Chapter 5, Problem 80E

Interpretation Introduction

(a)

Interpretation:

The electron configuration for ${\text{Br}}^{-}$ ion with the help of periodic table is to be predicted.

Concept introduction:

Ionic charge is defined as the charge possesses by an ion that result by the gain or loss of an electron by an atom or a molecule. Metals are electropositive in nature because they lose electrons from their outermost shells. Nonmetals are electronegative in nature because they gain electrons in their outermost shells.

Answer to Problem 80E

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

Explanation of Solution

The given negative ion is ${\text{Br}}^{-}$.

Bromine belongs to the group $17$ of a periodic table. The atomic number of bromine is $35$. The atomic number corresponds to the number of electrons present in an element. Electronic configuration tells about the arrangement of an electron in each subshell and orbit of an atom. The electronic configuration of $\text{Br}$ is $\left[\text{Ar}\right]4s^{2}4d^{10}4p^5$. It gain one electron and act as an ${\text{Br}}^{-}$ ion. Therefore, the predicted electronic configuration of ${\text{Br}}^{-}$ is $\left[\text{Ar}\right]4s^{2}4d^{10}4p^6$.

Conclusion

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

Interpretation Introduction

(b)

Interpretation:

The electron configuration for ${\text{Te}}^{2-}$ ion with the help of periodic table is to be predicted.

Concept introduction:

Ionic charge is defined as the charge possesses by an ion that result by the gain or loss of an electron by an atom or a molecule. Metals are electropositive in nature because they lose electrons from their outermost shells. Nonmetals are electronegative in nature because they gain electrons in their outermost shells.

Answer to Problem 80E

The predicted electronic configuration of ${\text{Te}}^{2-}$ is $\left[\text{Kr}\right]4d^{10}5s^{2}5p^6$.

Explanation of Solution

The given negative ion is ${\text{Te}}^{2-}$.

Tellurium belongs to the group $16$ of a periodic table. The atomic number of tellurium is $52$. The atomic number corresponds to the number of electrons present in an element. Electronic configuration tells about the arrangement of an electron in each subshell and orbit of an atom. The electronic configuration of $\text{Te}$ is $\left[\text{Kr}\right]4d^{10}5s^{2}5p^4$. It gain two electrons and act as an ${\text{Te}}^{2-}$ ion. Therefore, the predicted electronic configuration of ${\text{Te}}^{2-}$ is $\left[\text{Kr}\right]4d^{10}5s^{2}5p^6$.

Conclusion

The predicted electronic configuration of ${\text{Te}}^{2-}$ is $\left[\text{Kr}\right]4d^{10}5s^{2}5p^6$.

Interpretation Introduction

(c)

Interpretation:

The electron configuration for ${\text{As}}^{3-}$ ion with the help of periodic table is to be predicted.

Concept introduction:

Ionic charge is defined as the charge possesses by an ion that result by the gain or loss of an electron by an atom or a molecule. Metals are electropositive in nature because they lose electrons from their outermost shells. Nonmetals are electronegative in nature because they gain electrons in their outermost shells.

Answer to Problem 80E

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

Explanation of Solution

The given negative ion is ${\text{As}}^{3-}$.

Arsenic belongs to the group $15$ of a periodic table. The atomic number of arsenic is $33$. The atomic number corresponds to the number of electrons present in an element. Electronic configuration tells about the arrangement of an electron in each subshell and orbit of an atom. The electronic configuration of $\text{As}$ is $\left[\text{Ar}\right]3d^{10}4s^{2}4p^3$. It gain three electrons and act as an ${\text{As}}^{3-}$ ion. Therefore, the predicted electronic configuration of ${\text{As}}^{3-}$ is $\left[\text{Ar}\right]4s^{2}4p^6$.

Conclusion

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

Interpretation Introduction

(d)

Interpretation:

The electron configuration for ${\text{O}}^{2-}$ ion with the help of periodic table is to be predicted.

Concept introduction:

Ionic charge is defined as the charge possesses by an ion that result by the gain or loss of an electron by an atom or a molecule. Metals are electropositive in nature because they lose electrons from their outermost shells. Nonmetals are electronegative in nature because they gain electrons in their outermost shells.

Answer to Problem 80E

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

Explanation of Solution

The given negative ion is ${\text{O}}^{2-}$.

Oxygen belongs to the group $16$ of a periodic table. The atomic number of oxygen is $8$. The atomic number corresponds to the number of electrons present in an element. Electronic configuration tells about the arrangement of an electron in each subshell and orbit of an atom. The electronic configuration of $\text{O}$ is $\left[\text{He}\right]2s^{2}2p^4$. It gain two electrons and act as an ${\text{O}}^{2-}$ ion. Therefore, the predicted electronic configuration of ${\text{O}}^{2-}$ is $\left[\text{Kr}\right]5s^{2}4d^{10}5p^6$.

Conclusion

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