Chapter 1, Problem 1E.11E

(a)

Interpretation Introduction

Interpretation:

The ground state configuration of sodium atom has to be predicted.

Concept introduction:

Electronic configuration: The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

Electrons occupy the lowest energy orbitals. The increasing order of orbital energy is $s,p,dandf.$  The lowest energy orbital is $ls.$

The energy order of the orbital for the first three periods is as follows,

    $ls,2s,2p,3s,and3p.$

The orbital which is closer to the nucleus has lower energy; therefore the $2s$ is lower in energy than $3s.$   Accordingly $2s$ is lower in energy than $2pand4s$ is lower in energy than $3d.$

In general, the orbitals can hold maximum of two electrons, the two electrons must have opposite spin.

The subshell ordering by Aufbau principle is given below,

    $ls,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p,8s,\mathrm{...}$

Explanation of Solution

The electronic configuration is depends on the electrons in the atom.  The sodium atom has $11$ electrons.

The subshell ordering by Aufbau principle is given below;

    $ls,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p,8s,\mathrm{...}$

Therefore ground state electronic configuration of sodium atom is $l{s}^{2}2s^{2}2p^{6}3s^1$ $\left(11electrons\right).$

Sodium belongs to Period $3$ and Group $1.$  It has a neon core with additional one valence electron.

The electronic configuration also can be written as follows,

    $\left[Ne\right]3s^1.$

(b)

Interpretation Introduction

Interpretation:

The ground state configuration of silicon atom has to be predicted.

Concept introduction:

Refer to part (a).

Explanation of Solution

The electronic configuration is depends on the electrons in the atom.  The silicon atom has $14$ electrons.

The subshell ordering by Aufbau principle is given below;

    $ls,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p,8s,\mathrm{...}$

Therefore ground state electronic configuration of silicon atom is $l{s}^{2}2s^{2}2p^{6}3s^{2}3p^2$ $\left(14electrons\right).$

Silicon belongs to Period $3$ and Group $14.$  It has a neon core with four additional valence electrons.

The electronic configuration also can be written as follows,

    $\left[Ne\right]3s^{2}3p^2.$

(c)

Interpretation Introduction

Interpretation:

The ground state configuration of chlorine atom has to be predicted.

Concept introduction:

Refer to part (a).

Explanation of Solution

The electronic configuration is depends on the electrons in the atom.  The chlorine atom has $17$ electrons.

The subshell ordering by Aufbau principle is given below;

    $ls,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p,8s,\mathrm{...}$

Therefore ground state electronic configuration of chlorine atom is $l{s}^{2}2s^{2}2p^{6}3s^{2}3p^5$ $\left(17electrons\right).$

Chlorine belongs to Period $3$ and Group $17.$  It has a neon core with seven additional valence electrons.

The electronic configuration also can be written as follows,

    $\left[Ne\right]3s^{2}3p^5.$

(d)

Interpretation Introduction

Interpretation:

The ground state configuration of rubidium atom has to be predicted.

Concept introduction:

Refer to part (a).

Explanation of Solution

The electronic configuration is depends on the electrons in the atom.  The rubidium atom has $37$ electrons.

The subshell ordering by Aufbau principle is given below;

    $ls,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s,5f,6d,7p,8s,\mathrm{...}$

Therefore ground state electronic configuration of rubidium atom is $l{s}^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^1$ $\left(37electrons\right).$

Rubidium belongs to Period $5$ and Group $1.$  It has a krypton core with one additional valence electron.

The electronic configuration also can be written as follows,

    $\left[Kr\right]5s^1.$