Which Best Describes The Reducing Agent In The Reaction Below?${ Cl_2(aq) + 2 Br^{-}(aq) \longrightarrow 2 Cl^{-}(aq) + Br_2(aq) }$A. Bromine (Br) Loses An Electron, So It Is The Reducing Agent.B. Bromine (Br) Gains An Electron, So It Is The
Which Best Describes the Reducing Agent in the Reaction Below?
Understanding Redox Reactions
Redox reactions, also known as oxidation-reduction reactions, involve the transfer of electrons from one species to another. In these reactions, one species loses electrons, while another species gains electrons. The species that loses electrons is called the oxidizing agent, while the species that gains electrons is called the reducing agent.
The Reaction: Chlorine and Bromide
The reaction below is a classic example of a redox reaction:
In this reaction, chlorine gas (Cl2) reacts with bromide ions (Br-) to form chloride ions (Cl-) and bromine molecules (Br2).
Identifying the Reducing Agent
To determine which species is the reducing agent, we need to look at the reaction and identify which species loses or gains electrons.
The Oxidation State of Bromine
In the reaction, bromine (Br) is initially in the form of bromide ions (Br-). As the reaction proceeds, bromine is converted into bromine molecules (Br2). This means that the oxidation state of bromine changes from -1 to 0.
The Oxidation State of Chlorine
In the reaction, chlorine (Cl) is initially in the form of chlorine gas (Cl2). As the reaction proceeds, chlorine is converted into chloride ions (Cl-). This means that the oxidation state of chlorine changes from 0 to -1.
Which Species Loses or Gains Electrons?
Since the oxidation state of bromine changes from -1 to 0, it means that bromine gains electrons. On the other hand, since the oxidation state of chlorine changes from 0 to -1, it means that chlorine loses electrons.
Conclusion
Based on the analysis above, we can conclude that bromine (Br) is the reducing agent in the reaction below. This is because bromine gains electrons as it is converted from bromide ions (Br-) to bromine molecules (Br2).
Why is Bromine the Reducing Agent?
Bromine is the reducing agent because it has a greater tendency to gain electrons than chlorine. In other words, bromine is more easily oxidized than chlorine. This is because bromine has a higher electronegativity than chlorine, which means that it has a greater tendency to attract electrons.
The Role of the Oxidizing Agent
In the reaction, chlorine (Cl) is the oxidizing agent. This is because chlorine loses electrons as it is converted from chlorine gas (Cl2) to chloride ions (Cl-). The oxidizing agent is responsible for accepting electrons from the reducing agent, which in this case is bromine.
The Importance of Redox Reactions
Redox reactions are an important class of chemical reactions that play a crucial role in many natural and industrial processes. They are involved in the formation of many important compounds, including acids, bases, and salts. Understanding redox reactions is essential for understanding many chemical and biological processes.
Conclusion
In conclusion, the reducing agent in the reaction below is bromine (Br). This is because bromine gains electrons as it is converted from bromide ions (Br-) to bromine molecules (Br2). The oxidizing agent in the reaction is chlorine (Cl), which loses electrons as it is converted from chlorine gas (Cl2) to chloride ions (Cl-). Understanding redox reactions is essential for understanding many chemical and biological processes.
Key Takeaways
- Redox reactions involve the transfer of electrons from one species to another.
- The species that loses electrons is called the oxidizing agent, while the species that gains electrons is called the reducing agent.
- In the reaction below, bromine (Br) is the reducing agent because it gains electrons as it is converted from bromide ions (Br-) to bromine molecules (Br2).
- Chlorine (Cl) is the oxidizing agent because it loses electrons as it is converted from chlorine gas (Cl2) to chloride ions (Cl-).
References
- Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
- Brown, T. E., & LeMay, H. E. (2014). Chemistry: The Central Science (13th ed.). Pearson Education.
- Chang, R. (2010). Chemistry: The Central Science (11th ed.). McGraw-Hill.