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Chapter 49: Problem 7

Describe, in grammatically correct English sentences, how one can determine whether or not a reaction is an oxidation-reduction reaction.

Short Answer

Expert verified
To determine if a reaction is a redox reaction, assign oxidation numbers to all atoms in the reactants and products. Then compare these numbers to identify any changes. If an atom's oxidation number increases, it's being oxidized; if it decreases, it's being reduced. If both processes are happening simultaneously, the reaction is a redox reaction.

Step by step solution

01

Definition

To identify a redox reaction, it's important to understand what Redox reactions are. Redox reactions are chemical reactions where oxidation and reduction occur simultaneously. In these reactions, one element gets oxidized (loses electrons), and another element gets reduced (gains electrons).
02

Identify the Oxidation Numbers

The first step in identifying a redox reaction is to assign oxidation numbers to all atoms present in the reactants and the products. An Oxidation number refers to the charge an atom of element would have if all its bonds to atoms of different elements were 100% ionic.
03

Compare the Oxidation Numbers

The second step is to compare the oxidation numbers of every atom in the reactants and the products. The atoms which exhibit a change in oxidation number are involved in the redox reaction.
04

Determine Oxidation and Reduction

After comparing oxidation numbers, identify the atoms that undergo oxidation and reduction. If the oxidation number of an atom increases during the reaction, that atom is oxidized. If the oxidation number of an atom decreases during the reaction, that atom is reduced.
05

Confirm Redox Reaction

A redox reaction will always involve both oxidation and reduction. If you can identify both an element that was oxidized and an element that was reduced, you have a redox reaction.

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Most popular questions from this chapter

In which of the following are the oxidation number and the partial charge the same number? \(\mathrm{MgO} ; \mathrm{CO}_{2} ; \mathrm{NaF} ; \mathrm{H}_{2} \mathrm{O} ; \mathrm{CCl}_{4} ; \mathrm{NiCl}_{2}\).

Is a species that has an atom for which there is an increase in oxidation number oxidized or reduced? Is that species the oxidizing agent or the reducing agent?

Which is the better representation of the actual charge on an atom in a moleculethe formal charge; the partial charge; the oxidation state? Why?
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