Chapter 8, Problem 8.47P

Interpretation Introduction

Interpretation:

The region of the periodic table with relatively high and low $\text{IEs}$ is to be determined.

Concept introduction:

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 IE. Its value varies with the ease of removal of the outermost valence electron.

The ionization energy of an element increases along the period and its value decreases down the group.

When the first electron is removed from a neutral, isolated gaseous atom then the ionization energy is known as the first ionization energy $\left({\text{IE}}_1\right)$. Similarly, when then the second electron is removed from the positively charged cation the ionization energy is called the second ionization energy $\left({\text{IE}}_2\right)$ and so on.

The values of the successive ionization energies are always greater than the preceding ones as the electron has to be removed from the cation which is very difficult due to stronger attractive forces with the nucleus.