Textbook Question
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (a) HClO(aq) → Cl2(g)
Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 44
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
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Identify the elements involved in each reaction and their positions in the periodic table.
Determine the relative reactivity of the elements based on their positions. Elements on the left side of the periodic table are generally more reactive than those on the right.
Consider the concept of oxidation and reduction. In a redox reaction, the more reactive element will tend to lose electrons (oxidize), while the less reactive element will gain electrons (reduce).
Analyze each reaction: (a) Check if Red is more reactive than Green. If so, Red will not oxidize, and the reaction is unlikely. (b) Check if Blue is more reactive than Green. If so, Blue will oxidize, and the reaction is likely. (c) Check if Red is more reactive than Blue. If so, Red will oxidize, and the reaction is likely.
Conclude which reactions are expected to occur based on the reactivity series and the positions of the elements in the periodic table.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Periodic Table Trends
The periodic table organizes elements based on their atomic number and properties. Elements in the same group often exhibit similar chemical behaviors, while trends such as electronegativity, ionization energy, and atomic radius influence how elements interact in reactions. Understanding these trends helps predict the likelihood of reactions occurring between different elements.
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Periodic Trends
Oxidation and Reduction
Oxidation and reduction (redox) reactions involve the transfer of electrons between species. In these reactions, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. Identifying which species is oxidized and which is reduced is crucial for predicting the outcome of a reaction, especially when dealing with ions and their charges.
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Ionic and Covalent Compounds
Ionic compounds are formed through the transfer of electrons from one atom to another, resulting in charged ions that attract each other. In contrast, covalent compounds involve the sharing of electrons between atoms. Recognizing whether the reactants are ionic or covalent helps in understanding their reactivity and the types of products that can form during a chemical reaction.
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Related Practice
Textbook Question
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (d) SbCl4-(aq) → SbCl6-(aq)
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?
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
How many moles of solute are present in each of the following solutions? (a) 35.0 mL of 1.200 M HNO3
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Textbook Question
How many moles of solute are present in each of the following solutions? (b) 175 mL of 0.67 M glucose (C6H12O6)
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