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Chapter 6: Electrochemistry
Transcript of Chapter 6: Electrochemistry
cannot conduct electricity in any state. Chemical compound that can conduct electricity
in the molten state or aqueos state and
undergo chemical changes. A simple electrolytic cell Examples: Ionic substances
Dilute acid solution
Dilute alkaline solution
Aqueous salt solution Examples: Covalent substances
Hydrogen chloride in organic solvents is an electrolyte because it is in MOLTEN state & can conduct electricity. Chemical Substances (tetrachloromethane) Light bulb does not light up.
There is no conductivity of electricity.
The solution exist as a covalent compound.
So the solution is a non-electrolyte. Electrolyte
In solid state DO NOT conduct electricity WHY? Because the ions are
held in a fixed crystal lattice They are held with the strong
electrostatic forces of attraction The ions do not freely move It contains Electrolyte in
molten & aqueous state can conduct electricity This is because of the presence of
moving ions in both state. The freely moving ions
(cations & anions) allow
the conductivity of electricity. Electrolysis introduction Electrodes (Cathode) (Anode) (Anion) (Cation) - attracts positively charged ions - attracts negatively charged ions Electrolytes & non electrolytes Classify the following chemicals into electrolytes
or non electrolytes: Potassium chloride, KCl solution
Molten lead(ii) bromide, PbBr2
Molten zinc oxide, ZnO
Sodium chloride, NaCl solution
Ammonia in tetrachloromethane Hit it!