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Chapter 19: Problem 10

Describe the roles of oxidizing agents and reducing agents in a redox reaction. How is each changed in the reaction?

Short Answer

Expert verified
In a redox reaction, the oxidizing agent facilitates oxidation by accepting electrons from another species and getting reduced itself, while the reducing agent promotes reduction by donating electrons to another species and getting oxidized itself. The oxidizing agent experiences a reduction in its oxidation state, whereas the reducing agent undergoes an increase in its oxidation state. These changes can be observed in the balanced redox reaction, such as the reaction between hydrogen and oxygen to form water: \(2H_2 + O_2 \rightarrow 2H_2O\), where oxygen is the oxidizing agent and hydrogen is the reducing agent.

Step by step solution

01

Definition: Redox Reactions

Redox reactions are chemical reactions that involve a transfer of electrons between two species. One species gains electrons (reduction) while the other species loses electrons (oxidation).
02

Oxidizing Agent

An oxidizing agent is a chemical species that causes the oxidation of another species in the reaction. The oxidizing agent accepts electrons from another species and gets reduced itself. It is called an oxidizing agent because, by accepting electrons, it causes the oxidation or electron loss in another substance.
03

Reducing Agent

A reducing agent is a chemical species that causes the reduction of another species in the reaction. The reducing agent donates electrons to another species and gets oxidized itself. It is called a reducing agent because, by donating electrons, it facilitates the reduction or electron gain in another substance.
04

Changes in Oxidizing and Reducing Agents

In a redox reaction, both oxidizing and reducing agents undergo changes. The oxidizing agent accepts electrons and experiences a reduction in its oxidation state. Conversely, the reducing agent donates electrons and undergoes an increase in its oxidation state. These changes in oxidation states can be observed in the balanced redox reaction. For example, consider the reaction between hydrogen and oxygen to form water: \(2H_2 + O_2 \rightarrow 2H_2O\) In this reaction: - Oxygen (O2) is the oxidizing agent: it gains electrons from hydrogen and is reduced to water (H2O). - Hydrogen (H2) is the reducing agent: it loses electrons to oxygen and is oxidized to water (H2O). Overall, the redox reaction shows the interplay between oxidizing agents and reducing agents, where they act in support of each other to facilitate the transfer of electrons between chemical species.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidizing Agent
An oxidizing agent plays a crucial role in a redox reaction. It is the chemical species that causes oxidation of another substance by accepting electrons from it. When it accepts these electrons, it undergoes reduction.

Here are some key points to remember about oxidizing agents:
  • They are the species that gain electrons.
  • During a redox reaction, their oxidation state decreases.
  • Common examples include oxygen, chlorine, and fluorine, which are very good at gaining electrons.
In the reaction of hydrogen and oxygen to form water, oxygen acts as an oxidizing agent. It gains electrons from hydrogen, thus reducing its own oxidation state to form water.
Reducing Agent
The reducing agent in a redox reaction is the species that donates electrons to another substance, effectively causing the reduction of that substance. As it donates electrons, it gets oxidized itself.

Here's what to keep in mind about reducing agents:
  • They are the species that lose electrons during the reaction.
  • Their oxidation state increases due to electron loss.
  • Examples include hydrogen, carbon, and metals like sodium and lithium, which easily give up their electrons.
In the reaction forming water, hydrogen is the reducing agent because it donates electrons to oxygen and is oxidized in the process.
Electron Transfer
Electron transfer is the fundamental mechanism behind redox reactions. It involves the movement of electrons from one substance to another. This transfer is what drives the changes in the oxidation states of the oxidizing and reducing agents.

In any redox reaction:
  • The reducing agent donates electrons, resulting in its oxidation.
  • The oxidizing agent accepts those electrons, leading to its reduction.
To visualize this, picture an electron jumping from one atom to another. In our example of water formation, electrons from hydrogen atoms "leap" to oxygen atoms, enabling the redox reaction.
Oxidation State
Understanding oxidation states is essential for grasping redox reactions. The oxidation state, or oxidation number, indicates the number of electrons an atom gains or loses in a reaction. It helps keep track of electron transfers in redox reactions.

When analyzing oxidation states:
  • A decrease in oxidation state indicates reduction (gain of electrons).
  • An increase in oxidation state indicates oxidation (loss of electrons).
For instance, in the water formation reaction, oxygen starts with an oxidation state of zero in O鈧� and ends with -2 in H鈧侽, signifying it has gained electrons. Conversely, hydrogen moves from zero in H鈧� to +1 in H鈧侽, indicating it has lost electrons.

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Most popular questions from this chapter

Determine the oxidation number of the boldface element in each of the following a. \({OF}_{2}\) b. \({UO}_{2}^{2+}\) c. \({RuO}_{4}\) d. \({Fe}_{2} {O}_{3}\)

Use the half-reaction method to balance the redox equations. Begin by writing the oxidation and reduction half-reactions. Leave the balanced equation in ionic form. Challenge \(\mathrm{N}_{2} \mathrm{O}(\mathrm{g})+\mathrm{ClO}^{-}(\mathrm{aq}) \rightarrow \mathrm{NO}_{2}^{-}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})\) (in basic solution)

How does the oxidation number in an oxidation process relate to the number of electrons lost? How does the change in oxidation number in a reduction process relate to the number of electrons gained?

Silverware Practice your technical writing skills by writing a procedure for cleaning tarnished silverware by a redox chemical process. Be sure to include background information describing the process as well as logical steps that would enable anyone to accomplish the task.

Use the half-reaction method to balance these equations for redox reactions. Add water molecules and hydrogen ions (in acid solutions) or hydroxide ions (in basic solutions) as needed a. \(\mathrm{NH}_{3}(\mathrm{g})+\mathrm{NO}_{2}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1)\) b. \(\mathrm{Br}_{2} \rightarrow \mathrm{Br}^{-}+\mathrm{BrO}_{3}^{-}(\text { in basic solution })\)
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