Chapter 8, Problem 8.77P

(a)

Interpretation Introduction

Interpretation:

The charge and full ground state electron configuration of the ion likely to be formed by $\text{Al}$ is to be determined.

Concept introduction:

The electronic configuration of an atom describes how the electrons are ditributed in its atom among various shells and subshells. It is used to predict the chemical, physical, electrical and magnetic properties of the substance. The full electronic configuration of an atom tells about the distribution of electrons in the various atomic orbitals.

Answer to Problem 8.77P

The charge of monoatomic ion likely to be formed by $\text{Al}$ atom is $+3$.

The full ground state electron configuration of the ion likely to be formed by $\text{Al}$ is $1s^{2}2s^{2}2p^6$.

Explanation of Solution

The atomic number of so its ground state electronic configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^1$. Its configuration is just three electrons more of the stable noble gas configuration of neon so it loses three electrons to become ${\text{Al}}^{3+}$ whose full ground state electron configuration is $1s^{2}2s^{2}2p^6$.

The ion formation occurs as follows:

$\text{Al}\left(1s^{2}2s^{2}2p^{6}3s^{2}3p^1\right)-3{\text{e}}^{-}\to {\text{Al}}^{3+}\left(1s^{2}2s^{2}2p^6\right)$

So the charge on the ion formed by $\text{Al}$ is $+3$ and its full ground state electron configuration is $1s^{2}2s^{2}2p^6$.

Conclusion

The charge of monoatomic ion likely to be formed by $\text{Al}$ atom is $+3$ and the full ground state electron configuration of the ion likely to be formed by $\text{Al}$ is $1s^{2}2s^{2}2p^6$.

(b)

Interpretation Introduction

Interpretation:

The charge and full ground state electron configuration of the ion likely to be formed by $\text{S}$ is to be determined.

Concept introduction:

The electronic configuration of an atom describes how the electrons are ditributed in its atom among various shells and subshells. It is used to predict the chemical, physical, electrical and magnetic properties of the substance. The full electronic configuration of an atom tells about the distribution of electrons in the various atomic orbitals.

Answer to Problem 8.77P

The charge of monoatomic ion likely to be formed by $\text{S}$ atom is $-2$.

The full ground state electron configuration of the ion likely to be formed by $\text{S}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

Explanation of Solution

The atomic number of sulphur is 16 so its ground state electronic configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$. Its configuration is just two electrons short of the stable noble gas configuration of argon so it gains two electrons to become ${\text{S}}^{2-}$ whose full ground state electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

The ion formation occurs as follows:

$\text{S}\left(1s^{2}2s^{2}2p^{6}3s^{2}3p^4\right)+2{\text{e}}^{-}\to {\text{S}}^{2-}\left(1s^{2}2s^{2}2p^{6}3s^{2}3p^6\right)$

So the charge on the ion formed by $\text{S}$ is $-2$ and its full ground state electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

Conclusion

The charge of monoatomic ion likely to be formed by $\text{S}$ atom is $-2$ and the full ground state electron configuration of the ion likely to be formed by $\text{S}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

(c)

Interpretation Introduction

Interpretation:

The charge and full ground state electron configuration of the ion likely to be formed by $\text{Sr}$ is to be determined.

Concept introduction:

The electronic configuration of an atom describes how the electrons are ditributed in its atom among various shells and subshells. It is used to predict the chemical, physical, electrical and magnetic properties of the substance. The full electronic configuration of an atom tells about the distribution of electrons in the various atomic orbitals.

Answer to Problem 8.77P

The charge of monoatomic ion likely to be formed by $\text{Sr}$ atom is $\text{+2}$.

The full ground state electron configuration of the ion likely to be formed by $\text{Sr}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.

Explanation of Solution

The atomic number of strontium is 38 so its ground state electronic configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^2$. Its configuration is two electrons more of the stable noble gas configuration of krypton so it loses two electrons to become ${\text{Sr}}^{2+}$ whose full ground state electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.

The ion formation occurs as follows:

$\text{Sr}\left(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^2\right)-\text{}2{\text{e}}^{-}\to {\text{Sr}}^{2+}\left(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6\right)$

So the charge on the ion formed by $\text{Sr}$ is $\text{+2}$ and its full ground state electron configuration is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.

Conclusion

The charge of monoatomic ion likely to be formed by $\text{Sr}$ atom is $\text{+2}$ and the full ground state electron configuration of the ion likely to be formed by $\text{Sr}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.