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Chapter 20: Problem 2

You may have heard that "antioxidants" are good for your health. Is an "antioxidant" an oxidizing agent or a reducing agent?

Short Answer

Expert verified
An antioxidant is a reducing agent, as it prevents oxidation of other molecules by donating electrons, neutralizing free radicals, and stabilizing them in the process.

Step by step solution

01

Define Antioxidant

An antioxidant is a molecule that inhibits or prevents the oxidation of other molecules by donating an electron to a free radical, thus neutralizing it. Oxidation is a chemical reaction that involves the loss of electrons or an increase in oxidation state, while reduction is a chemical reaction that involves the gain of electrons or a decrease in oxidation state.
02

Understand Oxidizing Agent and Reducing Agent

An oxidizing agent is a substance that gains electrons or reduces its oxidation state during the redox (reduction-oxidation) reaction, whereas a reducing agent is a substance that loses electrons or increases its oxidation state during the redox reaction.
03

Identify the Role of Antioxidants in Redox Reactions

Since antioxidants prevent oxidation by donating electrons, they act as a reducing agent, which loses electrons during the redox reaction. By donating electrons, they decrease the oxidation state of the free radicals, thus stabilizing them.
04

Conclusion

Based on the provided information, an antioxidant acts as a reducing agent—since it inhibits or prevents oxidation of other molecules by donating electrons, neutralizing free radicals and stabilizing them in the process.

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Most popular questions from this chapter

Iron corrodes to produce rust, \(\mathrm{Fe}_{2} \mathrm{O}_{3},\) but other corrosion products that can form are \(\mathrm{Fe}(\mathrm{O})(\mathrm{OH})\), iron oxyhydroxide, and magnetite, \(\mathrm{Fe}_{3} \mathrm{O}_{4} .\) (a) What is the oxidation number of Fe in iron oxyhydroxide, assuming oxygen's oxidation number is \(-2 ?(\mathbf{b})\) The oxidation number for Fe in magnetite was controversial for a long time. If we assume that oxygen's oxidation number is \(-2,\) and Fe has a unique oxidation number, what is the oxidation number for Fe in magnetite? (c) It turns out that there are two different kinds of Fe in magnetite that have different oxidation numbers. Suggest what these oxidation numbers are and what their relative stoichiometry must be, assuming oxygen's oxidation number is -2 .

(a) In the Nernst equation, what is the numerical value of the reaction quotient, \(Q,\) under standard conditions? (b) Can the Nernst equation be used at temperatures other than room temperature?

Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (a) \(\mathrm{Mo}^{3+}(a q) \longrightarrow \mathrm{Mo}(s)\) (acidic solution) (b) $\mathrm{H}_{2} \mathrm{SO}_{3}(a q) \longrightarrow \mathrm{SO}_{4}^{2-}(a q)$ (acidic solution) (c) \(\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{NO}(g)\) (acidic solution) (d) \(\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)\) (acidic solution) (e) \(\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)\) (basic solution) (f) \(\mathrm{Mn}^{2+}(a q) \longrightarrow \mathrm{MnO}_{2}(s)\) (basic solution) (g) $\mathrm{Cr}(\mathrm{OH})_{3}(s) \longrightarrow \mathrm{CrO}_{4}^{2-}(a q)$ (basic solution)

(a) Write the half-reaction that occurs at an oxygen electrode in acidic aqueous solution when it serves as the cathode of a voltaic cell. (b) Write the half-reaction that occurs at an oxygen electrode in acidic aqueous solution when it serves as the anode of a voltaic cell. (c) What is standard about the standard oxygen electrode?

Consider the half-reaction $\mathrm{Ag}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)$ (a) Which of the lines in the following diagram indicates how the reduction potential varies with the concentration of \(\mathrm{Ag}^{+}(a q) ?(\mathbf{b})\) What is the value of \(E_{\text {red }}\) when \(\log \left[\mathrm{Ag}^{+}\right]=0 ?\)
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