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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 oxidation state decreases, signifying a reduction in its level of oxidation. The term "reduced" means the decrease in the oxidation state of a chemical species due to electron gain. What is being reduced is the oxidation state of the species, making it less oxidized.

Step by step solution

01

Understand Reduction and Oxidation

Reduction and oxidation, also known as redox reactions, are chemical processes that involve the transfer of electrons between two species. In a redox reaction, one species gains electrons (reduction) while the other species loses electrons (oxidation).
02

Identify the Reduced Species

In a chemical reaction, the species gaining electrons is termed as the reduced species. This is because when a species gains electrons, it experiences an increase in its negative charge. It means that the oxidation state (a measure of the degree of oxidation of an atom in a chemical compound) has decreased. For example, consider the following reaction: \[Cu^{2+ (aq)} + 2e^- \rightarrow Cu(s)\] In this case, the copper ion (Cu虏鈦�) gains 2 electrons (2e鈦�) and is reduced to a solid copper metal (Cu). As you can see, the oxidation state of copper decreases from +2 to 0, that means it has experienced reduction.
03

Define "Reduced" in the Context of Reduction

The term "reduced" in the context of a redox reaction refers to the decrease in the oxidation state of a chemical species when it gains electrons. In other words, "reduced" essentially means the decrease in the level of oxidation of that species due to the electron gain.
04

Explain What is Being Reduced

In a redox reaction, what is being reduced is the oxidation state of the species. As a species gains electrons, its oxidation state decreases, making it less oxidized and therefore "reduced". In summary, when a species gains electrons in a chemical reaction, it is said to be "reduced" because the process leads to a decrease in its oxidation state. This change signifies a reduction in its level of oxidation.

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Most popular questions from this chapter

A sample may contain any or all of the following ions: \(\mathrm{Hg}_{2}^{2+}\) \(\mathrm{Ba}^{2+}\) and \(\mathrm{Mn}^{2+}\) a. No precipitate formed when an aqueous solution of NaCl was added to the sample solution. b. No precipitate formed when an aqueous solution of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) was added to the sample solution. c. A precipitate formed when the sample solution was made basic with NaOH. Which ion or ions are present in the sample solution?

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

Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were started simultaneously. The total volume in the beaker at the stoichiometric point is 655 mL. Calculate the flow rates of burets Y and Z. Assume the flow rates remain constant during the experiment.

Specify which of the following are oxidation鈥搑eduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. a. \(\mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \rightarrow 2 \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)\) b. \(\mathrm{HCl}(g)+\mathrm{NH}_{3}(g) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\) c. \(\mathrm{SiCl}_{4}(i)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 4 \mathrm{HCl}(a q)+\mathrm{SiO}_{2}(s)\) d. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{Mg}(s) \rightarrow 2 \mathrm{MgCl}_{2}(s)+\mathrm{Si}(s)\) e. \(\mathrm{Al}(\mathrm{OH})_{4}-(a q) \rightarrow \mathrm{AlO}_{2}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

What mass of iron(III) hydroxide precipitate can be produced by reacting 75.0 mL of 0.105 M iron(III) nitrate with 125 mL of 0.150 M sodium hydroxide?
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