Chapter 8, Problem 8.1P

Interpretation Introduction

Interpretation: The electronic configuration for each of the given elements is to be stated.

Concept introduction: The electrons of an atom or molecule are distributed in molecular or atomic orbitals. This distribution of electrons is known as the electronic configuration of the atom or molecule.

To determine: The electronic configuration for each of the given elements.

Answer to Problem 8.1P

Solution: The electronic configuration of $\text{Cl}$is $\left[\text{Ne}\right]{\text{3s}}^{\text{2}}{\text{3p}}^{\text{5}}$ . The electronic configuration of $\text{Si}$is $\left[\text{Ne}\right]{\text{3s}}^{\text{2}}{\text{3p}}^2$ . The electronic configuration of $\text{Sr}$is $\left[\text{Kr}\right]5{\text{s}}^{\text{2}}$ . The electronic configuration of $\text{O}$is $\left[\text{He}\right]{\text{2s}}^{\text{2}}{\text{2p}}^{\text{4}}$ .

(a)

Explanation of Solution

Atomic number is the total number of electrons present in a neutral atom.

On basis of the periodic table of elements, the atomic number $\left(\text{Z}\right)$of chlorine is $17$ .

So, chlorine has $17$ electrons which are distributed in respective orbitals.

The electronic configuration of element $\text{Cl}$is $\left[\text{Ne}\right]{\text{3s}}^{\text{2}}{\text{3p}}^{\text{5}}$ .

Where, $\left[\text{Ne}\right]$represents the inner electrons this is the nearest noble gas and the electronic configuration for $\left[\text{Ne}\right]$is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^6$ .

(b)

Atomic number is the total number of electrons present in a neutral atom.

On basis of the periodic table of elements, the atomic number $\left(\text{Z}\right)$of silicon is $14$ .

So, silicon has $14$electrons which are distributed in respective orbitals.

The electronic configuration of element $\text{Si}$is $\left[\text{Ne}\right]{\text{3s}}^{\text{2}}{\text{3p}}^2$ .

Where, $\left[\text{Ne}\right]$represents the inner electrons this is the nearest noble gas and the electronic configuration for $\left[\text{Ne}\right]$is ${\text{1s}}^{\text{2}}{\text{2s}}^{\text{2}}{\text{2p}}^6$ .

(c)

Atomic number is the total number of electrons present in a neutral atom.

On basis of the periodic table of elements, the atomic number $\left(\text{Z}\right)$of strontium is $38$ .

So, strontium has $38$electrons which are distributed in respective orbitals.

The electronic configuration of element $\text{Sr}$is $\left[\text{Kr}\right]{\text{5s}}^{\text{2}}$ .

Where, $\left[\text{Kr}\right]$represents the inner electrons this is the nearest noble gas and the electronic configuration for $\left[\text{Kr}\right]$is $\left[\text{Ar}\right]{\text{3d}}^{10}{\text{4s}}^{\text{2}}{\text{4p}}^6$ .

(d)

Atomic number is the total number of electrons present in a neutral atom.

On basis of the periodic table of elements, the atomic number $\left(\text{Z}\right)$of oxygen is $8$ .

So, oxygen has $8$electrons which are distributed in their respective orbitals.

The electronic configuration of element $\text{O}$is $\left[\text{He}\right]{\text{2s}}^{\text{2}}{\text{2p}}^4$ .

Where, $\left[\text{He}\right]$represents the inner electrons this is the nearest noble gas and the electronic configuration for $\left[\text{He}\right]$is ${\text{1s}}^{\text{2}}$ .