Chapter 5, Problem 55E

Interpretation Introduction

(a)

Interpretation:

The predicted electron configuration of $\text{Li}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{Li}$ is $1s^{2}2s^1$ or $\left[\text{He}\right]2s^1$.

Explanation of Solution

The symbol for lithium is $\text{Li}$. Lithium is the first element in the $2s$ sublevel. The electron configuration is written by filling the electrons according to the energy level order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons and $p$ orbital contains six electrons. The atomic number of lithium is $3$. Therefore, the electron configuration for $\text{Li}$ is $1s^{2}2s^1$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of preceding noble gas. The preceding noble gas of lithium is helium $\left(\text{He}\right)$.

The electron configuration of helium is $1s^2$.

Therefore, the electron configuration for lithium is $\left[\text{He}\right]2s^1$.

Conclusion

The electron configuration for $\text{Li}$ is $1s^{2}2s^1$.

Interpretation Introduction

(b)

Interpretation:

The predicted electron configuration of $\text{F}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{F}$ is $1s^{2}2s^{2}2p^5$ or $\left[\text{He}\right]2s^{2}2p^5$.

Explanation of Solution

The symbol for fluorine is $\text{F}$. Fluorine is the fifth element in the $2p$ sublevel. The electron configuration is written by filling the electrons according to the energy level order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons, $p$ orbital contains six electrons and $d$ orbital contains ten electrons. The atomic number of fluorine is $9$. Therefore, the electron configuration for $\text{F}$ is $1s^{2}2s^{2}2p^5$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of preceding noble gas. The preceding noble gas of fluorine is helium $\left(\text{He}\right)$.

The electron configuration of helium is $1s^2$.

Therefore, the electron configuration for fluorine is $\left[\text{He}\right]2s^{2}2p^5$.

Conclusion

The electron configuration for $\text{F}$ is $1s^{2}2s^{2}2p^5$.

Interpretation Introduction

(c)

Interpretation:

The predicted electron configuration of $\text{Mg}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{Mg}$ is $1s^{2}2s^{2}2p^{6}3s^2$ or $\left[\text{Ne}\right]3s^2$.

Explanation of Solution

The symbol for magnesium is $\text{Mg}$. Magnesium is the second element in the $3s$ sublevel. The electron configuration is written by filling the electrons according to the increasing energy sublevel order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons, $p$ orbital contains six electrons and $d$ orbital contains ten electrons. The atomic number of magnesium is $12$. Therefore, the electron configuration for $\text{Mg}$ is $1s^{2}2s^{2}2p^{6}3s^2$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of preceding noble gas. The preceding noble gas of magnesium is neon $\left(\text{Ne}\right)$.

The electron configuration of neon is $1s^{2}2s^{2}2p^6$.

Therefore, the electron configuration for magnesium is $\left[\text{Ne}\right]3s^2$.

Conclusion

The electron configuration for $\text{Mg}$ is $1s^{2}2s^{2}2p^{6}3s^2$.

Interpretation Introduction

(d)

Interpretation:

The predicted electron configuration of $\text{P}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{P}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^3$ or $\left[\text{Ne}\right]3s^{2}3p^3$.

Explanation of Solution

The symbol for phosphorus is $\text{P}$. Phosphorus is the third element in the $3p$ sublevel. The electron configuration is written by filling the electrons according to the increasing energy sublevel order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons, $p$ orbital contains six electrons and $d$ orbital contains ten electrons. The atomic number of phosphorus is $15$. Therefore, the electron configuration for $\text{P}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^3$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of preceding noble gas. The preceding noble gas of phosphorus is neon $\left(\text{Ne}\right)$.

The electron configuration of neon is $1s^{2}2s^{2}2p^6$.

Therefore, the electron configuration for phosphorus is $\left[\text{Ne}\right]3s^{2}3p^3$.

Conclusion

The electron configuration for $\text{P}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^3$.

Interpretation Introduction

(e)

Interpretation:

The predicted electron configuration of $\text{Ca}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{Ca}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^2$ or $\left[\text{Ar}\right]4s^2$.

Explanation of Solution

The symbol for calcium is $\text{Ca}$. Calcium is the second element in the $4s$ sublevel. The electron configuration is written by filling the electrons according to the increasing energy sublevel order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons, $p$ orbital contains six electrons and $d$ orbital contains ten electrons. The atomic number of calcium is $20$. Therefore, the electron configuration for $\text{Ge}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^2$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of preceding noble gas. The preceding noble gas of calcium is argon $\left(\text{Ar}\right)$.

The electron configuration of argon is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

Therefore, the electron configuration of calcium is $\left[\text{Ar}\right]4s^2$.

Conclusion

The electron configuration for $\text{Ca}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^2$.

Interpretation Introduction

(f)

Interpretation:

The predicted electron configuration of $\text{Mn}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{Mn}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^5$ or $\left[\text{Ar}\right]4s^{2}3d^5$.

Explanation of Solution

The symbol for manganese is $\text{Mn}$. Manganese is the fifth element in the $3d$ sublevel. The electron configuration is written by filling the electrons according to the increasing energy sublevel order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons, $p$ orbital contains six electrons and $d$ orbital contains ten electrons. The atomic number of manganese is $25$. Therefore, the electron configuration for $\text{Mn}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^5$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of preceding noble gas. The preceding noble gas of manganese is argon $\left(\text{Ar}\right)$.

The electron configuration of argon is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

Therefore, the electron configuration of manganese is $\left[\text{Ar}\right]4s^{2}3d^5$.

Conclusion

The electron configuration for $\text{Mn}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^5$.

Interpretation Introduction

(g)

Interpretation:

The predicted electron configuration of $\text{Ga}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{Ga}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^1$ or $\left[\text{Ar}\right]4s^{2}3d^{10}4p^1$.

Explanation of Solution

The symbol for gallium is $\text{Ga}$. Gallium is the first element in the $4p$ sublevel. The electron configuration is written by filling the electrons according to the increasing energy sublevel order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons, $p$ orbital contains six electrons and $d$ orbital contains ten electrons. The atomic number of gallium is $31$. Therefore, the electron configuration for $\text{Ga}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^1$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of the preceding noble gas. The preceding noble gas of gallium is argon $\left(\text{Ar}\right)$.

The electron configuration of argon is $1s^{2}2s^{2}2p^{6}3s^{2}3p^6$.

Therefore, the electron configuration of gallium is $\left[\text{Ar}\right]4s^{2}3d^{10}4p^1$.

Conclusion

The electron configuration for $\text{Ga}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^1$.

Interpretation Introduction

(h)

Interpretation:

The predicted electron configuration of $\text{Rb}$ is to be stated.

Concept introduction:

The arrangement of electrons in the energy sublevels is explained by the electron configuration of an atom. The electron configuration of an atom can be written according to the arrangement of energy levels as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

Answer to Problem 55E

The electron configuration for $\text{Rb}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^1$ or $\left[\text{Kr}\right]5s^1$.

Explanation of Solution

The symbol for rubidium is $\text{Rb}$. Rubidium is the first element in the $5s$ sublevel. The electron configuration is written by filling the electrons according to the increasing energy sublevel order as shown below.

$1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s$

The $s$ orbital contains two electrons, $p$ orbital contains six electrons and $d$ orbital contains ten electrons. The atomic number of rubidium is $37$. Therefore, the electron configuration for $\text{Rb}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^1$.

The abbreviation of the electron configuration is done by denoting the innermost electrons by the symbol of preceding noble gas. The preceding noble gas with less than the atomic number of rubidium is krypton $\left(\text{Kr}\right)$.

The electron configuration of krypton is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.

Therefore, the electron configuration of rubidium is $\left[\text{Kr}\right]5s^1$.

Conclusion

The electron configuration for $\text{Rb}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^1$.