Explanation The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge. Usually ionization energy increases along the period since the valence electron is added to the same shell and thus attraction by the nucleus gets stronger. Hence, the expected order of ionization is I . E N < I . E O < I . E F . Nitrogen, oxygen and fluorine are in same period (Period 2)

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Question

Chapter 1, Problem 1.13E

Interpretation Introduction

Interpretation:

Reason for why ionization energy of oxygen is slightly less comparing to that of nitrogen and fluorine has to be explained.

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Chapter 1, Problem 1.12E

Chapter 1, Problem 1.14E

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