Chapter 2, Problem 52P

For each element in Problem 2.50: (a) Write out the electronic configuration using a superscript with each orbital; (b) write out the electronic configuration using noble gas notation.

Interpretation Introduction

(a)

Interpretation:

The electronic configuration for the indicated elements in the periodic table, using a superscript with each orbital,is to be written.

Concept introduction:

The elements are placed in periodic table in increasing order of their atomic numbers. The electronic configuration of these elements is the distribution of electrons in different shells, sub shells and orbital of the atom.

Answer to Problem 52P

The orbital diagram of the electronic configuration for the indicated elements (a), $\text{N}$ is shown below.

  $1s^{2}2s^{2}2p^3$

The orbital diagram of the electronic configuration for the indicated elements (b), $\text{I}$ is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^5$

The orbital diagram of the electronic configuration for the indicated elements (c), $\text{Ga}$ is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^1$

The orbital diagram of the electronic configuration for the indicated elements (d), $\text{Ti}$ is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^2$

The orbital diagram of the electronic configuration for the indicated elements (e), $\text{Mn}$ is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^5$

Explanation of Solution

The electrons are distributed in different orbitals of atom. This is known as the electronic configuration of the element.

The distribution is written in a special manner. First the name of the sub shell is written and the number of electron in it is written as superscript of it.

The electronic configuration of the element (a) nitrogen (atomic number $7$ ) indicated in the periodic table, is shown below.

  $1s^{2}2s^{2}2p^3$

The electronic configuration of the element (b) iodine (atomic number $53$ ) indicated in the periodic table, is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^5$

The electronic configuration of the element (c) gallium (atomic number $31$ )indicated in the periodic table, is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^1$

The electronic configuration of the element (d) titanium (atomic number $22$ )indicated in the periodic table, is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^2$

The electronic configuration of the element (e) manganese (atomic number $25$ )indicated in the periodic table, is shown below.

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^5$

Interpretation Introduction

(b)

Interpretation:

The electronic configuration for the indicated elements in the periodic table, using a noble gas notationis to be stated.

Concept introduction:

The elements are placed in periodic table in increasing order of their atomic numbers. The electronic configuration of these elements is the distribution of electrons in different shells, sub shells and orbital of the atom.

Answer to Problem 52P

The orbital diagram of the electronic configuration for the indicated elements (a) $\text{N}$ is shown below.

  $\left[\text{He}\right]2s^{2}2p^3$

The orbital diagram of the electronic configuration for the indicated elements (b) $\text{I}$ is shown below.

  $\left[\text{Kr}\right]5s^{2}4d^{10}5p^5$

The orbital diagram of the electronic configuration for the indicated elements (c) $\text{Ga}$ is shown below.

  $\left[\text{Ar}\right]4s^{2}3d^{10}4p^1$

The orbital diagram of the electronic configuration for the indicated elements (d) $\text{Ti}$ is shown below.

  $\left[\text{Ar}\right]4s^{2}3d^2$

The orbital diagram of the electronic configuration for the indicated elements (e) $\text{Mn}$ is shown below.

  $\left[\text{Ar}\right]4s^{2}3d^5$

Explanation of Solution

The electrons are distributed in the different orbitals of atom. This is known as the electronic configuration of the element.

The distribution can be written in two manners. First the name of the sub shell is written and the number of electron in it is written as superscript of it.

This can be written in noble gas notations also. In this manner the noble gas of the previous period is written in large brackets to represent the electronic configuration of the completely filled orbits of this noble gas. The rest of the configuration is written as usual.

The electronic configuration of the element (a) nitrogen, indicated in the periodic table is

  $1s^{2}2s^{2}2p^3$ .The noble gas notation is as given below.

  $\left[\text{He}\right]2s^{2}2p^3$

The electronic configuration of the element (b) iodine, indicated in the periodic table is

  $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^5$ . The noble gas notation is as given below.

  $\left[\text{Kr}\right]5s^{2}4d^{10}5p^5$

The electronic configuration of the element (c) gallium, indicated in the periodic table is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^1$ . The noble gas notation is as given below.

  $\left[\text{Ar}\right]4s^{2}3d^{10}4p^1$

The electronic configuration of the element (d) titanium, indicated in the periodic table is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^2$ . The noble gas notation is as given below.

  $\left[\text{Ar}\right]4s^{2}3d^2$

The electronic configuration of the element (e) manganese, indicated in the periodic table is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^5$ . The noble gas notation is as given below.

  $\left[\text{Ar}\right]4s^{2}3d^5$

Here, $\left[\text{He}\right]=1s^2$ , $\left[\text{Kr}\right]=1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^6$ and $\left[\text{Ar}\right]=1s^{2}2s^{2}2p^{6}3s^{2}3p^6$