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Questions and Answers
What occurs at the cathode during electrolysis?
What occurs at the cathode during electrolysis?
Why must the ionic compound be molten or dissolved for electrolysis to occur?
Why must the ionic compound be molten or dissolved for electrolysis to occur?
In the half equation 2Cl- → Cl₂ + 2e-, what type of reaction is taking place?
In the half equation 2Cl- → Cl₂ + 2e-, what type of reaction is taking place?
Which half equation demonstrates a reduction reaction?
Which half equation demonstrates a reduction reaction?
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Study Notes
Electrolysis
- Electrolysis is the process of using electricity to break down ionic compounds.
- Positive ions (cations) are attracted to the negative electrode (cathode).
- Negative ions (anions) are attracted to the positive electrode (anode).
- At the electrodes, ions gain or lose electrons to become neutral atoms, a process called discharge.
- The compound to be electrolyzed must be in a molten or dissolved state, allowing ions to move freely.
Half Equations
- Half equations represent the chemical reactions occurring at each electrode.
- Reduction half equations show the gain of electrons by cations.
- Examples of reduction half equations include:
- Mg+2 + 2e- → Mg
- Na+ + e- → Na
- Al+3 + 3e- →Al
- 2H- + 2e- → H2
- Oxidation half equations show the loss of electrons by anions.
- Examples of oxidation half equations include:
- 2Cl- →Cl₂ + 2e-
- 2Br- →Br2 + 2e-
- 2I- →I2 + 2e-
- 4 0H- → 2H20+ 02 + 4e-
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Description
Test your knowledge on the process of electrolysis, including ion movement, electrode reactions, and half equations. Understand how cations and anions interact at the cathode and anode. This quiz will challenge your grasp of these fundamental concepts in chemistry.
