Question

Which of the following is MOST likely to act as a stronger oxidizing agent than phosphorus? A. \(\mathrm{Na}\) B. Cs C. \(\mathrm{O}\) D. Bi

Short answer

C. \(\text{O}\)

Step-by-step solution

– Understand the Concept of Oxidizing Agents

Oxidizing agents are substances that gain electrons in a chemical reaction and, in the process, oxidize another substance. Strong oxidizing agents have a high affinity for gaining electrons.

– Identify the Properties of Each Element

Review the properties of each given element to determine their ability to gain electrons:- \(\text{Na}\) (Sodium) is a metal and tends to lose electrons easily.- \(\text{Cs}\) (Cesium) is similar to sodium and also tends to lose electrons.- \(\text{O}\) (Oxygen) is a non-metal and has a high tendency to gain electrons.- \(\text{Bi}\) (Bismuth) is a metal that does not gain electrons as readily as oxygen.

– Compare Elements to Phosphorus

Phosphorus (P) is a non-metal, and its position in the periodic table suggests it is more inclined to gain electrons than metals like Na, Cs, and Bi. However, compare it specifically with Oxygen (O), which is also a non-metal.

– Determine the Stronger Oxidizing Agent

Oxygen is known to be one of the strongest oxidizing agents due to its high electronegativity and ability to gain electrons readily. Therefore, it is more likely to act as a stronger oxidizing agent than phosphorus.

Key concepts

Electron Affinity

When talking about oxidizing agents, it's important to understand electron affinity. This concept describes the ability of an atom to accept an electron. In simple terms, it tells you how much an atom 'wants' an extra electron. Atoms with high electron affinity tend to be good oxidizing agents because they readily gain electrons in chemical reactions. Oxygen, for example, has a high electron affinity because it strongly attracts electrons to itself. As a result, it often acts as a powerful oxidizing agent, making other substances lose electrons.

Periodic Table

The periodic table is a crucial tool in chemistry. It organizes elements in a way that showcases their properties systematically. Elements are arranged by their atomic number, which is the number of protons in an atom's nucleus. By looking at the periodic table, you can quickly understand an element's characteristics, including its tendency to gain or lose electrons. Non-metals, like oxygen and phosphorus, are typically found on the right side of the periodic table. These elements generally have higher electron affinities compared to metals, which are mostly on the left side. Metals like sodium (Na) and cesium (Cs) tend to lose electrons and are thus poor oxidizing agents.

Electronegativity

Electronegativity is another key concept linked to oxidizing agents. It measures an atom's tendency to attract electrons within a chemical bond. The higher the electronegativity, the stronger the pull on the electrons. Oxygen has a very high electronegativity, which is why it’s often involved in reactions as an oxidizing agent. Phosphorus has lower electronegativity than oxygen, which is why oxygen is the better oxidizing agent between the two. Electronegativity generally increases as you move from left to right across a period and decreases as you move down a group in the periodic table.

Chemical Reactions

Understanding oxidizing agents requires some knowledge of chemical reactions. In a redox (reduction-oxidation) reaction, the oxidizing agent gains electrons and, in the process, causes another substance to lose electrons (get oxidized). These chemical reactions are fundamental to many processes, including metabolism in the human body and industrial chemical manufacturing. Knowing which elements can act as strong oxidizing agents can help predict and explain outcomes in these reactions. For instance, oxygen is frequently used in processes needing strong oxidation capabilities due to its high electron affinity and electronegativity.