Reducing agents are mostly non-metals while oxidizing agents are mostly metals.

State whether the given statement is true or false.

• A. True
• B. False

The statement that reducing agents are mostly non-metals while oxidizing agents are mostly metals is actually false. The correct understanding of reducing and oxidizing agents involves a bit more nuance regarding their chemical properties and roles in redox reactions.

Understanding Redox Reactions

In a redox (reduction-oxidation) reaction, one substance loses electrons (is oxidized) while another gains electrons (is reduced). The substance that donates electrons is called the reducing agent, and the one that accepts electrons is the oxidizing agent.

Characteristics of Reducing Agents

Reducing agents are typically substances that can easily lose electrons. While many non-metals can act as reducing agents, especially in certain contexts, it is more common for metals to serve this role. For instance:

• Alkali Metals: Elements like sodium (Na) and potassium (K) readily lose electrons to form positive ions, making them excellent reducing agents.
• Transition Metals: Metals such as iron (Fe) and zinc (Zn) can also act as reducing agents in various reactions.

Characteristics of Oxidizing Agents

Oxidizing agents, on the other hand, are substances that gain electrons. While many oxidizing agents are indeed metals, particularly in their ionic forms, there are also notable non-metals that serve this function:

• Halogens: Elements like chlorine (Cl) and fluorine (F) are powerful oxidizing agents because they readily accept electrons.
• Oxygen: As a non-metal, oxygen is one of the most common oxidizing agents in various chemical reactions.

Conclusion on the Statement

Given this information, the assertion that reducing agents are mostly non-metals while oxidizing agents are mostly metals is misleading. Both categories can include a variety of elements from different groups in the periodic table. Therefore, the correct answer to the question is B. False.