Which Best Describes The Oxidizing Agent In This Reaction? C L 2 ( A Q ) + 2 B R − ( A Q ) ⟶ 2 C L − ( A Q ) + B R 2 ( A Q Cl_2(aq) + 2 Br^{-}(aq) \longrightarrow 2 Cl^{-}(aq) + Br_2(aq C L 2 ​ ( A Q ) + 2 B R − ( A Q ) ⟶ 2 C L − ( A Q ) + B R 2 ​ ( A Q ]A. Bromine (Br) Is The Oxidizing Agent Because It Gains An Electron. B. Bromine (Br) Is The Oxidizing Agent Because It

Introduction

Chemical reactions involve the transfer of electrons, resulting in the formation of new substances. In these reactions, certain substances can act as either oxidizing or reducing agents. An oxidizing agent is a substance that causes another substance to lose one or more electrons, resulting in the gain of oxygen or the loss of hydrogen. In this article, we will explore which best describes the oxidizing agent in the given reaction: $Cl_2(aq) + 2 Br^{-}(aq) \longrightarrow 2 Cl^{-}(aq) + Br_2(aq)$.

What is an Oxidizing Agent?

An oxidizing agent is a substance that causes another substance to lose one or more electrons, resulting in the gain of oxygen or the loss of hydrogen. Oxidizing agents are typically strong oxidizers, meaning they have a high tendency to accept electrons from other substances. In the context of the given reaction, we need to determine which substance is the oxidizing agent.

The Given Reaction

The given reaction is: $Cl_2(aq) + 2 Br^{-}(aq) \longrightarrow 2 Cl^{-}(aq) + Br_2(aq)$. In this reaction, chlorine gas ($Cl_2$) reacts with bromide ions ($Br^{-}$) to form chloride ions ($Cl^{-}$) and bromine gas ($Br_2$).

Analyzing the Reaction

To determine which substance is the oxidizing agent, we need to examine the oxidation states of the atoms involved in the reaction. The oxidation state of an atom is a measure of its ability to gain or lose electrons.

• Chlorine gas ($Cl_2$) has an oxidation state of 0, as it is a diatomic molecule.
• Bromide ions ($Br^{-}$) have an oxidation state of -1, as they have gained one electron.
• Chloride ions ($Cl^{-}$) have an oxidation state of -1, as they have gained one electron.
• Bromine gas ($Br_2$) has an oxidation state of 0, as it is a diatomic molecule.

Determining the Oxidizing Agent

Based on the analysis of the oxidation states, we can see that bromide ions ($Br^{-}$) have an oxidation state of -1, while bromine gas ($Br_2$) has an oxidation state of 0. This indicates that bromide ions have lost one electron to form bromine gas, resulting in the gain of oxygen.

Conclusion

Based on the analysis of the oxidation states, we can conclude that bromine (Br) is the oxidizing agent in the given reaction. This is because bromide ions ($Br^{-}$) have lost one electron to form bromine gas ($Br_2$), resulting in the gain of oxygen.

Answer

The correct answer is B. Bromine (Br) is the oxidizing agent because it gains an electron.

Why is Bromine the Oxidizing Agent?

Bromine is the oxidizing agent in this reaction because it gains an electron from the bromide ions ($Br^{-}$). This results in the formation of bromine gas ($Br_2$), which has an oxidation state of 0. The gain of an electron by bromine is a characteristic of an oxidizing agent, as it causes another substance to lose one or more electrons.

Key Takeaways

• An oxidizing agent is a substance that causes another substance to lose one or more electrons, resulting in the gain of oxygen or the loss of hydrogen.
• In the given reaction, bromine (Br) is the oxidizing agent because it gains an electron from the bromide ions ($Br^{-}$).
• The gain of an electron by bromine is a characteristic of an oxidizing agent, as it causes another substance to lose one or more electrons.

Common Misconceptions

• Some students may mistakenly believe that bromine (Br) is the reducing agent in this reaction, as it gains an electron. However, this is incorrect, as the gain of an electron by bromine is a characteristic of an oxidizing agent.
• Others may believe that chlorine gas ($Cl_2$) is the oxidizing agent in this reaction, as it is a strong oxidizer. However, this is also incorrect, as chlorine gas is not the substance that gains an electron in this reaction.

Conclusion

Q: What is an oxidizing agent?

A: An oxidizing agent is a substance that causes another substance to lose one or more electrons, resulting in the gain of oxygen or the loss of hydrogen.

Q: How do you determine which substance is the oxidizing agent in a reaction?

A: To determine which substance is the oxidizing agent, you need to examine the oxidation states of the atoms involved in the reaction. The substance that gains an electron is the oxidizing agent.

Q: What is the difference between an oxidizing agent and a reducing agent?

A: An oxidizing agent is a substance that causes another substance to lose one or more electrons, resulting in the gain of oxygen or the loss of hydrogen. A reducing agent is a substance that causes another substance to gain one or more electrons, resulting in the loss of oxygen or the gain of hydrogen.

Q: Can a substance be both an oxidizing agent and a reducing agent?

A: Yes, a substance can be both an oxidizing agent and a reducing agent, depending on the reaction. For example, in the reaction $Cl_2(aq) + 2 Br^{-}(aq) \longrightarrow 2 Cl^{-}(aq) + Br_2(aq)$, chlorine gas ($Cl_2$) is the oxidizing agent, but in the reaction $2 Cl^{-}(aq) + Br_2(aq) \longrightarrow 2 Cl^{-}(aq) + Br^{-}(aq)$, chlorine gas ($Cl_2$) is the reducing agent.

Q: How do you identify the oxidizing agent in a reaction with multiple substances?

A: To identify the oxidizing agent in a reaction with multiple substances, you need to examine the oxidation states of all the substances involved in the reaction. The substance that gains an electron is the oxidizing agent.

Q: Can a substance be an oxidizing agent if it does not gain an electron?

A: No, a substance cannot be an oxidizing agent if it does not gain an electron. An oxidizing agent is a substance that causes another substance to lose one or more electrons, resulting in the gain of oxygen or the loss of hydrogen.

Q: What is the role of an oxidizing agent in a reaction?

A: The role of an oxidizing agent in a reaction is to cause another substance to lose one or more electrons, resulting in the gain of oxygen or the loss of hydrogen.

Q: Can an oxidizing agent be a gas, liquid, or solid?

A: Yes, an oxidizing agent can be a gas, liquid, or solid. For example, chlorine gas ($Cl_2$) is a gas, while potassium permanganate ($KMnO_4$) is a solid.

Q: How do you store oxidizing agents safely?

A: To store oxidizing agents safely, you need to follow proper safety protocols, such as storing them in a well-ventilated area, away from heat sources, and in a container that is designed to prevent leakage.

Q: Can oxidizing agents be used in everyday life?

A: Yes, oxidizing agents are used in everyday life, such as in bleach, disinfectants, and cleaning products.

Q: What are some common examples of oxidizing agents?

A: Some common examples of oxidizing agents include chlorine gas ($Cl_2$), potassium permanganate ($KMnO_4$), and hydrogen peroxide ($H_2O_2$).

Q: Can oxidizing agents be used in industrial processes?

A: Yes, oxidizing agents are used in industrial processes, such as in the production of bleach, disinfectants, and cleaning products.

Q: What are some safety precautions to take when handling oxidizing agents?

A: Some safety precautions to take when handling oxidizing agents include wearing protective gear, such as gloves and goggles, and following proper safety protocols, such as storing them in a well-ventilated area, away from heat sources, and in a container that is designed to prevent leakage.