Bromine is obtained from sea water by the following redox...

Bromine is obtained from sea water by the following redox reaction: $$\mathrm{Cl}_{2}(\mathrm{g})+2 \mathrm{NaBr}(\mathrm{aq}) \rightarrow 2 \mathrm{NaCl}(\mathrm{aq})+\mathrm{Br}_{2}(\ell)$$ (a) What has been oxidized? What has been reduced? (b) Identify the oxidizing and reducing agents.

Bromine is obtained from sea water by the following redox reaction:
$$\mathrm{Cl}_{2}(\mathrm{g})+2 \mathrm{NaBr}(\mathrm{aq}) \rightarrow 2 \mathrm{NaCl}(\mathrm{aq})+\mathrm{Br}_{2}(\ell)$$
(a) What has been oxidized? What has been reduced?
(b) Identify the oxidizing and reducing agents.

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Key Concepts

Oxidation

Oxidation refers to the chemical process in which a substance loses electrons. In redox reactions, the species that undergoes oxidation experiences an increase in oxidation state, and this process is fundamental when analyzing how electrons are transferred between reactants.

Reduction

Reduction is the process by which a substance gains electrons, resulting in a decrease in its oxidation state. In the context of redox reactions, the species that is reduced accepts electrons from another species, often leading to significant changes in its chemical properties.

Oxidizing Agent

An oxidizing agent is a substance that facilitates oxidation by accepting electrons from another species, thereby becoming reduced itself. It is responsible for causing the oxidation of the other reactant in a redox reaction.

Reducing Agent

A reducing agent is a substance that causes reduction by donating electrons to another substance, resulting in its own oxidation. In redox reactions, this agent is the electron donor, enabling the reduction of another species.

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