Chapter 5, Problem 56E

Interpretation Introduction

(a)

Interpretation:

The predicted electron configuration of $\text{B}$ 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 56E

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

Explanation of Solution

The symbol for boron is $\text{B}$. Boron is the first 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 can accommodate two electrons and $p$ orbital can accommodate six electrons. The atomic number of boron is $5$. Therefore, the electron configuration for $\text{B}$ is $1s^{2}2s^{2}2p^1$.

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 atomic number less than the atomic number of boron is helium $\left(1s^2\right)$. Therefore, the electronic configuration for boron is $\left[\text{He}\right]2s^{2}2p^1$.

Conclusion

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

Interpretation Introduction

(b)

Interpretation:

The predicted electron configuration of $\text{Ti}$ 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 56E

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

Explanation of Solution

The symbol for titanium is $\text{Ti}$. Titanium is the second element in the $3d$ 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 can accommodate two electrons, $p$ orbital can accommodate six electrons and $d$ orbital can accommodate ten electrons. The atomic number of titanium is $22$. Therefore, the electron configuration for $\text{Ti}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^2$.

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

The electronic configuration of argon is $\left(1s^{2}2s^{2}2p^{6}3s^{2}3p^6\right)$.

Therefore, the electronic configuration for titanium is $\left[\text{Ar}\right]4s^{2}3d^2$.

Conclusion

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

Interpretation Introduction

(c)

Interpretation:

The predicted electron configuration of $\text{Na}$ 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 56E

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

Explanation of Solution

The symbol for sodium is $\text{Na}$. Sodium is the first 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 can accommodate two electrons, $p$ orbital can accommodate six electrons and $d$ orbital can accommodate ten electrons. The atomic number of sodium is $11$. Therefore, the electron configuration for $\text{Na}$ is $1s^{2}2s^{2}2p^{6}3s^1$.

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 atomic number less than the atomic number of sodium is neon $\left(\text{Ne}\right)$.

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

Therefore, the electronic configuration for sodium is $\left[\text{Ne}\right]3s^1$.

Conclusion

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

Interpretation Introduction

(d)

Interpretation:

The predicted electron configuration of $\text{O}$ 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 56E

The electron configuration for $\text{O}$ is $1s^{2}2s^{2}2p^4$ or $\left[\text{He}\right]2s^{2}2p^4$.

Explanation of Solution

The symbol for oxygen is $\text{O}$. Oxygen is the fourth element in the $2p$ 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 can accommodate two electrons, $p$ orbital can accommodate six electrons and $d$ orbital can accommodate ten electrons. The atomic number of oxygen is $8$. Therefore, the electron configuration for $\text{O}$ is $1s^{2}2s^{2}2p^4$.

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 atomic number less than the atomic number of oxygen is helium $\left(\text{He}\right)$.

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

Therefore, the electronic configuration for oxygen is $\left[\text{He}\right]2s^{2}2p^4$.

Conclusion

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

Interpretation Introduction

(e)

Interpretation:

The predicted electron configuration of $\text{Ge}$ 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 56E

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

Explanation of Solution

The symbol for germanium is $\text{Ge}$. Germanium is the second 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 can accommodate two electrons, $p$ orbital can accommodate six electrons and $d$ orbital can accommodate ten electrons. The atomic number of germanium is $32$. 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 with atomic number less than the atomic number of germanium is argon $\left(\text{Ar}\right)$.

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

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

Conclusion

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

Interpretation Introduction

(f)

Interpretation:

The predicted electron configuration of $\text{Ba}$ 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 56E

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

Explanation of Solution

The symbol for barium is $\text{Ba}$. Barium is the second element in the $6s$ 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 can accommodate two electrons, $p$ orbital can accommodate six electrons and $d$ orbital can accommodate ten electrons. The atomic number of barium is $56$. Therefore, the electron configuration for $\text{Ba}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^2$.

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

The electronic configuration of xenon is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^6$.

Therefore, the electronic configuration of barium is $\left[\text{Xe}\right]6s^2$.

Conclusion

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

Interpretation Introduction

(g)

Interpretation:

The predicted electron configuration of $\text{Pd}$ 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 56E

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

Explanation of Solution

The symbol for palladium is $\text{Pd}$. Palladium is the eight element in the $4d$ 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 can accommodate two electrons, $p$ orbital can accommodate six electrons and $d$ orbital can accommodate ten electrons. The atomic number of palladium is $46$. Therefore, the electron configuration for $\text{Pd}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}4d^{10}$.

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 atomic number less than the atomic number of palladium is krypton $\left(\text{Kr}\right)$.

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

Therefore, the electronic configuration of palladium is $\left[\text{Kr}\right]4d^{10}$.

Conclusion

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

Interpretation Introduction

(h)

Interpretation:

The predicted electron configuration of $\text{Kr}$ 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 56E

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

Explanation of Solution

The symbol for krypton is $\text{Kr}$. Krypton is the sixth 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 can accommodate two electrons, $p$ orbital can accommodate six electrons and $d$ orbital can accommodate ten electrons. The atomic number of krypton is $36$. Therefore, the electron configuration for $\text{Kr}$ is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$.

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 atomic number less than the atomic number of krypton 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 krypton is $\left[\text{Ar}\right]4s^{2}3d^{10}4p^6$.

Conclusion

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