Skip to main content
Ch.4 - Reactions in Aqueous Solution
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook
All textbooksMcMurry 8th EditionCh.4 - Reactions in Aqueous SolutionProblem 42d
Chapter 4, Problem 42d

Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (d) SbCl4-(aq) → SbCl6-(aq)

Verified step by step guidance
1
Identify the oxidation states of the central atom (Sb) in both the reactant and the product.
In SbCl_4^- (aq), determine the oxidation state of Sb by considering the oxidation state of Cl as -1.
In SbCl_6^- (aq), determine the oxidation state of Sb by considering the oxidation state of Cl as -1.
Compare the oxidation states of Sb in the reactant and product to determine if it has increased or decreased.
If the oxidation state of Sb increases, it is an oxidation reaction; if it decreases, it is a reduction reaction.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
6m
Was this helpful?

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 species. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction involves the gain of electrons, leading to a decrease in oxidation state. These processes are always coupled, meaning that when one species is oxidized, another must be reduced.
Recommended video:
Guided course
01:53
Oxidation and Reduction Reactions

Oxidation States

Oxidation states (or oxidation numbers) are a way to keep track of electron transfer in redox reactions. Each element in a compound is assigned an oxidation state based on its electron configuration and bonding. Understanding how to assign oxidation states is crucial for identifying which species is oxidized and which is reduced in a half-reaction.
Recommended video:
Guided course
02:42
Oxidation Numbers

Half-Reactions

Half-reactions are equations that show either the oxidation or reduction process separately. They are useful for balancing redox reactions and understanding the electron transfer involved. In the context of the given question, analyzing the half-reaction allows us to determine whether the species is gaining or losing electrons, thus classifying it as oxidation or reduction.
Recommended video:
Guided course
01:49
First-Order Half-Life
Related Practice
Textbook Question
Assume that an aqueous solution of OH-, represented as a blue sphere, is allowed to mix with a solution of an acid HnA, represented as a red sphere. Three possible outcomes are depicted by boxes (1)–(3), where the green spheres represent An-, the anion of the acid: Which outcome corresponds to each of the following reactions? (a) (b) (c)
1
views
Textbook Question
The concentration of an aqueous solution of NaOCl (sodium hypochlorite; the active ingredient in household bleach) can be determined by a redox titration with iodide ion in acidic solution:

Assume that the blue spheres in the buret represent I-ions, the red spheres in the flask represent OCl-ions, the con-centration of the I-ions in the buret is 0.120 M, and the volumes in the buret and the flask are identical. What is the concentration of NaOCl in the flask? What percentage of the I-solution in the buret must be added to the flask to react with all the OCl-ions?

Textbook Question

Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (a) HClO(aq) → Cl2(g)

Textbook Question

The following two redox reactions occur between aqueous cations and solid metals. Will a solution of green cations react with solid blue metal? Explain.

(a)

(b)

Textbook Question

Based on the positions in the periodic table, which of the following reactions would you expect to occur? (a) Red+ + Green → Red + Green+ (b) Blue + Green+ → Blue+ + Green (c) Red + Blue+ → Red+ + Blue

Textbook Question

Assume that the electrical conductivity of a solution depends on the total concentration of dissolved ions and that you measure the conductivity of three different solutions while carrying out titration procedures: (a) Begin with 1.00 L of 0.100 M KCl, and titrate by adding 0.100 M AgNO3. (b) Begin with 1.00 L of 0.100 M HF, and titrate by adding 0.100 M KOH. (c) Begin with 1.00 L of 0.100 M BaCl2, and titrate by adding 0.100 M Na2SO4. Which of the following graphs corresponds to which titration?