Which Of The Following Species Is Undergoing Oxidation In The Reaction Below?${ 2 \text{CuBr} \rightarrow 2 \text{Cu} + \text{Br}_2 }$A. ${\text{Br}^-}$ B. ${\text{Br}_2}$ C. Cu D. ${\text{Cu}^+}$ E. CuBr

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Oxidation is a fundamental concept in chemistry that involves the loss of electrons by an atom, molecule, or ion. It is a crucial aspect of chemical reactions, and understanding oxidation is essential to comprehend the underlying mechanisms of various chemical processes. In this article, we will delve into the concept of oxidation and identify the species undergoing oxidation in a given chemical reaction.

What is Oxidation?

Oxidation is a chemical reaction that involves the loss of one or more electrons by an atom, molecule, or ion. This process results in the formation of a new compound with a different oxidation state. Oxidation is often accompanied by the gain of electrons by another atom, molecule, or ion, which is known as reduction.

Types of Oxidation

There are several types of oxidation, including:

  • Redox reactions: These are chemical reactions that involve both oxidation and reduction processes.
  • Oxidation of metals: This involves the loss of electrons by a metal atom, resulting in the formation of a metal ion.
  • Oxidation of nonmetals: This involves the loss of electrons by a nonmetal atom, resulting in the formation of a nonmetal ion.

The Given Reaction

The given reaction is:

2CuBr→2Cu+Br2{ 2 \text{CuBr} \rightarrow 2 \text{Cu} + \text{Br}_2 }

In this reaction, copper(I) bromide (CuBr) is converted into copper (Cu) and bromine (Br2). We need to identify the species undergoing oxidation in this reaction.

Analysis of the Reaction

To determine the species undergoing oxidation, we need to analyze the reaction and identify the changes in oxidation states.

  • Copper (Cu): In the reactant, copper is present as CuBr, which means it has an oxidation state of +1. In the product, copper is present as Cu, which means it has an oxidation state of 0. This indicates that copper has lost one electron, resulting in a decrease in oxidation state.
  • Bromine (Br): In the reactant, bromine is present as CuBr, which means it has an oxidation state of -1. In the product, bromine is present as Br2, which means it has an oxidation state of 0. This indicates that bromine has gained one electron, resulting in an increase in oxidation state.

Conclusion

Based on the analysis of the reaction, we can conclude that the species undergoing oxidation is copper (Cu). Copper has lost one electron, resulting in a decrease in oxidation state from +1 to 0.

Answer

The correct answer is:

  • C. Cu

Discussion

The given reaction is a classic example of a redox reaction, where copper is oxidized and bromine is reduced. Oxidation is a crucial aspect of chemical reactions, and understanding it is essential to comprehend the underlying mechanisms of various chemical processes.

Key Takeaways

  • Oxidation is a chemical reaction that involves the loss of electrons by an atom, molecule, or ion.
  • Oxidation is often accompanied by the gain of electrons by another atom, molecule, or ion, which is known as reduction.
  • The given reaction is a classic example of a redox reaction, where copper is oxidized and bromine is reduced.
  • Copper is the species undergoing oxidation in the given reaction.

References

  • Atkins, P. W., & De Paula, J. (2010). Physical chemistry. Oxford University Press.
  • Brown, T. E., LeMay, H. E., Bursten, B. E., & Murphy, C. (2012). Chemistry: The Central Science. Pearson Education.
  • Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2011). General chemistry: Principles and modern applications. Pearson Education.
    Frequently Asked Questions (FAQs) on Oxidation =====================================================

Oxidation is a fundamental concept in chemistry that involves the loss of electrons by an atom, molecule, or ion. It is a crucial aspect of chemical reactions, and understanding oxidation is essential to comprehend the underlying mechanisms of various chemical processes. In this article, we will address some frequently asked questions (FAQs) on oxidation.

Q: What is the difference between oxidation and reduction?

A: Oxidation is the loss of electrons by an atom, molecule, or ion, while reduction is the gain of electrons by an atom, molecule, or ion. Oxidation and reduction are two complementary processes that occur simultaneously in a redox reaction.

Q: What is the oxidation state of an atom in a compound?

A: The oxidation state of an atom in a compound is the hypothetical charge that the atom would have if it were a free ion. It is a measure of the degree of oxidation of the atom.

Q: How do you determine the oxidation state of an atom in a compound?

A: To determine the oxidation state of an atom in a compound, you need to follow these steps:

  1. Assign the oxidation state of the atom with the highest electronegativity (usually oxygen or fluorine) as -2.
  2. Assign the oxidation state of the atom with the lowest electronegativity (usually hydrogen or alkali metals) as +1.
  3. Add the oxidation states of all the atoms in the compound to get the total charge of the compound.
  4. Subtract the total charge of the compound from the sum of the oxidation states of the atoms to get the oxidation state of the remaining atom.

Q: What is the difference between oxidation and combustion?

A: Oxidation is the loss of electrons by an atom, molecule, or ion, while combustion is a specific type of oxidation reaction that involves the reaction of a substance with oxygen to produce heat and light.

Q: Can oxidation occur without oxygen?

A: Yes, oxidation can occur without oxygen. This type of oxidation is called non-aqueous oxidation or anhydrous oxidation.

Q: What is the role of oxidation in biological systems?

A: Oxidation plays a crucial role in biological systems, including:

  1. Energy production: Oxidation is involved in the production of energy in cells through the process of cellular respiration.
  2. Detoxification: Oxidation is involved in the detoxification of harmful substances in the body.
  3. Immune response: Oxidation is involved in the immune response, where it helps to kill pathogens.

Q: Can oxidation be reversed?

A: Yes, oxidation can be reversed through a process called reduction. Reduction involves the gain of electrons by an atom, molecule, or ion, which can restore the original oxidation state.

Q: What are some common examples of oxidation reactions?

A: Some common examples of oxidation reactions include:

  1. Rusting of iron: Iron reacts with oxygen to form iron oxide, which is rust.
  2. Burning of wood: Wood reacts with oxygen to produce heat and light.
  3. Corrosion of metals: Metals react with oxygen to form oxides, which can lead to corrosion.

Q: How can oxidation be prevented or minimized?

A: Oxidation can be prevented or minimized through various methods, including:

  1. Using antioxidants: Antioxidants can help to prevent oxidation by neutralizing free radicals.
  2. Storing substances in airtight containers: Storing substances in airtight containers can help to prevent oxidation.
  3. Using inert atmospheres: Using inert atmospheres, such as nitrogen or argon, can help to prevent oxidation.

Conclusion

Oxidation is a fundamental concept in chemistry that involves the loss of electrons by an atom, molecule, or ion. It is a crucial aspect of chemical reactions, and understanding oxidation is essential to comprehend the underlying mechanisms of various chemical processes. By addressing some frequently asked questions (FAQs) on oxidation, we hope to have provided a better understanding of this complex topic.