Redox reactions are reactions during which electron transfer takes place. Here magnesium atom transfers two electrons one each to the two chlorine atoms.
i) What are the products of this reaction?
ii) Write the balanced equation for the complete reaction.
iii) Which element is being oxidized?
iv) Which element is being reduced?
v) Write the reduction part of the reaction?

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Solution

(i) $M g + 2 C l ⟶ M g C l_{2}$
Product is $M g C l_{2}$ (magnesium chloride)
(ii) Balanced equation: $M g + 2 C l ⟶ M g C l_{2}$
(iii) The element which gets oxidized looses electrons. Here, $M g$ is getting oxidized.
(iv) The element which gets reduced gains electrons. Here, $C l$ is getting reduced.
(v) Reduction part= $2 C l + 2 e^{-} ⟶ 2 C l^{-}$

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(i) Mg+2Cl⟶MgCl2Product is MgCl2 (magnesium chloride)(ii) Balanced equation: Mg+2Cl⟶MgCl2(iii) The element which gets oxidized looses electrons. Here, Mg is getting oxidized.(iv) The element which gets reduced gains electrons. Here, Cl is getting reduced.(v) Reduction part= 2Cl+2e−⟶2Cl−