Chapter 11, Problem 68A

Interpretation Introduction

Interpretation: Comparison of ionization energy of metals and non-metals has to be made and explained.

Concept introduction: Ionization energy can be described as the minimum energy absorbed by an electron in a gaseous atom or ion to get removed from the atom. As energy is absorbed, the process is endothermic.

Answer to Problem 68A

Metals generally have low ionization energy and non-metals have generally high ionization energy.

Explanation of Solution

Metals typically have 1, 2 or 3 electrons in their outermost orbital. They tend to lose electrons to attain stable noble gas configuration of full-filled orbital.

For example electronic configuration of sodium (Na) is $1s^{2}2s^{2}2p^{6}3s^1$ .It is favourable for Na to lose one electron to attain configuration of argon (Ar) which is a noble gas having complete octet.

On the other hand, non-metals are generally electronegative that tend to have affinity towards electrons.Most of the non-metals have more than 4 valence electrons. So, it is relatively easier for them to complete its octet by accepting electron rather than donating electron.

For example electronic configuration of oxygen (O) is $1s^{2}2s^{2}2p^4$ . So, if O accepts two electrons it will complete its octet.

Conclusion

Metals generally have low ionization energy and non-metals have generally high ionization energy.