What is oxidation?
The loss of electrons
An increase in oxidation number
What is reduction?
The gain of electrons
A decrease in oxidation number
What is the oxidising agent?
They take an electron from the species being oxidised, therefore being reduced
What is the reducing agent?
Gives electrons to the species that is being reduced, therefore being oxidised
What is a half equation?
Shows oxidation or reduction
It will have electrons on the RHS for oxidation and electrons on the LHS for reduction
What is a voltaic cell?
Arranges for the two half equations to occur in different half-cells
The electrons are transferred from one half-cell to the other (generates the current)
What does a half-cell contain?
The chemical species that are present in the redox half equations
What does a Voltmeter measure?
The difference in potential difference between the two electrodes
What is the purpose of the salt bridge?
Allows for the ions to flow
What does having a more negative electrode potential mean?
There is a greater tendency for the electrons to flow
What is the standard electrode potential?
A half-cell connected to a standard hydrogen half-cell, under standard conditions.
What does the value of Electrode potential tell us?
The more negative the electrode potential, the higher the tendency for electrons to flow.
The more positive the electrode potential, the lower the tendency for electrons to flow.
What are the limitations to using the Electrode potential values?
The predictions indicate the thermodynamic feasibility, but give no indication of the rate.
The values apply to only aqueous reactions, other conditions may not be standard.
The reaction concentrations may not be standard, which affects the position of the redox system compared to the other redox system.
What is a storage cell?
Based on the voltaic cells
Can be non-rechargeable or rechargeable
What is a primary cell?
Non-rechargeable cells
The reaction cannot be reversed
What is a secondary cell?
Rechargeable cell
The cell reaction is reversable
What is a fuel cell?
Use the energy from the reaction of a fuel with oxygen to create a voltage.
Fuel and oxygen flow into the cell, the products flow out.
The can operate continuously.
What are the two types of fuel cells?
Alkali and Acid hydrogen fuel cells
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chapter 29
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chapter 519
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chapter 618
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chapter 716
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chapter 86
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chapter 920
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chapter 1010
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key definitions for organic chemistry15
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naming alkanes9
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isomerism6
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chapter 1217
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chapter 1318
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alcohols14
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chapter 1515
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acids and redox8
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practical techniques in organic chemistry2
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recycling polymers7
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mass spectroscopy4
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infrared spectroscopy6
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preparing a standard solution11
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chapter 1811
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chapter 1917
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Chapter 2634
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chapter 2231
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Chapter 2034
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Chapter 2113
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Chapter 2318
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Chapter 2437
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Chapter 2723
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Chapter 2518
