Question

Give an example of a reaction in which a less reactive non-metal is displaced by a more reactive non-metal.

Answer 1

We know that the reactivity series of metals, also known as the activity series, refers to the arrangement of metals in the descending order of their reactivities. Displacement reaction is a reaction in which one element is displaced by another element. The more reactive element will displace the less reactive element.

Complete answer:
As we know from the displacement reaction, a metal from the electrochemical series is mixed with the metal which is placed lower down in the electrochemical series. In this displacement reaction, a more reactive push their electrons on the less reactive metal. In the reactivity series, metals present on the top are highly reactive and can displace the metals at the bottom of the series. A metal that is placed higher in the activity series can displace the metal present at a lower position from the aqueous solution of its salt. For example, Iron which is more reactive than copper displaces copper from copper sulphate solution to form iron sulphate solution. Displacement reaction is a chemical reaction in which a more reactive element displaces a less reactive element from its compound. Both metals and nonmetals take part in displacement reactions. For example: Reaction of iron nail with copper sulphate solution.
The displacement reaction is not just limited to metals. Here Iron displaces the copper metal and forms iron sulfate solution. As per the reactivity series Iron is more reactive than copper. Non-metals take part in these reactions as well. It is a reaction in which either a metal or a non-metal displaces another non-metal of a compound. The non-metals have similar activity series just like the metals. Hydrogen can easily be displaced by the more electropositive metals in non-metal displacement reactions because hydrogen lies below the electropositive metals in the electrochemical series and therefore, the reactivity of the electropositive metals is much more than the hydrogen. $F{{e}_{\left( s \right)}}+CuS{{O}_{4}}_{\left( aq \right)}\to FeS{{O}_{4}}_{\left( aq \right)}+C{{u}_{\left( s \right)}}$

Note:
Remember that the elements are arranged in the order of their increasing electrode potential values. Electropositive elements are the elements which tend to lose their electrons to their solution. Electronegative elements are the elements that tend to withdraw electrons.