[Q.Solved] Which Reaction Below Represents The First Ionization Of O(Oxygen)?

Which reaction below represents the first ionization of O? 

a. O(g) + e- → O-(g)

b. O+(g) + e- → O(g)

c. O(g) → O+(g) + e-

d. O-(g) + e- → O2-(g)

e. O-(g) → O(g) + e

Solution of this question is

C.  O(g) → O+(g) + e-

The reaction that gives the first ionization energy of Oxygen is the one which shows the removal of the outermost electron from the neutral oxygen atom. The removal of the outermost electron results in the formation of a positive oxygen ion. Thus the correct answer for the question is the option that satisfies these requirements.

This question deals with the ionization energy and successive ionization energy. Ionization Energy is defined as:

The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom to form a gaseous ion is called the ionization enthalpy or ionization energy of that atom.

The elements follow a regular trend when we look at the values of Ionization Energy.

Equations for Successive Ionization Energy of Oxygen

                        O (g)  + IE1            → O+ (g) + e-

                        O+ (g)  + IE2          → O2+ (g) + e-

                        O2+ (g)   + IE3        → O3+ (g) + e-

From the above equations we can see how ionization change of charge in Oxygen takes place. The three equations are for the first, second and third ionization of Oxygen, respectively.

Oxygen ion is stable in its Dipositive ion state. So it further undergoes second ionization energy reaction. Which in turn results in the stable O2+ state of Oxygen. 

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