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Chapter 4: Problem 71

In a certain reaction, \(\mathrm{Cu}^{+}\) is converted to \(\mathrm{Cu}^{2+}\). Is \(\mathrm{Cu}^{+}\) ion oxidized or reduced in this reaction? Is \(\mathrm{Cu}^{+}\) ion an oxidizing agent or a reducing agent in this reaction?

Short Answer

Expert verified
\( \mathrm{Cu}^{+} \) is oxidized and acts as a reducing agent.

Step by step solution

01

Understanding Oxidation and Reduction

Oxidation is a process where an ion, atom, or molecule loses electrons, while reduction is a process where electrons are gained. Here, we need to determine whether the transition from \( \mathrm{Cu}^{+} \) to \( \mathrm{Cu}^{2+} \) involves a gain or loss of electrons.
02

Electron Change Calculation

In this reaction, \( \mathrm{Cu}^{+} \) is transitioning to \( \mathrm{Cu}^{2+} \). To determine this, observe:\[ \mathrm{Cu}^{+} \rightarrow \mathrm{Cu}^{2+} + e^{-} \]This equation shows the loss of one electron (\( e^- \)), indicating oxidation.
03

Determining Oxidizing or Reducing Agent

An oxidizing agent is a substance that causes oxidation by accepting electrons. Conversely, a reducing agent donates electrons and is themselves oxidized. Since \( \mathrm{Cu}^{+} \) loses an electron, it is oxidized and acts as a reducing agent.

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Key Concepts

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

Electron Transfer
Electron transfer is a fundamental concept in chemistry, especially when discussing oxidation and reduction. When we talk about reactions, electrons can move from one atom, ion, or molecule to another.
In the reaction where \( \mathrm{Cu}^{+} \) converts to \( \mathrm{Cu}^{2+} \), there's a loss of one electron. This shows how electron transfer plays a critical role, dictating whether a substance undergoes oxidation or reduction.
  • If an entity gains electrons, we call it reduction.
  • If an entity loses electrons, we term it oxidation.
In this instance, since \( \mathrm{Cu}^{+} \) loses an electron, it is oxidized, depicting a clear electron transfer occurring during the reaction.
Oxidizing Agent
Understanding what an oxidizing agent is can be tricky, but it's crucial for grasping redox reactions. An oxidizing agent is a species that facilitates the oxidation of another by being reduced itself.
Essentially, it accepts electrons. Think of it like a friend who takes on your burden, which in this case is electrons.
In our reaction, \( \mathrm{Cu}^{+} \) is not an oxidizing agent, as it loses an electron rather than gaining one. When you notice a substance getting reduced in a reaction, that particular substance acts as the oxidizing agent, making the process of identifying it easier.
Reducing Agent
A reducing agent is slightly different from an oxidizing agent. It donates electrons to another substance, causing the reduction of that substance.
In simple terms, a reducing agent is like someone who gives a gift (electrons, in this case) to another.
This generous gesture means the reducing agent itself is oxidized.
  • It donates electrons and gets oxidized in return.
  • It's responsible for reducing the other component by handing over electrons.
In the conversion of \( \mathrm{Cu}^{+} \) to \( \mathrm{Cu}^{2+} \), \( \mathrm{Cu}^{+} \) acts as a reducing agent as it sacrifices its electrons to the reaction, allowing others to be reduced.

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Most popular questions from this chapter

Caffeine, a central nervous system stimulant, has the molecular formula \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{N}_{4} \mathrm{O}_{2}\) (a) How many moles of caffeine are present in \(6.19 \times 10^{25}\) molecules of caffeine? (b) Imagine you dissolve caffeine in water to a volume of \(100.0 \mathrm{mL}\), which is known to have a density of \(1.23 \mathrm{g} / \mathrm{mL}\). How many molecules of caffeine are present in this volume? (c) How many nitrogen atoms are present in \(3.5 \mathrm{mg}\) of caffeine? (d) Complete the skeletal structure of caffeine, where all the bonded atoms are shown but double bonds, triple bonds, and/or lone pairs are missing. (e) Identify the various types of geometries present in each central atom of caffeine using VSEPR theory. (f) Determine the various relative bond angles associated with each central atom of caffeine using VSEPR theory. (g) What is the most polar bond in caffeine? (h) Would you predict caffeine to be polar or nonpolar? (i) Consider the combustion of caffeine, which results in formation of \(\mathrm{NO}_{2}(\mathrm{g})\) as well as other expected products. Write a balanced chemical equation for this reaction. (j) The heat of combustion for caffeine is \(2211 \mathrm{kcal} / \mathrm{mol} .\) How much heat will be given off if \(0.81 \mathrm{g}\) of caffeine is burned completely? (k) Calculate the weight of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) that can be prepared from \(8.00 \mathrm{g}\) of caffeine mixed with \(20.3 \mathrm{g}\) of oxygen gas.

Calculate the number of moles of: (a) 0 atoms in 18.1 mol of formaldehyde, \(\mathrm{CH}_{2} \mathrm{O}\) (b) \(\mathrm{Br}\) atoms in \(0.41 \mathrm{mol}\) of bromoform, \(\mathrm{CHBr}_{3}\) (c) \(\quad O\) atoms in \(3.5 \times 10^{3}\) mol of \(A l_{2}\left(S O_{4}\right)_{3}\) (d) \(\mathrm{Hg}\) atoms in \(87 \mathrm{g}\) of \(\mathrm{HgO}\)

A sample of gold consisting of \(8.68 \times 10^{23}\) atoms with a density of \(19.3 \mathrm{g} / \mathrm{mL}\) is hammered into a sheet that covers an area of \(1.00 \times 10^{2} \mathrm{ft}^{2}\). Determine the thick- ness of the sheet in centimeters.

When a piece of sodium metal is added to water, hydrogen is evolved as a gas and a solution of sodium hydroxide is formed. (a) Write a balanced equation for this reaction. (b) What is oxidized in this reaction? What is reduced?

The rusting of iron is a chemical reaction of iron with oxygen in the air to form iron(III) oxide. Write a balanced equation for this reaction.
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