Chemistry
Chemistry
9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Cengage Learning
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Textbook Question
Chapter 8, Problem 46E

Write electron configurations for

a. the cations Sr2+, Cs+, In+, and Pb2+.

b. the anions P3−, S2−, and Br.

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The electronic configuration of given cation and anion is to be written.

Concept introduction: The electronic configuration is a method to explain the atomic orbitals in ground state. It is the representation of distribution of electrons of atoms and molecules. In ground state of an atom, the electrons fill in atomic orbitals according to the Aufbau principle.

Chemistry, Chapter 8, Problem 46E , additional homework tip  1

Figure 1

To determine: The electronic configuration of cations Sr2+,Cs+,In+ and Pb2+.

Answer to Problem 46E

Answer

The electronic configuration of cations is as follows,

The electronic configuration of cation Sr2+ is 1s22s22p63s23p63d104s24p6.

The electronic configuration of Cs+ is 1s22s22p63s23p63d104s24p64d105s25p6. The electronic configuration of In+ is 1s22s22p63s23p63d104s24p64d105s2.

The electronic configuration of Pb2+ is,

1s22s22p63s23p63d104s24p64d105s25p64f145d106s2

Explanation of Solution

  • To determine: The electronic configuration of cation Sr2+.

The atomic number of strontium (Sr) is 38. The electronic configuration of strontium is,

1s22s22p63s23p63d104s24p65s2

It loses two electrons to get most stable inert gas configuration and form Sr2+. The electronic configuration of Sr2+ is 1s22s22p63s23p63d104s24p6.

  • To determine: The electronic configuration of cation Cs+.

The atomic number of Cesium is 55. The electronic configuration of Cesium is,

1s22s22p63s23p63d104s24p64d105s25p6

It can lose an electron to get most stable inert gas configuration and form Cs+. The electronic configuration of Cs+ is 1s22s22p63s23p63d104s24p64d105s25p6.

  • To determine: The electronic configuration of cation In+.

The atomic number of Indium is 49. The electronic configuration of Indium is,

1s22s22p63s23p63d104s24p64d105s25p1

It can lose an electron to get most stable state configuration and form In+. The electronic configuration of In+ is 1s22s22p63s23p63d104s24p64d105s2.

  • To determine: The electronic configuration of cation Pb2+.

The atomic number of lead is 82. The electronic configuration of lead is,

1s22s22p63s23p63d104s24p64d105s25p64f145d106s26p2

It loses two electrons to get most stable state configuration and form Pb2+. The electronic configuration of Pb2+ is 1s22s22p63s23p63d104s24p64d105s25p64f145d106s2.

Conclusion

In ionic compounds, cation loses electrons to get stable state by acquiring nearest noble gas electronic configuration.

The electronic configuration of cation Sr2+ is 1s22s22p63s23p63d104s24p6.

The electronic configuration of cation Cs+ is 1s22s22p63s23p63d104s24p64d105s25p6.

The electronic configuration of cation In+ is 1s22s22p63s23p63d104s24p64d105s2.

The electronic configuration of cation Pb2+ is,

1s22s22p63s23p63d104s24p64d105s25p64f145d106s2.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The electronic configuration of given cation and anion is to be written.

Concept introduction: The electronic configuration is a method to explain the atomic orbitals in ground state. It is the representation of distribution of electrons of atoms and molecules. In ground state of an atom, the electrons fill in atomic orbitals according to the Aufbau principle.

Chemistry, Chapter 8, Problem 46E , additional homework tip  2

Figure 1

To determine: The electronic configuration of anions P3,S2 and Br.

Answer to Problem 46E

Answer

The electronic configuration of anions is as follows,

The electronic configuration of P3 is 1s22s22p63s23p6.

The electronic configuration of S2 is 1s22s22p63s23p6.

            The electronic configuration of Br is 1s22s22p63s23p63d104s24p6.

Explanation of Solution

  • To determine: The electronic configuration of anion P3.

The atomic number of Phosphorous is 15. The electronic configuration of Phosphorous is,

1s22s22p63s23p3

It can gain three electrons to get most stable inert gas configuration and form P3. The electronic configuration of P3 is 1s22s22p63s23p6.

  • To determine: The electronic configuration of anion S2.

The atomic number of sulfur is 16. The electronic configuration of sulfur is,

1s22s22p63s23p4

It can gain two electrons to get most stable inert gas configuration and form S2. The electronic configuration of S2 is 1s22s22p63s23p6.

  • To determine: The electronic configuration of anion Br.

The atomic number of bromine is 35. The electronic configuration of bromine is,

1s22s22p63s23p63d104s24p5

It can gain an electron to get most stable inert gas configuration and form Br. The electronic configuration of Br is 1s22s22p63s23p63d104s24p6.

Conclusion

In ionic compounds, anions gain electrons to get stable state by acquiring nearest noble gas electronic configuration.

The electronic configuration of anions P3 is 1s22s22p63s23p6.

The electronic configuration of anions S2 is 1s22s22p63s23p6.

The electronic configuration of anions Br is 1s22s22p63s23p63d104s24p6.

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Chapter 8 Solutions

Chemistry

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