Question

An oxidizing agent causes the (oxidation/reduction) of another species, and the oxidizing agent itself is (oxidized/reduced).

Short answer

An oxidizing agent causes the \(oxidation\) of another species, and the oxidizing agent itself is \(reduced\).

Step-by-step solution

Understand the role of an oxidizing agent

An oxidizing agent is a chemical species that gains electrons from other species during a redox reaction. In other words, it causes another species to lose electrons.

Determine the action of an oxidizing agent on another species

Since the oxidizing agent causes another species to lose electrons, we can say that it causes the (oxidation) of another species. This is because oxidation is defined as the process of losing electrons.

Determine what happens to the oxidizing agent itself

As the oxidizing agent gains electrons from another species, it undergoes (reduction), which is the process of gaining electrons. So, the oxidizing agent itself is (reduced).

Final answer

An oxidizing agent causes the (oxidation) of another species, and the oxidizing agent itself is (reduced).

Key concepts

Redox Reactions

Redox reactions, short for reduction-oxidation reactions, are fundamental chemical processes where electrons are transferred between molecules, atoms, or ions. During a redox reaction, two simultaneous occurrences take place: oxidation and reduction. Understanding redox reactions is crucial for a plethora of applications in chemistry, such as metabolism in biology, batteries in physics, or corrosion processes in materials science.

In the realm of redox reactions, an oxidizing agent plays a key role; it is the substance that receives electrons, thereby getting reduced itself. Meanwhile, the substance that donates electrons is oxidized. It's similar to a dance where one partner (the reducing agent) offers a hand (electrons) and the other partner (the oxidizing agent) accepts it, leading to a coordinated movement (electron transfer). This transfer of electrons is what drives the dance of chemistry in a redox reaction.

Oxidation Process

The oxidation process is an essential half of a redox reaction where a substance loses electrons. Imagine it as the substance giving away pieces of itself, in the form of electrons. In chemical terms, we often say a species is oxidized when its oxidation state increases. This could be due to losing electrons to another atom, ion, or molecule during the reaction.

An easy way to remember this is by using the mnemonic OIL RIG, which stands for 'Oxidation Is Loss, Reduction Is Gain' of electrons. During oxidation, the substance that loses the electrons is known as the reducing agent because it 'reduces' the charge of the oxidizing agent by providing electrons.

Signs of Oxidation

• Loss of electrons
• Increase in oxidation state
• Release of energy
• Often involves the formation of oxides when oxygen is involved

Reduction Process

The reduction process is the other half of the redox equation, where a substance gains electrons, thus reducing its oxidation state. This is basically the opposite of oxidation. When a substance gains electrons, it is said to be reduced. The agent that causes this electron gain is called the oxidizing agent since it 'oxidizes' the other substance and gets reduced in the process.

Reduction is vital in many chemical processes, from industrial synthesis to biological respiration.

Characteristics of Reduction

• Gain of electrons
• Decrease in oxidation state
• Often accompanied by an energy gain in the substance being reduced
• Can result in the formation of new compounds

These concepts are two sides of the same coin and always occur together in a redox reaction.