Chapter 8, Problem 8.58P

Interpretation Introduction

Interpretation:

The full electronic configuration of the element of the third period is to be determined with the help of its ionization energies.

Concept introduction:

The electronic configuration tells about the distribution of electrons in various atomic orbitals. The full electronic configuration of an atom tells about the distribution of electrons in its various atomic orbital.

The ionization energy is the amount of energy required to remove the most loosely bound valence electrons from an isolated neutral gaseous atom. It is represented by $\text{IE}$. The amount of energy required to remove one electron from the valence shell of an atom in the gaseous state is called first ionization energy $\left({\text{IE}}_1\right)$. The amount of energy required to remove the second electron from the valence shell of an atom in the gaseous state is called second ionization energy $\left({\text{IE}}_2\right)$ so on.

Its value varies with the ease of removal of the outermost valence electron. If the outermost electron is removed very easily then the value of ionization energy is very small. If the electron is removed with quite a difficulty then the value of ionization energy will be very high. An abrupt increase in the successive ionization energy indicates that the electron is removed from the core-shell and therefore from the successive ionization data the electronic configuration and the name of the element can be identified.

The ionization energy of an element increases along the period because the electrons are held by high effective nuclear charge. The value of ionization energy decreases from top to bottom because the valence electrons are much farther from the nucleus and therefore experiences weaker forces of attraction.