Question

In redox reaction electrons are transferred from reductant to oxidant or oxidant to reductant

Answer 1

By looking at each element's oxidation state on the reactant side of a chemical equation compared with the same element's oxidation state on the product side, one can determine if the element is reduced or oxidized, and can therefore identify the oxidizing and reducing agents of a chemical reaction.

 Oxidizing AgentsReducing AgentsOxidation StateDecreasesIncreases# of ElectronsGainedLostSubstance is...ReducedOxidized

Answer 2

Answer:

Oxidation number or oxidation state : The oxidation number (or oxidation state) of an atom in a molecule or an ion is defined as the number of charges it would carry if the electrons were completely transferred.

Explanation:

(1) The oxidation number or oxidation state does not always imply ionic charges on the species.

(2) The oxidation number of monoatomic ion is equal to charge of the ion. For example, Na^+ has + 1 charge while Cl^- has 1 charge, Ca²^+ has +2 charge and so on (But the oxidation states are 1+, 1-, 2+ respectively).

(3) In case of a neutral molecule, the sum of the oxidation numbers of all the constituent atoms is always zero.

(4) The charge on a polyatomic ion is equal to the algebraic sum of the oxidation numbers of all the constituent atoms of the ion.

(5) From the change in the oxidation numbers in a redox reaction, an oxidant and a reductant can be identified.

[Note : Oxidation number or oxidation state is represented as 1+, 2+, etc. while charge is represented as +1, + 2, etc.)