Structure And Bonding Chart Page 3
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4[HT] Recall the unit of concentrations of solutions
[HT] Recall that equal volumes of gases at the same temperature and
pressure have the same number of molecules
C2.5 Exothermic/Endothermic Reactions
Can you…?
State that when chemical reactions occur, energy is transferred to or from the
surroundings.
State what an exothermic reaction is in terms of energy and give examples.
Define an endothermic reaction in terms of energy and give examples.
Recall that if a reversible reaction is exothermic in one direction, it is
endothermic in the opposite direction.
C2.6 Acids, Bases and Salts
Can you…?
Use the state symbols in equations - (s), (l), (g) and (aq).
Describe how soluble salts can be made by reacting acids with metals,
insoluble bases and alkalis
Describe how salt solutions can be crystallised to produce solid salts.
Insoluble salts can be made by mixing certain salts in solution (precipitate
formed)
Describe how precipitation can be used to remove unwanted ions from
solutions, e.g. in treating water for drinking.
Describe the difference between a base (metal oxides) and an alkali (metal
hydroxides)
Name the salts that HCl, HNO
, H
SO
produce
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State that ammonia dissolves in water to produce an alkaline solution. It is
used to produce ammonium salts, which are important as fertilisers.
Recall that the pH scale is a measure of the acidity or alkalinity of a
solution.
Describe an acid as releasing H+ ions in solution.
Describe an alkali as releasing OH- ions in solution.
In neutralisation reactions, hydrogen ions react with hydroxide ions to
produce water. Represent this reaction with the equation:
H+(aq) + OH–(aq) ➞ H2O(l)
C2.7 Electrolysis
Can you…?
Describe what electrolysis is and what it does.
State the type of compound that can be used as an electrolyte
Explain why the electrolyte must been molten or in solution for
electrolysis to work
Describe which ions move to which electrode.
Explain what then happens to ions at that electrode, in terms of electrons.
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