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Questions and Answers
What does an oxidising agent do in a redox reaction?
What does an oxidising agent do in a redox reaction?
Why do half equations need to be balanced in a redox reaction?
Why do half equations need to be balanced in a redox reaction?
Which step is used to balance hydrogen in a half equation?
Which step is used to balance hydrogen in a half equation?
What happens to the oxidation number of a reducing agent in a redox reaction?
What happens to the oxidation number of a reducing agent in a redox reaction?
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How are half equations combined to determine the overall redox reaction?
How are half equations combined to determine the overall redox reaction?
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Why does an oxidising agent gain electrons in a redox reaction?
Why does an oxidising agent gain electrons in a redox reaction?
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Which of the following defines oxidation?
Which of the following defines oxidation?
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What is the oxidation state of hydrogen?
What is the oxidation state of hydrogen?
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In a charged compound, the oxidation states of the elements add up to what?
In a charged compound, the oxidation states of the elements add up to what?
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What does the acronym OILRIG stand for in relation to redox reactions?
What does the acronym OILRIG stand for in relation to redox reactions?
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What is the oxidation state of oxygen?
What is the oxidation state of oxygen?
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Which group of elements have an oxidation state of +1?
Which group of elements have an oxidation state of +1?
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Study Notes
Oxidation, Reduction, and Redox Reactions
- Oxidation is the loss of electrons, while reduction is the gain of electrons.
- Oxidation and reduction occur simultaneously in a reaction, making them redox reactions.
- The acronym OILRIG helps remember that oxidation is loss and reduction is gain.
Oxidation Number
- Oxidation number gives the oxidation state of an element or ionic substance.
- Rules for allocating oxidation states:
- Oxidation state of an element is zero.
- Oxidation states in a neutral compound add up to zero.
- Oxidation states in a charged compound add up to the total charge.
- Hydrogen has an oxidation state of +1.
- Oxygen has an oxidation state of -2.
- All halogens have an oxidation state of -1.
- Group I metals have an oxidation state of +1.
Oxidising and Reducing Agents
- An oxidising agent accepts electrons from the species being oxidised, gaining electrons and being reduced.
- A reducing agent donates electrons to the species being reduced, losing electrons and being oxidised.
Half Equations
- Half equations show separate oxidation and reduction reactions in a redox reaction.
- Half equations must be balanced in terms of species and charges.
- A useful method for writing half equations:
- Balance all species excluding oxygen and hydrogen.
- Balance oxygen using H2O.
- Balance hydrogen using H+ ions.
- Balance changes using e- (electrons).
- Half equations can be combined to determine the overall redox reaction, ensuring the number of electrons is the same for both half equations.
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Description
This quiz provides detailed notes on oxidation, reduction, and redox reactions in AQA Chemistry A-level 3.1.7. It covers concepts such as the definitions of oxidation and reduction, electron transfer, and the occurrence of oxidation and reduction simultaneously in reactions.