Chapter 11, Problem 53A

Interpretation Introduction

Interpretation: Reason for the metallic elements of a given period to have lower ionization energies than the nonmetallic elements needs to be explained.

Concept introduction: Ionization energy is defined as the minimum energy required to eject out the outermost electron from an isolated gaseous atom.

Answer to Problem 53A

This is because metallic elements are electropositive and nonmetallic elements are electronegative in nature.

Explanation of Solution

Being electropositive metallic elements have tendency to lose electrons. Thus an electron can be easily removed from its outermost shell due to which the ionization energy is low whereas being electronegative nonmetallic elements have tendency to gain electrons due to which it is difficult to remove an electron from its outermost shell due to which the ionization energy is higher in this case.

Conclusion

Because of electropositive nature of metallic elements they have lower ionization energies than nonmetallic elements in the same period.