What is an oxidizing agent?

Oxidizing and reducing agents are key terms used to describe reactants in redox (reduction-oxidation) reactions that transfer electrons between reactants to form product.

Oxidizing and reducing agents

An oxidizing agent is one that gains electrons and is reduced in a chemical reaction. Also known as an electron acceptor, the oxidizing agent is normally in one of its highest possible oxidation states, because it will gain electrons and be reduced. Some examples of oxidizing agents are halogens, potassium nitrate, and nitric acid.

A reducing agent, on the other hand, loses electrons and is oxidized in a chemical reaction. A reducing agent is usually in one of its lowest possible oxidation states and is known as an electron donor. A reducing agent oxidizes because it loses electrons in the redox reaction, also known as the reduction-oxidation reaction. Some examples of reducing agents are earth metals, formic acid, and sulfite compounds.

Oxidation state

The oxidation state shows the total number of electrons that have been removed from an element (a positive oxidation state) or added to an element (a negative oxidation state) to get to its current state.

Therefore, it is important that we keep two things in mind:

1. Oxidation involves an increase in the oxidation state.
2. Reduction implies a decrease in the oxidation state.

Recognizing this simple pattern is at the heart of the oxidation state concept, because if we know how the oxidation state of an element changes during a reaction, we can also instantly tell if it is being oxidized or reduced without having to work in terms of means. electron equations and electron transfers.

Applications

Oxidizing and reducing agents are important in industrial applications. These are used in processes such as water purification, fabric bleaching, and energy storage such as batteries and gasoline. Oxidizing and reducing agents are especially crucial in biological processes such as metabolism and photosynthesis. For example, organisms use electron acceptors such as NAD+ to harvest energy from redox reactions such as the hydrolysis of glucose:

C ₆ H ₁₂ O ₆ +2ADP+2P+2NAD ⁺ →2CH ₃ COCO ₂ H+2ATP+2NADH

All combustion reactions are also examples of redox reactions. A combustion reaction occurs when a substance reacts with oxygen to generate heat. An example is the combustion of octane, the main component of gasoline:

2C ₈ H ₁₈ (l)+25O ₂ (g)→16CO ₂ (g)+18H ₂ O(g)

Combustion reactions are also an important source of energy for modern industry.

Fountain

Academic Resource Center. (nd). Oxidation-Reduction Reactions.