Question

Can ${{\text{F}}^{\text{ - }}}$ be oxidised to ${{\text{F}}_{\text{2}}}$ by any substance listed in the electrochemical series?

Answer 1

In the above question, it is asked if ${{\text{F}}^{\text{ - }}}$ can be oxidised to ${{\text{F}}_{\text{2}}}$ by any substance listed in the electrochemical series. This is only possible if there is any element which is a stronger oxidising agent than fluorine. Elements are placed in the electrochemical series according to their standard electrode potentials. Metals present at the top and bottom of the series are good reducing and oxidising agents respectively.

Complete step by step solution:
An oxidizing agent is one which oxidises other elements. It is a reactant which removes electrons from other reactants during a redox reaction. The oxidizing agent usually takes these electrons and thus after gaining electrons it gets reduced. Hence, we can say that an oxidizing agent is an electron acceptor.
Examples of oxidising agents are hydrogen peroxide, ozone, oxygen, potassium nitrate and nitric acid along with all halogens.
The group 17 elements of the periodic table are collectively known as Halogens. They have a strong ability to gain electrons because of their high electronegativity when compared with elements of other groups. This implies that they have the ability to easily attract electrons towards their respective nuclei. Examples of the halogens that are good oxidizing agents include iodine, bromine, chlorine, and fluorine.
Due to the smaller size of fluorine, the tendency to gain electrons is maximum. And hence, the strongest oxidising agent is fluorine in the whole electrochemical series.
So, ${{\text{F}}^{\text{ - }}}$ cannot be oxidised to ${{\text{F}}_{\text{2}}}$ by any substance listed in the electrochemical series.

Note:
-Oxidising agents are used in bleaching of fabrics, storage of energy in batteries and vulcanisation of rubber.
-An oxidiser can easily contribute to combustion, hence, they are often called as dangerous material.