Question

Water is oxidized to oxygen by (a) \(\mathrm{H}_{2} \mathrm{O}_{2}\) (b) \(\mathrm{KMnO}_{4}\) (c) \(\mathrm{ClO}_{2}\) (d) fluorine

Short answer

(d) fluorine

Step-by-step solution

Understanding the Reaction

To determine which substance can oxidize water to oxygen, we need to identify if the substance is a strong oxidizing agent. Water becomes oxidized when its oxidation number increases from -2 in water to 0 in oxygen gas.

Analyzing Each Option

Let's analyze each option:(a) Hydrogen peroxide (\(\mathrm{H}_2\mathrm{O}_2\)) can act as both an oxidizing and a reducing agent, but typically reduces to water and oxygen.(b) Potassium permanganate (\(\mathrm{KMnO}_4\)) is a strong oxidizing agent and can act under acidic conditions to cause reactions which generate oxygen. (c) Chlorine dioxide (\(\mathrm{ClO}_2\)) can potentially oxidize various substances but is less commonly known for oxidizing water.(d) Fluorine is the strongest oxidizing agent known and can oxidize water to oxygen.

Identifying the Strongest Oxidizing Agent

Fluorine (\(\mathrm{F}_2\)) is identified as the strongest oxidizing agent and is capable of oxidizing water into oxygen gas under normal conditions.

Conclusion

The correct answer to which substance oxidizes water to oxygen is (d) fluorine, as it is the most powerful oxidizing agent among the given options.

Key concepts

Oxidizing Agents

In the world of chemistry, an oxidizing agent is a substance that can receive electrons from another substance. This action not only reduces the oxidizing agent itself but also causes the other substance to lose electrons—a process known as oxidation. Some substances are powerful oxidizing agents and can provoke intense reactions. These agents can typically force other substances to part with their electrons:

• Oxidizing agents generally have high electronegativity, meaning they readily attract electrons.
• Strong oxidizing agents include halogens like chlorine and highly electronegative molecules such as oxygen.

Oxidizing agents play vital roles in many chemical reactions, especially in redox processes where they facilitate the exchange of electrons. Understanding their ability to acquire electrons helps in predicting reaction outcomes.

Redox Reactions

Redox reactions, short for reduction-oxidation reactions, are chemical processes in which two species exchange electrons. One substance serves as the oxidizing agent, while the other acts as the reducing agent. During a redox reaction, several things happen:

• The oxidizing agent gains electrons and becomes reduced.
• The reducing agent loses electrons and becomes oxidized.
• Typically, this results in the transfer of energy.

Consider the oxidation of water to oxygen. In this type of redox reaction, water loses electrons (is oxidized), while a strong oxidizing agent like fluorine takes these electrons (is reduced). Observing these electron exchanges is crucial in recognizing how substances interact in their chemical environments.

Fluorine as an Oxidizing Agent

Fluorine stands out as the strongest oxidizing agent in chemistry. This attribute is due to its high electronegativity and ability to bind with almost all elements. Fluorine's prowess as an oxidizing agent enables it to effortlessly oxidize water to oxygen, even under standard conditions. Consider some of fluorine's properties:

• It readily captures electrons from other substances, oxidizing them in the process.
• Its reactions are often highly exothermic, producing considerable energy.
• Fluorine's ability to oxidize water to oxygen highlights its significant reactivity.

This makes fluorine indispensable in various industrial and chemical applications. Understanding fluorine’s oxidizing power provides insight into why it remains unmatched in chemical reactivity.