Question

“Reducing agents are electron acceptors”. Is the statement true or false?

• A. True
• B. False

Answer 1

The correct option is B False

• The reaction in which one or more electrons are lost by a species is called an oxidation reaction. In the oxidation process, the oxidation number of a substance increases by the loss of electrons.
• The reaction in which one or more electrons are gained by a species is called a reduction reaction. In the reduction process, the oxidation number of a substance decreases by the gain of electrons.
• The reducing agent is the species that reduces other substances but oxidizes itself in the reaction. Example, Iron(III) ion (Fe³⁺) is formed by the loss of one electron (${\mathrm{e}}^{-}$) from Iron(II) ion (Fe²⁺).

${\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)\to {\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}$

• The oxidation number of Iron (Fe) is +2 in Fe²⁺ and +3 in Fe³⁺. Therefore, the loss of electrons results in an increase in the oxidation number of Fe which implies that oxidation of Iron(II) (Fe²⁺) takes place.
• Since Iron(II) (Fe²⁺) undergoes oxidation in the reaction by losing one electron, it acts as the reducing agent.
• Hence, reducing agents are electron donors, not electron acceptors.
• Hence, the statement is false.