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Chapter 6: 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 something gains electrons, it is said to be reduced because its oxidation state has been decreased. The term "reduced" originates from early chemistry, where it was thought to mean the removal of oxygen. However, it now refers to the gain of electrons and the reduction of the oxidation state, making the atom more negative or less positive. The acronym OIL RIG (Oxidation Is Loss, Reduction Is Gain) can help remember this concept.

Step by step solution

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1. Understanding Redox Reactions

Redox reactions, short for reduction-oxidation reactions, are chemical reactions in which the oxidation state (or number) of one or more elements changes. In these reactions, two key processes occur: reduction and oxidation. These two processes always happen simultaneously, with one substance being reduced while another is being oxidized.
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2. Reduction and Oxidation

In a redox reaction, reduction refers to the process where a substance gains electrons, whereas oxidation is the process where a substance loses electrons. An easy way to remember this is by using the acronym OIL RIG: Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons).
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3. Origin of the Term "Reduced"

The term "reduced" in redox reactions has its origin in early chemistry, where reduction was thought to mean the removal of oxygen from a substance. As the understanding of chemistry developed, it was discovered that reduction actually involves a gain in electrons. However, the name "reduction" stuck because it still made sense in a different context: reduction of the oxidation state (or number).
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4. What is Being Reduced?

When something gains electrons and we say it is "reduced," we are actually referring to its decrease in oxidation state. The oxidation state of an atom is a number assigned to the atom in a molecule that signifies the atom's apparent charge. By gaining electrons, the atom becomes more negative or less positive, which means its oxidation state has been reduced or decreased. In conclusion, when something gains electrons in a redox reaction, it is said to be reduced because its oxidation state has been decreased. The term "reduced" originates from the early understanding of the removal of oxygen from a substance but now refers to the gain of electrons and the decrease in an oxidation state.

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Most popular questions from this chapter

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$ \begin{array}{c} \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) \\ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g) \end{array} $$ A \(10.00-\mathrm{g}\) mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with \(156 \mathrm{mL}\) of \(3.00 \mathrm{M}\) silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If \(78.0 \mathrm{mL}\) of HCl was added, what was the concentration of the HCl?

A \(25.00-\mathrm{mL}\) sample of hydrochloric acid solution requires \(24.16 \mathrm{mL}\) of \(0.106 \mathrm{M}\) sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?

A solution is prepared by dissolving \(10.8 \mathrm{g}\) ammonium sulfate in enough water to make \(100.0 \mathrm{mL}\) of stock solution. A \(10.00-\) mL sample of this stock solution is added to \(50.00 \mathrm{mL}\) of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

A standard solution is prepared for the analysis of fluoxymesterone \(\left(\mathrm{C}_{20} \mathrm{H}_{29} \mathrm{FO}_{3}\right),\) an anabolic steroid. A stock solution is first prepared by dissolving \(10.0 \mathrm{mg}\) of fluoxymesterone in enough water to give a total volume of \(500.0 \mathrm{mL}\). A \(100.0-\mu \mathrm{L}\) aliquot (portion) of this solution is diluted to a final volume of \(100.0 \mathrm{mL} .\) Calculate the concentration of the final solution in terms of molarity.

Specify which of the following are oxidation-reduction 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. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 4 \mathrm{HCl}(a q)+\mathrm{SiO}_{2}(s)\) d. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{Mg}(s) \rightarrow 2 \mathrm{MgCl}_{2}(s)+\mathrm{Si}(s)\) e. \(\mathrm{Al}(\mathrm{OH})_{4}^{-}(a q) \rightarrow \mathrm{AlO}_{2}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(i)\)
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