Question

Drawing Conclusions A substance has an element in one of its highest possible oxidation states. Is this substance more likely to be an oxidizing agent or a reducing agent? Explain your reasoning.

Short answer

The substance is more likely to be an oxidizing agent because it is in a high oxidation state and tends to gain electrons.

Step-by-step solution

Understand Oxidation States

An element in a high oxidation state has lost many electrons. Oxidation states indicate the degree of oxidation (loss of electrons) of an element.

Define Oxidizing and Reducing Agents

An oxidizing agent gains electrons and gets reduced. A reducing agent loses electrons and gets oxidized.

Apply the Definitions to the Substance

Given that the substance has an element in one of its highest possible oxidation states, it has lost many electrons and is thus likely to gain electrons.

Draw the Conclusion

Since the substance with an element in a high oxidation state is likely to gain electrons, it acts as an oxidizing agent as it will oxidize other substances.

Key concepts

Oxidation States

Oxidation states, also known as oxidation numbers, are a way of keeping track of electrons in atoms while they form compounds. Each element in a compound is assigned a number that represents its oxidation state. The oxidation state indicates the total number of electrons an element has lost, gained, or shared when forming chemical bonds.
For example, in its highest oxidation state, an element has lost a significant number of electrons. This value is important because it gives us clues about the chemical behavior of the element.
High oxidation states often mean the element is more reactive and has a greater tendency to gain electrons to return to a more stable state.

Oxidizing Agent

An oxidizing agent is a substance that causes another substance to lose electrons during a chemical reaction. In turn, the oxidizing agent gains those electrons. Simply put, oxidizing agents are substances that get reduced.
For example:

• When an oxidizing agent participates in a reaction, it pulls electrons off another substance.
• This electron gain reduces the oxidizing agent.
• Common oxidizing agents include oxygen, hydrogen peroxide, and certain acids.

Understanding that an element in its highest oxidation state is likely to act as an oxidizing agent can help predict the outcome of chemical reactions.

Reducing Agent

A reducing agent is the opposite of an oxidizing agent. It donates electrons to another substance, thus getting oxidized in the process. This means a reducing agent causes the reduction of another substance while it itself gets oxidized.
For example:

• When a reducing agent takes part in a reaction, it gives away electrons to another substance.
• This electron donation oxidizes the reducing agent.
• Common reducing agents include hydrogen, carbon monoxide, and metals like sodium or magnesium.

Reducing agents are powerful because they help substances gain electrons, altering their chemical state.

Electron Transfer

Electron transfer refers to the movement of electrons from one atom or molecule to another during chemical reactions. It's a fundamental concept that underlies oxidation and reduction.
When an atom loses electrons, it gets oxidized, and when it gains electrons, it gets reduced.
This transfer of electrons is a key part of redox (reduction-oxidation) reactions. For example:

• Oxidizing agents gain electrons (are reduced).
• Reducing agents donate electrons (are oxidized).

Understanding electron transfer helps in grasping why substances behave as they do in chemical reactions and why an element in its high oxidation state tends to act as an oxidizing agent.