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Chapter 20: Problem 11

(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?

Short Answer

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(a) Oxidation is a chemical process in which a substance loses electrons, resulting in an increase in its oxidation state. It usually involves a gain of oxygen or a loss of hydrogen atoms. (b) In an oxidation half-reaction, electrons appear on the right side (product side) of the equation, as the reactant loses electrons transferred to another substance. (c) An oxidant, also known as an oxidizing agent or electron acceptor, is a substance that gains electrons from other substances during a chemical reaction, promoting their oxidation. (d) An oxidizing agent is a substance that causes another substance to lose electrons in a redox reaction. It gains electrons from the substance being oxidized and is reduced itself, driving the redox reaction forward.

Step by step solution

01

(a) Define Oxidation)

Oxidation is a chemical process in which a substance loses one or more electrons, resulting in an increase in its oxidation state. This process is usually accompanied by a gain of oxygen or a loss of hydrogen atoms. In simple terms, oxidation can be seen as the process where a molecule, atom, or ion becomes more positively charged due to the loss of electrons.
02

(b) Side of Oxidation Half-reaction)

In an oxidation half-reaction, the electrons appear on the right side (or the product side) of the equation. This is because the reactant (substance being oxidized) is losing electrons, and these electrons are then transferred to another substance.
03

(c) Define Oxidant)

An oxidant, also known as an oxidizing agent or electron acceptor, is a substance that has the ability to gain electrons from other substances during a chemical reaction. In other words, it promotes the oxidation of other substances by accepting the electrons released during the oxidation process.
04

(d) Define Oxidizing Agent)

An oxidizing agent is a substance that causes another substance to lose electrons in a redox reaction. It gains electrons from the substance being oxidized and, therefore, is reduced itself. The oxidizing agent is essential in driving the redox reaction forward, as it is responsible for removing electrons from the reducing agent (or the substance being oxidized) and facilitating the electron transfer process.

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Most popular questions from this chapter

(a) What does the term electromotive force mean? (b) What is the definition of the volt? (c) What does the term cell potential mean?

Gold exists in two common positive oxidation states, \(+1\) and \(+3\). The standard reduction potentials for these oxidation states are $$ \begin{aligned} \mathrm{Au}^{+}(a q)+\mathrm{e}^{-}-\longrightarrow \mathrm{Au}(s) & E_{\mathrm{red}}^{\circ}=+1.69 \mathrm{~V} \\ \mathrm{Au}^{3+}(a q)+3 \mathrm{e}^{-}-\ldots \mathrm{Au}(s) & E_{\mathrm{red}}^{\circ}=+1.50 \mathrm{~V} \end{aligned} $$ (a) Can you use these data to explain why gold does not tarnish in the air? (b) Suggest several substances that should be strong enough oxidizing agents to oxidize gold metal. (c) Miners obtain gold by soaking goldcontaining ores in an aqueous solution of sodium cyanide. A very soluble complex ion of gold forms in the aqueous solution because of the redox reaction $$ \begin{array}{r} 4 \mathrm{Au}(s)+8 \mathrm{NaCN}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)-\longrightarrow \\ 4 \mathrm{Na}\left[\mathrm{Au}(\mathrm{CN})_{2}\right](a q)+4 \mathrm{NaOH}(a q) \end{array} $$ What is being oxidized, and what is being reduced, in this reaction? (d) Gold miners then react the basic aqueous product solution from part (c) with Zn dust to get gold metal. Write a balanced redox reaction for this process. What is being oxidized, and what is being reduced?

This oxidation-reduction reaction in acidic solution is spontaneous: \(5 \mathrm{Fe}^{2+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}^{+}(a q)-\rightarrow\) \(5 \mathrm{Fe}^{3+}(a q)+\mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l)\) A solution containing \(\mathrm{KMnO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is poured into one beaker, and a solution of \(\mathrm{FeSO}_{4}\) is poured into another. A salt bridge is used to join the beakers. A platinum foil is placed in each solution, and a wire that passes through a voltmeter connects the two solutions. (a) Sketch the cell, indicating the anode and the cathode, the direction of electron movement through the external circuit, and the direction of ion migrations through the solutions. (b) Sketch the process that occurs at the atomic level at the surface of the anode. (c) Calculate the emf of the cell under standard conditions. (d) Calculate the emf of the cell at \(298 \mathrm{~K}\) when the concentrations are the following: \(\mathrm{pH}=0.0, \quad\left[\mathrm{Fe}^{2+}\right]=0.10 \mathrm{M}, \quad\left[\mathrm{MnO}_{4}^{-}\right]=1.50 \mathrm{M}\) \(\left[\mathrm{Fe}^{3+}\right]=2.5 \times 10^{-4} \mathrm{M},\left[\mathrm{Mn}^{2+}\right]=0.001 \mathrm{M}\)

(a) Which electrode of a voltaic cell, the cathode or the anode, corresponds to the higher potential energy for the electrons? (b) What are the units for electrical potential? How does this unit relate to energy expressed in joules? (c) What is special about a standard cell potential?

At \(900^{\circ} \mathrm{C}\) titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction. (b) What is being oxidized, and what is being reduced? (c) Which substance is the reductant, and which is the oxidant?
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