Chapter 11, Problem 11.41P

(a)

Interpretation Introduction

Interpretation:

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom in ${\text{IF}}_2^{-}$ is to be drawn.

Concept introduction:

The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

The partial orbital diagram is the one that shows the distribution of electrons in the valence shell only.

Answer to Problem 11.41P

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom iodine in ${\text{IF}}_2^{-}$ is as follows:

Explanation of Solution

The Lewis structure of ${\text{IF}}_2{}^{-}$ is as follows:

Iodine forms two single bonds with two fluorine atoms and three lone pairs are present on it so the hybridization of iodine in ${\text{IF}}_2{}^{-}$ is $s{p}^{3}d$.

The atomic number of iodine is 53 so its electronic configuration is $\left[\text{Kr}\right]4d^{10}5s^{2}5p^5$.

The partial orbital diagram for an isolated $\text{I}$ atom is as follows:

The partial orbital for hybridized $\text{I}$ atom is as follows:

One s orbital, three p orbitals and one d orbital of central atom iodine combine to form five $s{p}^{3}d$ hybridized orbitals. Iodine has 7 valence electrons and it has one negative charge also that adds one more electron in the valence orbital of iodine in the orbital diagram. The formation of hybrid orbitals can be shown as follows:

Conclusion

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom iodine in ${\text{IF}}_2^{-}$ is as follows:

(b)

Interpretation Introduction

Interpretation:

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom in ${\text{ICl}}_{\text{3}}$ is to be drawn.

Concept introduction:

The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

The partial orbital diagram is the one that shows the distribution of electrons in the valence shell only.

Answer to Problem 11.41P

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom iodine in ${\text{ICl}}_{\text{3}}$ is as follows:

Explanation of Solution

The Lewis structure of ${\text{ICl}}_3$ is as follows:

Iodine forms three single bonds with three chlorine atoms and two lone pairs are present on it so five hybrid orbitals are required. The hybridization of $\text{I}$ in ${\text{ICl}}_3$ is $s{p}^{3}d$.

The atomic number of iodine is 53 so its electronic configuration is $\left[\text{Kr}\right]4d^{10}5s^{2}5p^5$.

The partial orbital diagram for an isolated $\text{I}$ atom is as follows:

The partial orbital for hybridized $\text{I}$ atom is as follows:

One s orbital, three p orbitals and one d orbital of central atom iodine combine to form five $s{p}^{3}d$ hybridized orbitals. The formation of hybrid orbitals can be shown as follows:

Conclusion

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom iodine in ${\text{ICl}}_{\text{3}}$ is as follows:

(c)

Interpretation Introduction

Interpretation:

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom in ${\text{XeOF}}_{\text{4}}$ is to be drawn.

Concept introduction:

The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

The partial orbital diagram is the one that shows the distribution of electrons in the valence shell only.

Answer to Problem 11.41P

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom xenon in ${\text{XeOF}}_{\text{4}}$ is as follows:

Explanation of Solution

The Lewis structure of ${\text{XeOF}}_4$ is as follows:

Xenon forms four single bonds with four fluorine atoms and one double bond with oxygen and one lone pair is present on it so six hybrid orbitals are required. The hybridization of xenon in ${\text{XeOF}}_4$ is $s{p}^3{d}^2$.

The atomic number of xenon is 54 so its electronic configuration is $\left[\text{Kr}\right]4d^{10}5s^{2}5p^6$.

The partial orbital diagram for an isolated $\text{Xe}$ atom is as follows:

The partial orbital for hybridized $\text{Xe}$ atom is as follows:

One s orbital, three p orbitals and two d orbitals of central atom xenon combine to form six $s{p}^3{d}^2$ hybridized orbitals. The formation of hybrid orbitals can be shown as follows:

Conclusion

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom xenon in ${\text{XeOF}}_{\text{4}}$ is as follows:

(d)

Interpretation Introduction

Interpretation:

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom in ${\text{BHF}}_2$ is to be drawn.

Concept introduction:

The atomic orbital is the wave function that is used to find the probability to find an electron around the nucleus of an atom. It is the space around the nucleus of an atom where the electrons are supposed to be found.

Hybridization is the process of intermixing of atomic orbital of slightly different energies to form hybrid orbitals that have similar energy. These orbital have lower energy and more stability than the atomic orbital.

The partial orbital diagram is the one that shows the distribution of electrons in the valence shell only.

Answer to Problem 11.41P

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom boron in ${\text{BHF}}_2$ is as follows:

Explanation of Solution

The Lewis structure of ${\text{BHF}}_2$ is as follows:

Boron forms one single bond with hydrogen and two single bonds with two fluorine atoms so three hybrid orbitals are required. The hybridization of boron in ${\text{BHF}}_2$ is $s{p}^2$.

The atomic number of boron is 5 so its electronic configuration is $1s^{2}2s^{2}2p^1$.

The partial orbital diagram for an isolated $\text{B}$ atom is as follows:

The partial orbital for hybridized $\text{B}$ atom is as follows:

One s orbital and two p orbitals of central atom boron combine to form three $s{p}^2$ hybridized orbitals. The formation of hybrid orbitals can be shown as follows:

Conclusion

The partial orbital diagram that shows the formation of hybrid orbitals from the atomic orbitals of the central atom boron in ${\text{BHF}}_2$ is as follows: