Questions and Answers
Reduction-Oxidation reactions (REDOX reactions) involve the gain and loss of electrons.
True
What method do we use to balance REDOX reactions?
half-reactions method
What happens during oxidation?
What happens during reduction?
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In the same reaction K (s) + Br2 (l) → KBr (aq), what species is reduced?
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The oxidation half-reaction for K is K0 → K+ + ______
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In the reaction K (s) + Br2 (l) → KBr (aq), what species is oxidized?
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The reduction half-reaction for Br2 is Br20 + ______ → 2Br¯
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What is the balanced overall reaction for 2K (s) + Br2 (l)?
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Are Au3+ + I¯ → Au + I2 a REDOX reaction?
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Are Cu + Ag+ → Cu2+ + Ag a REDOX reaction?
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Is BaSO3 → BaO + SO2 a REDOX reaction?
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In an acidic solution, which species in the reaction ClO3¯ + I2 → IO3¯ + Cl¯ is being oxidized?
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In the same reaction ClO3¯ + I2 → IO3¯ + Cl¯, which species is being reduced?
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Study Notes
REDOX Reactions Overview
- REDOX reactions involve the transfer of electrons between species, where one species is oxidized (loses electrons) and another is reduced (gains electrons).
- Charge conservation is maintained through simultaneous oxidation and reduction.
- Assigning oxidation numbers is crucial for identifying oxidized and reduced species.
Key Definitions
- Oxidation: Loss of electrons, increasing positive charge.
- Reduction: Gain of electrons, increasing negative charge.
Balancing REDOX Reactions
- Use the half-reactions method for balancing.
- Identify oxidation and reduction half-reactions separately.
Example Problem: Balancing K + Br2 → KBr
- Assign oxidation numbers:
- K: 0 (elemental state) to +1 (in KBr).
- Br2: 0 to -1 (in KBr).
- Oxidation half-reaction: K → K⁺ + e⁻
- Reduction half-reaction: Br2 + 2e⁻ → 2Br⁻
- Balance charges by adding electrons to the appropriate sides:
- Oxidation: K → K⁺ + e⁻
- Reduction: Br2 + 2e⁻ → 2Br⁻
- Multiply the oxidation half-reaction by 2 to equalize electrons:
- 2K → 2K⁺ + 2e⁻
- Combine half-reactions, cancelling out electrons:
- 2K + Br2 → 2K⁺ + 2Br⁻
- Balanced equation: 2K (s) + Br2 (l) → 2KBr (aq)
Practice REDOX Reactions
- Confirm if a reaction is a REDOX reaction and balance it using the half-reaction method:
- Au³⁺ + I⁻ → Au + I2
- Cu + Ag⁺ → Cu²⁺ + Ag
- BaSO3 → BaO + SO2
Complex REDOX Reactions
- In aqueous solutions, especially in acidic or basic conditions, protons (H⁺) and hydroxides (OH⁻) play a significant role in balancing charges and species in half-reactions.
- Example in acidic solution:
- ClO3⁻ + I2 → IO3⁻ + Cl⁻
- Assign oxidation numbers to ascertain which species are oxidized and reduced before balancing.
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Description
Test your knowledge on balancing REDOX reactions in chemistry. This quiz covers the principles of oxidation and reduction, including how to assign oxidation numbers to reactants and products. Gain a deeper understanding of these essential chemical processes through practice questions.
