non bonding pairs of electrons and 2 pairs of bonding electrons with two F atoms. The hybrid orbital of ${\text{KrF}}_2$ is $s{p}^{3}d$. Lewis structure of ${\text{KrF}}_2$ as follows:

In ${\text{OF}}_2$ total valance electrons is $6+7\times 2=20$. Total number of bonding pair is $\frac{20\text{electrons}}{2\text{electrons}}=10\text{pairs}$. Hence, 10 pairs of electrons are available for bonding. Central atom O contains two non bonding pairs of electrons and 2 pairs of bonding electrons with two F atoms. The hybrid orbital of ${\text{OF}}_2$ is $s{p}^3$. Lewis structure of ${\text{OF}}_2$ as follows:

Conclusion

A process in which atomic orbitals mix and produce new, alike hybrid orbitals are known as hybridization.