Chapter 9, Problem 9.21P

(a)

Interpretation Introduction

Interpretation:

The condensed electron configurations and Lewis symbols to depict the formation of ions formed from atoms $\text{Cs}$ and $\text{S}$ is to be determined. Also, the formula of the compound formed is to be given.

Concept introduction:

The electronic configuration tells about the distribution of electrons in various atomic orbitals. The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and only the valence shell configuration is written in the expanded form.

Lewis electron-dot symbol is a representation employed to donate the valence electron present in the atom. It includes atom symbol to represent inner electrons and nucleus and the dots represent the valence present in the atom.

Answer to Problem 9.21P

The condensed electronic configuration of ${\text{Cs}}^{+}$ is $\left[\text{Xe}\right]$.

The condensed electronic configuration of ${\text{S}}^{2-}$ is $\left[\text{Ne}\right]3s^{2}3p^6$.

The Lewis orbital diagram is as follows:

The formula of the compound formed is ${\text{Cs}}_{\text{2}}\text{S}$.

Explanation of Solution

The condensed electronic configuration of a cesium atom $\left(\text{Cs}\right)$ is $\left[\text{Xe}\right]6s^1$.

The condensed electronic configuration of the sulfur atom $\left(\text{S}\right)$ is $\left[\text{Ne}\right]3s^{2}3p^4$.

Two cesium atoms lose one electron respectively to form ${\text{Cs}}^{+}$ and to attain noble gas configuration. The two electrons lost by $\text{Cs}$ atoms are gained by sulfur atoms to form ${\text{S}}^{2-}$ ions and to attain noble gas configuration.

The condensed electronic configuration of ${\text{Cs}}^{+}$ is $\left[\text{Xe}\right]$.

The condensed electronic configuration of ${\text{S}}^{2-}$ is $\left[\text{Ne}\right]3s^{2}3p^6$.

Two cesium atoms lose one electron respectively to form ${\text{Cs}}^{+}$ and then react with ${\text{S}}^{2-}$ ions formed from $\text{S}$ to form cesium sulfide $\left({\text{Cs}}_{\text{2}}\text{S}\right)$.

The Lewis orbital diagram is as follows:

Conclusion

$\text{Cs}$ belongs to Group 1A(1) and it loses one electron to form ${\text{Cs}}^{+}$. $\text{S}$ belongs to Group 6A(16) and it gains two electrons to form ${\text{S}}^{2-}$.

(b)

Interpretation Introduction

Interpretation:

The condensed electron configurations, partial orbital diagrams, and Lewis symbols to depict the formation of ions formed from atoms $\text{O}$ and $\text{Ga}$ is to be determined. Also, the formula of the compound formed is to be given.

Concept introduction:

The electronic configuration tells about the distribution of electrons in various atomic orbitals. The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and only the valence shell configuration is written in the expanded form.

The partial orbital diagram is a pictorial representation of the electrons present in an orbital. Each orbital can occupy only two electrons of opposite spin.

Lewis electron-dot symbol is a representation employed to donate the valence electron present in the atom. It includes atom symbol to represent inner electrons and nucleus and the dots represent the valence present in the atom.

Answer to Problem 9.21P

The condensed electronic configuration of ${\text{Ga}}^{3+}$ is $\left[\text{Ar}\right]3d^{10}$.

The condensed electronic configuration of ${\text{O}}^{\text{2}}{}^{-}$ is $\left[\text{He}\right]2s^{2}2p^6$.

The Lewis orbital diagram is as follows:

The formula of the compound formed is ${\text{Ga}}_2{\text{O}}_3$.

Explanation of Solution

The condensed electronic configuration of gallium atom $\left(\text{Ga}\right)$ is $\left[\text{Ar}\right]3d^{10}4s^{2}4p^1$.

The condensed electronic configuration of oxygen atom $\left(\text{O}\right)$ is $\left[\text{He}\right]2s^{2}2p^4$.

Two gallium atoms lose three electrons respectively to form ${\text{Ga}}^{3+}$ and to attain noble gas configuration. The six electrons lost by two $\text{Ga}$ atoms are gained by three oxygen atoms to form ${\text{O}}^{2-}$ ions and to attain noble gas configuration.

The condensed electronic configuration of ${\text{Ga}}^{3+}$ is $\left[\text{Ar}\right]3d^{10}$.

The condensed electronic configuration of ${\text{O}}^{\text{2}}{}^{-}$ is $\left[\text{He}\right]2s^{2}2p^6$.

Two gallium atoms lose three electrons respectively to form ${\text{Ga}}^{3+}$ and then react with three ${\text{O}}^{\text{2}}{}^{-}$ ions formed from three $\text{O}$ to form gallium oxide $\left({\text{Ga}}_2{\text{O}}_3\right)$.

The Lewis orbital diagram is as follows:

Conclusion

$\text{Ga}$ belongs to Group 3A(13) and it loses three electrons to form ${\text{Ga}}^{3+}$. $\text{O}$ belongs to Group 6A(16) and it gains two electrons to form ${\text{O}}^{\text{2}}{}^{-}$.

(c)

Interpretation Introduction

Interpretation:

The condensed electron configurations, partial orbital diagrams, and Lewis symbols to depict the formation of ions formed from atoms $\text{N}$ and $\text{Mg}$ is to be determined. Also, the formula of the compound formed is to be given.

Concept introduction:

The electronic configuration tells about the distribution of electrons in various atomic orbitals. The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and only the valence shell configuration is written in the expanded form.

The partial orbital diagram is a pictorial representation of the electrons present in an orbital. Each orbital can occupy only two electrons of opposite spin.

Lewis electron-dot symbol is a representation employed to donate the valence electron present in the atom. It includes atom symbol to represent inner electrons and nucleus and the dots represent the valence present in the atom.

Answer to Problem 9.21P

The condensed electronic configuration of $\text{Mg}$ is $\left[\text{Ne}\right]$.

The condensed electronic configuration of ${\text{N}}^{3-}$ is $\left[\text{He}\right]2s^{2}2p^6$.

The Lewis orbital diagram is as follows:

The formula of the compound formed is ${\text{Mg}}_{\text{3}}{\text{N}}_2$.

Explanation of Solution

The condensed electronic configuration of magnesium atom $\left(\text{Mg}\right)$ is $\left[\text{Ne}\right]3s^2$.

The condensed electronic configuration of nitrogen atom $\left(\text{N}\right)$ is $\left[\text{He}\right]2s^{2}2p^3$.

Three magnesium atoms lose two electrons respectively to form ${\text{Mg}}^{2+}$ and to attain noble gas configuration. The six electrons lost by three $\text{Mg}$ atoms are gained by two nitrogen atoms to form ${\text{N}}^{3-}$ ions and to attain noble gas configuration.

The condensed electronic configuration of $\text{Mg}$ is $\left[\text{Ne}\right]$.

The condensed electronic configuration of ${\text{N}}^{3-}$ is $\left[\text{He}\right]2s^{2}2p^6$.

Three magnesium atoms lose two electrons respectively to form ${\text{Mg}}^{2+}$ and then react with two ${\text{N}}^{3-}$ ions formed from three $\text{N}$ to form magnesium nitride $\left({\text{Mg}}_{\text{3}}{\text{N}}_2\right)$.

The Lewis orbital diagram is as follows:

Conclusion

$\text{Mg}$ belongs to Group 2A(2) and it loses two electrons to form ${\text{Mg}}^{2+}$. $\text{N}$ belongs to Group 5A(15) and it gains three electrons to form ${\text{N}}^{3-}$.

(d)

Interpretation Introduction

Interpretation:

The condensed electron configurations, partial orbital diagrams, and Lewis symbols to depict the formation of ions formed from atoms $\text{Br}$ and $\text{Li}$ is to be determined. Also, the formula of the compound formed is to be given.

Concept introduction:

The electronic configuration tells about the distribution of electrons in various atomic orbitals. The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and only the valence shell configuration is written in the expanded form.

The partial orbital diagram is a pictorial representation of the electrons present in an orbital. Each orbital can occupy only two electrons of opposite spin.

Lewis electron-dot symbol is a representation employed to donate the valence electron present in the atom. It includes atom symbol to represent inner electrons and nucleus and the dots represent the valence present in the atom.

Answer to Problem 9.21P

The condensed electronic configuration of ${\text{Li}}^{+}$ is $\left[\text{He}\right]$.

The condensed electronic configuration of ${\text{Br}}^{-}$ is $\left[\text{Ar}\right]3d^{10}4s^{2}4p^6$.

The Lewis orbital diagram is as follows:

The formula of the compound formed is $\text{LiBr}$.

Explanation of Solution

The condensed electronic configuration of a lithium atom $\left(\text{Li}\right)$ is $\left[\text{He}\right]2s^1$.

The condensed electronic configuration of the bromine atom $\left(\text{Br}\right)$ is $\left[\text{Ar}\right]3d^{10}4s^{2}4p^5$.

Lithium atom loses one electron to form ${\text{Li}}^{+}$ and to attain noble gas configuration. The electron is gained by the bromine atom to form ${\text{Br}}^{-}$ ions and to attain noble gas configuration.

The condensed electronic configuration of ${\text{Li}}^{+}$ is $\left[\text{He}\right]$.

The condensed electronic configuration of ${\text{Br}}^{-}$ is $\left[\text{Ar}\right]3d^{10}4s^{2}4p^6$.

Lithium atom loses one electron to form ${\text{Li}}^{+}$ and then react with ${\text{Br}}^{-}$ ion formed from $\text{Br}$ to form lithium bromide $\left(\text{LiBr}\right)$.

The Lewis orbital diagram is as follows:

Conclusion

$\text{Li}$ belongs to Group 1A(1) and it loses one electron to form ${\text{Li}}^{+}$. $\text{Br}$ belongs to Group 7A(17) and it gains one electron to form ${\text{Br}}^{-}$.