Chapter 1, Problem 1F.10E

Interpretation Introduction

Interpretation:

The reason why the first ionization energy of chlorine is greater than sulfur while the second ionization energy are nearly same has to be given.

Concept Introduction:

Ionization energy:

The ionization energy of an atom is the amount of energy required to remove an electron from the gaseous form of that atom or ion.

Example:

  $\text{Na}\left(\text{g}\right)\stackrel{}{\to }{\text{Na}}^{\text{+}}\left(\text{g}\right){\text{+e}}^{\text{-}}$

As moving across the period the atomic radius decreases therefore the outer electrons are closer to the nucleus and more strongly held by the nucleus and thus it requires a lot of energy to remove the outermost electron.

Second Ionization energy:

The energy required to remove a second electron from a singly charged gaseous cation is called as second ionization energy.

Example:

  ${\text{Na}}^{\text{+}}\left(\text{g}\right)\stackrel{}{\to }{\text{Na}}^{\text{2+}}\left(\text{g}\right){\text{+e}}^{\text{-}}$

The second ionization energy of sodium is $\text{4560}\text{kJ/mol}\text{.}$

The second ionization energy is almost ten times greater than the first ionization energy because the number of electrons causing repulsions is reduced.