Question

Which element is the reducing agent in a redox reaction?
O
A. The reactant that has the atom that gets oxidized
O
B. The product that has the atom that was oxidized
C. The reactant that has the atom that gets reduced
O
D. The product that has the atom that was reduced
SUBMI

Answer 1

Answer:

The reactant that has the atom that gets oxidized

Explanation:

A redox reaction is a reaction in which one substance is oxidized and one is reduced. The easiest way to remember the patterns of any redox reaction is to follow a simple abbreviation: OILRIG.

This acronym stands for: oxidation is loss, reduction is gain (of electrons). Therefore, if a substance is oxidized, then it loses electrons. If a substance is reduced, it gains electrons.

Let's take a look at the following example:

$Cu (s) + 2 Ag^+ (aq)\rightarrow Cu^{2+} (aq) + 2 Ag (s)$

Notice that copper loses two electrons, as it becomes positively charged:

$Cu (s)\rightarrow Cu^{2+} (aq) + 2e^-$

Since electrons are on the right-hand side, it means we produce them (they are lost). Hence, copper in this equation is oxidized. Similarly:

$Ag^+(aq)+e^-\rightarrow Ag(s)$

Now, silver cation gains electrons to become solid silver, neutrally charged, meaning it is reduced.

In terms of an oxidizing/reducing agents, the thought process is opposite: in an oxidation process, we have a reducing agent, hence, Cu (s) is our reducing agent. In a reduction process, we have an oxidizing agent, hence, silver cation is our oxidizing agent.

Both reducing and oxidizing agents are reactants.

Therefore, reducing agent is a reactant that has the atom that gets oxidized.

Answer 2

Answer: A

Explanation:

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