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Chapter 4: Problem 6

Why is it that when something gains electrons, it is said to be reduced? What is being reduced?

Short Answer

Expert verified
In a redox reaction, when a species gains electrons, it is said to be reduced because its overall charge is reduced due to the additional negative charges. This decrease in oxidation state indicates that the species involved has lost positive charge during the reaction. What is being reduced is the oxidizing agent, which accepts electrons from another species, while the reducing agent loses electrons and is oxidized. Both processes occur simultaneously in a redox reaction. For example, in the formation of water from hydrogen and oxygen, oxygen is the component being reduced as it gains electrons.

Step by step solution

01

Understanding Oxidation and Reduction in Chemistry

Oxidation and reduction are two processes that are part of redox (reduction-oxidation) reactions in chemistry. In a redox reaction, one reactant gets oxidized (loses electrons), while the other reactant gets reduced (gains electrons). These two processes occur simultaneously.
02

Explaining Reduction in terms of Electron Gain

In a redox reaction, reduction is the process where a species gains electrons. When a species gains electrons, its overall charge is reduced due to the additional negative charges. The term "reduction" implies a decrease in oxidation state, indicating that the species involved has lost positive charge (become less positive) during the reaction.
03

Identifying What is Being Reduced

When we say that something gains electrons and is being reduced, we are referring to the oxidizing agent in the reaction. The oxidizing agent accepts electrons from another species and is thus reduced. Conversely, the reducing agent loses electrons and is oxidized. In any redox reaction, both processes (oxidation and reduction) occur simultaneously. For example, for a redox reaction between hydrogen (H) and oxygen (O) to form water (H2O), the reaction can be represented as: \[ 2H_2 + O_2 \rightarrow 2H_2O \] In this redox reaction, hydrogen is being oxidized (losing electrons and becoming more positive) to form water. Oxygen, on the other hand, is being reduced (gaining electrons and becoming less positive), also forming water. In this case, what is being reduced is the oxygen molecule (O2).

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Key Concepts

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

Oxidation
In chemistry, oxidation is a fundamental concept in redox reactions. When oxidation occurs, it involves a loss of electrons. This means a molecule, atom, or ion initially has more electrons, and during the process of oxidation, these electrons are moved away. Therefore, the species undergoing oxidation becomes more positive due to the decrease in negative charges (electrons).

A common way to remember this is by the phrase "OIL RIG," which stands for "Oxidation Is Loss, Reduction Is Gain." This helps to keep in mind that during oxidation, something is losing electrons鈥攁 key point in understanding redox reactions. By knowing which species get oxidized, you can better predict and understand chemical reactions.
  • Oxidation involves the increase in oxidation state (loss of electrons).
  • Common in reactions like rusting, burning, and cellular respiration.
  • An oxidized species often transfers its electrons to another species (the oxidizing agent).
Reduction
Reduction is the flip side of oxidation. In a redox reaction, while one substance is oxidized, another is reduced. Reduction involves the gain of electrons, making the atom or molecule less positive or more negative.

The term "reduction" refers to the decrease in oxidation state. This means that as species gain electrons, they become more negatively charged due to the added negative charges.
  • Reduction results in a decrease in oxidation state.
  • It often accompanies oxidation, as the two occur in tandem in redox reactions.
  • Reduction is essential in processes like photosynthesis, where plants reduce carbon dioxide to glucose.
Understanding reduction is crucial because it explains how chemical reactions balance out鈥攖hey're always a combination of electron loss and gain.
Oxidizing Agent
An oxidizing agent is an essential player in a redox reaction. As the name suggests, its role is to oxidize another reactant by accepting electrons from it. In doing so, the oxidizing agent itself becomes reduced during the process.

Consider it as the entity that promotes the oxidation of others while undergoing a reduction. For example, in the reaction between hydrogen and oxygen to form water, oxygen serves as the oxidizing agent. It accepts electrons from hydrogen, thereby getting reduced to form water molecules.
  • The oxidizing agent gains electrons and gets reduced.
  • It leads to the oxidation of another substance.
  • Common examples include oxygen (O2), hydrogen peroxide (H2O2), and halogens like chlorine (Cl2).
Understanding the role of an oxidizing agent helps to map out the electron transfer processes in a reaction, making it smoother to understand and predict the outcomes.

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Most popular questions from this chapter

What mass of solid \(\mathrm{AgBr}\) is produced when \(100.0 \mathrm{~mL}\) of \(0.150 \mathrm{MAgNO}_{3}\) is added to \(20.0 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{NaBr} ?\)

A \(500.0-\mathrm{mL}\) sample of \(0.200 M\) sodium phosphate is mixed with \(400.0 \mathrm{~mL}\) of \(0.289 M\) barium chloride. What is the mass of the solid produced?

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\). A \(0.205-g\) sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The \(\mathrm{BaSO}_{4}\) that is formed is filtered, dried, and weighed. Its mass is \(0.298 \mathrm{~g}\). What mass of \(\mathrm{SO}_{4}^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}{ }^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

You are given a \(1.50-\mathrm{g}\) mixture of sodium nitrate and sodium chloride. You dissolve this mixture into \(100 \mathrm{~mL}\) of water and then add an excess of \(0.500 \mathrm{M}\) silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of \(0.641 \mathrm{~g}\). a. If you had an extremely magnified view of the solution (to the atomic- molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.

A \(50.00-\mathrm{mL}\) sample of aqueous \(\mathrm{Ca}(\mathrm{OH})_{2}\) requires \(34.66 \mathrm{~mL}\) of a \(0.944-M\) nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.
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