DSE Chem revision
Topic 7. Redox reactions, Chemical cells and Electrolysis
A. Redox reactions
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oxidation and reduction
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oxidation numbers
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Common oxidising agents:
MnO4-(aq)/H+(aq),
Cr2O72-(aq)/H+(aq),
Fe3+(aq),
Cl2(aq),
HNO3(aq) of different concentrations
conc. H2SO4(l)) -
Common reducing agents
SO32-(aq),
I-(aq),
Fe2+(aq),
reactive metals (e.g. Na(s), Mg(s), Zn(s)) -
balancing equations for redox reactions
B. Chemical cells in daily life
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primary cells and secondary cells
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uses of chemical cells in relation to their characteristics such as size, voltage, capacity, rechargeability and price
C. Simple chemical cells
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Chemical cells consisting of:
1. two metal electrodes and an electrolyte
2. metal-metal ion half cells and salt bridge
3. metal-metal ion half cells and porous device -
changes occurring at the electrodes and electron flow in the external circuit
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half equations and overall cell equations
D. Redox reactions in chemical cells
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zinc-carbon cell
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chemical cells with inert electrodes
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hydrogen-oxygen fuel cell
E. Electrolysis
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Electrolytic cell
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Electrolysis of dilute sulphuric acid
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Electrolysis of sodium chloride solutions of different concentrations
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Electrolysis of copper(II) sulphate solution
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anodic and cathodic reactions
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preferential discharge of ions in relation to the electrochemical series, concentration of ions and nature of electrodes
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industrial applications of electrolysis in electroplating
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