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Ch.4 - Reactions in Aqueous Solution
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
All textbooksBrown 15th EditionCh.4 - Reactions in Aqueous SolutionProblem 45a
Chapter 4, Problem 45a

True or false: a. If a substance is oxidized, it is gaining electrons.

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1
Understand the concept of oxidation: Oxidation is a chemical process where a substance loses electrons.
Recall the mnemonic 'OIL RIG': Oxidation Is Loss, Reduction Is Gain, which helps remember that oxidation involves the loss of electrons.
Analyze the statement: 'If a substance is oxidized, it is gaining electrons.'
Compare the statement with the definition of oxidation: Since oxidation involves losing electrons, the statement contradicts the definition.
Conclude that the statement is false because a substance that is oxidized loses electrons, not gains them.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation and Reduction

Oxidation and reduction are chemical processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. These processes are often coupled, meaning that when one substance is oxidized, another is reduced. Understanding these definitions is crucial for analyzing redox reactions.
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Electron Transfer

In redox reactions, the transfer of electrons is fundamental to the changes in oxidation states of the involved species. When a substance is oxidized, it loses electrons, resulting in an increase in its oxidation state. Conversely, the substance that gains these electrons is reduced, leading to a decrease in its oxidation state. This electron transfer is key to understanding the behavior of substances in chemical reactions.

Oxidation States

Oxidation states (or numbers) are a way to keep track of electrons in chemical compounds. They indicate the degree of oxidation of an atom in a molecule and help identify which atoms are oxidized and which are reduced during a reaction. By analyzing oxidation states, one can determine the flow of electrons and the overall redox process, which is essential for answering questions about oxidation and reduction.
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Related Practice
Textbook Question

Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.

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Textbook Question

Determine the oxidation number for the indicated element in each of the following substances: a. S in SO2

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(a) Which region of the periodic table shown here contains elements that are easiest to oxidize? (b) Which region contains the least readily oxidized elements?

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Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, BaSO4 (b) sulfurous acid, H2SO3 (c) strontium sulfide, SrS

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Textbook Question

Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: FeO(s) + 2 HClO4(aq) → Fe(ClO4)2(aq) + H2O(l) (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between NiO(s) and an aqueous solution of nitric acid.

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