Question

Explain oxidation and reduction reaction with examples.

Answer 1

Hint: The term "redox" is a combination of the terms "reduction" and "oxidation." Because dioxygen (${O_2}$ (g)) was the first known oxidising agent, the word oxidation originally meant a reaction with oxygen to create an oxide. Later, the name was broadened to include oxygen-like compounds that performed chemical processes in parallel. Eventually, the definition was broadened to cover any processes involving electron loss.

Complete answer:
Redox is a chemical process that involves changing the oxidation states of atoms. The actual or formal transfer of electrons between chemical species is defined by redox reactions, which usually include one species (the reducing agent) suffering oxidation (losing electrons) while another species (the oxidising agent) experiences reduction (gains electrons). The chemical species that loses an electron is said to have been oxidised, whereas the chemical species that gains an electron is said to have been reduced. To put it another way:
The loss of electrons or a rise in the oxidation state of an atom, an ion, or specific atoms in a molecule is referred to as oxidation.
The gain of electrons or a drop in the oxidation state of an atom, an ion, or specific atoms in a molecule is referred to as reduction (a reduction in oxidation state).
When zinc metal is put in a copper(II) sulphate solution, for example, copper is deposited:
\[Zn\left( s \right) + {\text{ }}CuS{O_4}\left( {aq} \right){\text{ }} \to {\text{ }}ZnS{O_4}\left( {aq} \right){\text{ }} + {\text{ }}Cu\left( s \right)\]
Zinc metal displaces the copper(II) ion from copper sulphate solution in the aforementioned process, releasing free copper metal. Because copper metal has a lower energy than zinc due to bonding via its partly full d-orbitals, the reaction is spontaneous and produces 213 kJ per 65 g of zinc.
For this reaction, the ionic equation is.
\[Zn{\text{ }} + {\text{ }}C{u^{2 + }}\; \to {\text{ }}Z{n^{2 + }}\; + {\text{ }}Cu\]
The zinc is oxidised as two half-reactions may be seen.
\[Zn{\text{ }} \to {\text{ }}Z{n^{2 + }}\; + {\text{ }}2\;{e^ - }\]
The copper is also reduced.
\[C{u^{2 + }}\; + {\text{ }}2\;{e^ - }\; \to {\text{ }}Cu\]

Note:
Electrochemical cells, which may create electrical energy or enable electrosynthesis, are built on the foundation of redox processes. Metal ores frequently contain oxidised metals such as oxides or sulphides, which are recovered by smelting at high temperatures in the presence of a reducing agent. Electroplating, which is used to coat chrome-plated automobile components, silver-plated flatware, galvanization, and gold-plated jewellery, employs redox processes to cover things with a thin layer of a substance.