Chapter 4, Problem 4.32QP

Interpretation Introduction

Interpretation: Define the term ionization energy (a), and why ionization energy measurements are usually made when atoms are in the gaseous state (b), the second ionization energy always greater than the first ionization energy for any element (c) and the types of elements having the highest ionization energies and what types have the lowest ionization energies (d) reasons for all these should be determined.

Concept introduction:

• The ionization energy is the minimum amount of energy required to remove the electron from an isolated atom which is in the gaseous state.

${\mathrm{atom}}_{\left(g\right)}$$\to$ positive ${\mathrm{ion}}_{\left(g\right)}$+ electron

To explain: why ionization energy is measured for atoms in gaseous state, which element having higher ionization energy and lower ionization energy and which element having higher ionization energy and lower ionization energy.