Oxidation–Reduction—Review Demonstration Kit for AP® Chemistry

Name: Oxidation–Reduction—Review Demonstration Kit for AP® Chemistry
Brand: By: The Flinn Staff
SKU: AP7436
Price: 79.75 USD
Availability: InStock

By: The Flinn Staff

Item #: AP7436

Price: $79.75

This item’s arrival date is greater than 60 days. Please call us at 800-452-1261 for more information

Use the Oxidation–Reduction Review Demonstration Kit for AP^® Chemistry to help students review principles of oxidation–reduction. Students review oxidation states, oxidizing and reducing agents and half-reactions by way of demonstrations.

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AP Chemistry Review Demonstration Kits

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Use this set of integrated, interactive demonstrations to help students review the major principles of oxidation–reduction. Set of two demonstrations includes:

Reactions of Iron(II) and Iron(III) Ions Investigate electron transfer reactions of Fe²⁺ and Fe³⁺ ions with a series of oxidizing and reducing agents, respectively. Students identify trends in the reduction of iron(III) ions as they review essential knowledge and skills, such as how to assign oxidation states and balance half-reactions, for the AP^® Chemistry Exam.
Colorful Oxidation States of Manganese—Demonstrate the wide range of colorful oxidation states of manganese, a continuous series from +7 to +2! Students observe and compare the sequence of projected colors arising from oxidation of manganese in its +2 form and corresponding reduction of its highest, +7 oxidation state. Excellent review of balancing redox equations!

Includes valuable Teacher Notes with helpful teaching tips, reproducible student worksheets, and enough materials to perform each demonstration twice.

Concepts: Oxidation–reduction, oxidation states, oxidizing and reducing agents, half-reactions.
Time Required: One class period

Specifications

Materials Included in Kit:
Hydrochloric acid solution, 3 M, 25 mL
Hydrogen peroxide, McKesson^©, 3%, 4 oz
Iron(III) chloride solution, 0.1 M, 125 mL
Iron(II) Ammonium sulfate, 4 g
Manganese sulfate solution, 0.12 M, 35 mL
Potassium ferricyanide solution, 0.1 M, 10 mL
Potassium permanganate solution, 0.006 M, 35 mL
Potassium permanganate solution, 0.025 M, 30 mL
Potassium thiocyanate solution, 0.1 M, 10 mL
Sodium bromide solution, 0.2 M, 30 mL
Sodium hydroxide solution, 50%, 15 mL
Sodium hydroxide solution, 6 M, 15 mL
Sodium hypochlorite solution, 30 mL
Sodium iodide solution, 0.2 M, 30 mL
Sodium sulfite, 25 g
Sulfuric acid solution, 6 M, 15 mL
Pipet, Beral-type, graduated, 20
Reaction plate, 6 well, 2
Toothpicks, wooden, flat, 750

Correlation to Next Generation Science Standards (NGSS)^†

Science & Engineering Practices

Asking questions and defining problems
Developing and using models
Planning and carrying out investigations
Analyzing and interpreting data
Using mathematics and computational thinking
Constructing explanations and designing solutions
Engaging in argument from evidence

Disciplinary Core Ideas

HS-PS1.A: Structure and Properties of Matter
HS-PS1.B: Chemical Reactions
HS-PS3.B: Conservation of Energy and Energy Transfer
HS-PS3.D: Energy in Chemical Processes

Crosscutting Concepts

Patterns
Cause and effect
Systems and system models
Energy and matter
Structure and function
Stability and change

Performance Expectations

HS-PS1-1. Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.
HS-PS1-2. Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.
HS-PS1-7. Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction.
HS-PS3-1. Create a computational model to calculate the change in the energy of one component in a system when the change in energy of the other component(s) and energy flows in and out of the system are known.