Question

$Mg^{+} + Cl_2$ is a redox reaction. Explain.

Answer 1

Redox reactions are oxidation-reduction chemical processes in which the oxidation states of the reactants change. The term ‘redox' refers to the reduction-oxidation process. All redox reactions may be split down into two types of reactions: reduction and oxidation. Oxidation is defined as the loss of electrons and the resulting rise in the oxidation state of a particular reactant. Reduction is the process of gaining electrons and decreasing the oxidation state of a reactant.

Complete answer:
Oxidizing agents are electron-accepting entities that tend to suffer a reduction in redox processes. A reducing agent is an electron-donating species that tends to hand over electrons. Oxidation is a common occurrence in several species. Any redox process may be decomposed into two half-reactions, namely the oxidation half-reaction and the reduction half-reaction.
Combination reactions are the polar opposite of decomposition reactions, involving the joining of two chemicals to produce a single compound ($A\text{ }+\text{ }B\text{ }\to \text{ }AB$).
The chemical molecule $MgC{{l}_{2}}$ and its many hydrates $MgC{{l}_{2}}{{({{H}_{2}}O)}_{x}}$ are referred to as magnesium chloride. Anhydrous $MgC{{l}_{2}}$ has a mass content of 25.5 percent elemental magnesium. These salts are typical ionic halides, with a high water solubility. Brine or sea water can be used to extract hydrated magnesium chloride. Magnesium chloride is predominantly manufactured in North America from brine from the Great Salt Lake.
$\mathrm{Mg}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow \mathrm{MgCl}_{2}(\mathrm{~s})$
The metal loses electrons, and in the process of producing $\mathrm{Mg}^{2}$ , it loses two electrons and becomes oxidised.
$\mathrm{Mg}(\mathrm{s}) \rightarrow \mathrm{Mg}^{2+}+2 \mathrm{e}^{-}(\mathrm{i})$
On the other hand, receiving electrons reduces chlorine to the chloride ion:
$\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}(\mathrm{ii})$
And (i) $+(\mathrm{ii})=\mathrm{Mg}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow \mathrm{MgCl}_{2}(\mathrm{~s})$
As needed, both charge and mass are balanced.

Note:
Many organic reactions are redox reactions because they include changes in oxidation levels but no clear electron transfer. For example, when wood is burned with molecular oxygen, the oxidation state of carbon atoms in the wood increases while the oxidation state of oxygen atoms drops, resulting in the formation of carbon dioxide and water. The oxygen atoms go through reduction and gain electrons, whereas the carbon atoms go through oxidation and lose electrons. In this reaction, oxygen is the oxidising agent and carbon is the reducing agent.