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Chapter 20: Problem 14

(a) What is meant by the term reduction? (b) On which side of a reduction half-reaction do the electrons appear? (c) What is meant by the term reductant? (d) What is meant by the term reducing agent?

Short Answer

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(a) Reduction is a chemical process where a substance gains electrons, resulting in a decrease of its oxidation state. (b) In a reduction half-reaction, electrons appear on the left-hand side (reactant side) of the equation. (c) A reductant, also known as a reducing agent, is a substance that donates electrons to another substance, causing the reduction of that substance. (d) A reducing agent is a substance that donates electrons to another substance, thus causing the reduction of that substance, and gets oxidized in the process.

Step by step solution

01

(a) Definition of reduction

Reduction is a chemical process in which a substance gains electrons, resulting in a decrease of its oxidation state. This process is the opposite of oxidation, in which a substance loses electrons and its oxidation state increases.
02

(b) Electrons in a reduction half-reaction

In a reduction half-reaction, electrons appear on the left-hand side (or reactant side) of the equation. This is because the substance undergoing reduction is gaining these electrons to achieve a lower oxidation state.
03

(c) Definition of reductant

A reductant, also known as a reducing agent, is a substance that donates electrons to another substance, thus causing the reduction of that substance. In a redox (reduction-oxidation) reaction, the reductant gets oxidized, while the substance it donates electrons to undergoes reduction.
04

(d) Definition of reducing agent

A reducing agent, also known as a reductant, is a substance that donates electrons to another substance, thus causing the reduction of that substance. Reducing agents play a crucial role in redox (reduction-oxidation) reactions, as they get oxidized while the substance they donate electrons to undergoes reduction.

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Key Concepts

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

Reduction
Reduction is a fundamental concept in redox reactions. It describes the process where a substance gains electrons. As electrons are negatively charged, when a substance gains them, its oxidation state decreases. This makes reduction the exact opposite of oxidation, where electrons are lost, and oxidation state increases. Consider how with more electrons, there's an increase in negative charge, leading to a reduction in the oxidation level. This mathematical representation is helpful:
  • Before reduction: higher oxidation state
  • After gaining electrons: lower oxidation state
Think of reduction as a scenario where electrons play the hero's role, joining the atoms and calming things down by reducing charge.
Oxidation State
Oxidation state, sometimes known as oxidation number, is a vital concept for understanding electron transfer in chemical reactions. It essentially represents the degree of oxidation of an atom, which can change as the atom gains or loses electrons. Each atom in a molecule can have different oxidation states, depending on its chemical environment. When a substance is reduced, its oxidation state decreases, which indicates that it has gained electrons:
  • An increase in oxidation state means loss of electrons (oxidation).
  • A decrease in oxidation state indicates gain of electrons (reduction).
By tracking oxidation states, chemists can map out how electrons are moving in a reaction and understand which substances are reducing or oxidizing agents.
Reducing Agent
In any redox reaction, a reducing agent plays a crucial role by donating electrons to another substance. This donation causes the reduction of the other substance. Sometimes mistaken as making itself weaker, the reducing agent actually is an electron donor powerhouse. As it donates electrons, it is itself oxidized because it loses those electrons:
  • Reduces another substance by donating electrons.
  • Becomes oxidized after donating electrons.
Think of a reducing agent as someone sharing a flashlight in the dark 鈥� it sends the light (electrons) over, lighting up the path (reducing the other substance) even as it runs out of supplies and gets dimmer (oxidized).
Electrons
Electrons are like the tiny workhorses of redox reactions. They are the particles that transfer between substances, driving the chemical changes at the heart of these processes. In redox reactions, electrons are moved from one atom or molecule to another, allowing for the transformation of substances. When considering a reduction half-reaction:
  • Electrons appear on the left-hand side, highlighting their addition to the substance getting reduced.
It's essential to view electrons as not just mere charges, but critical players enabling substances to gain stability through reduction. Understanding where electrons are in a reaction helps clarify how substances change and interact chemically.

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Most popular questions from this chapter

Disulfides are compounds that have \(S-S\) bonds, like peroxides have \(\mathrm{O}-\mathrm{O}\) bonds. Thiols are organic compounds that have the general formula \(\mathrm{R}-\mathrm{SH}\), where \(\mathrm{R}\) is a generic hydrocarbon. The \(\mathrm{SH}^{-}\) ion is the sulfur counterpart of hydroxide, \(\mathrm{OH}^{-}\). Two thiols can react to make a disulfide, \(\mathrm{R}-\mathrm{S}-\mathrm{S}-\mathrm{R} .\) (a) What is the oxidation state of sulfur in a thiol? (b) What is the oxidation state of sulfur in a disulfide? (c) If you react two thiols to make a disulfide, are you oxidizing or reducing the thiols? (d) If you wanted to convert a disulfide to two thiols, should you add a reducing agent or oxidizing agent to the solution? (e) Suggest what happens to the H's in the thiols when they form disulfides.

(a) A \(\mathrm{Cr}^{3+}(a q)\) solution is electrolyzed, using a current of \(7.60 \mathrm{~A}\). What mass of \(\mathrm{Cr}(s)\) is plated out after 2.00 days? (b) What amperage is required to plate out \(0.250 \mathrm{~mol} \mathrm{Cr}\) from a \(\mathrm{Cr}^{3+}\) solution in a period of \(8.00 \mathrm{~h}\) ?

A voltaic cell is constructed that uses the following reaction and operates at \(298 \mathrm{~K}\) : $$ \mathrm{Zn}(s)+\mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Ni}(s) $$ (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when \(\left[\mathrm{Ni}^{2+}\right]=3.00 \mathrm{M}\) and \(\left[\mathrm{Zn}^{2+}\right]=0.100 \mathrm{M} ?(\mathbf{c})\) What is the emf of the cell when \(\left[\mathrm{Ni}^{2+}\right]=0.200 M\) and \(\left[\mathrm{Zn}^{2+}\right]=0.900 \mathrm{M} ?\)

(a) What is meant by the term oxidation? (b) On which side of an oxidation half-reaction do the electrons appear? (c) What is meant by the term oxidant? (d) What is meant by the term oxidizing agent?

(a) Suppose that an alkaline battery was manufactured using cadmium metal rather than zinc. What effect would this have on the cell emf? (b) What environmental advantage is provided by the use of nickel-metal hydride batteries over nickel-cadmium batteries?
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