1. Write the chemical formula of each of the following ionic compounds:
[10 ]
a) Iron (III) sulphide
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b) Calcium hydroxide
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c) Sodium sulphate
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d) Ammonium phosphate _______________________________________________
e) Silver oxide
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f) Zinc nitrate
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g) Potassium managanate (VII) __________________________________________
h) Copper (II) carbonate ________________________________________________
2. Write name for each of the following ionic compounds:
[10]
a) Mg3(PO4)2 _________________________________________________________
b) AgCl
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c) ZnI2
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d) Al(HCO3)3 __________________________________________________________
e) FeBr3 ____________________________________________________________
f) FeSO4 ____________________________________________________________
g) Cu2O ____________________________________________________________
h) Pb(NO3)2 __________________________________________________________
3. Classify the reactions as synthesis, decomposition, single displacement or double
displacement (ionic precipitation).
[4]
a) FeSO4(aq) + 2NaOH(aq)  Fe (OH)2(s) + Na2SO4(aq)
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b) F2(g) + 2NaCl(aq)  NaF(aq) + Cl2(g)
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c) 2Na(s) + Cl2(g)  2NaCl(s)
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d) Pb(NO3)2(s)  2PbO (s) + 4NO2(g) + O2(g)
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4. Balance the following equations by putting the proper coefficients where they are
needed.
[6]
a) ___C4H10 + ___O2 ___CO2 + ___H2O
b) ___FeS +___ O2 ___Fe2O3 + ___SO2
c) ___Mg(NO3)2 ___MgO+___ NO2+ ___O2
d) ___Fe + ___Cl2___ FeCl3
e) ___NaOH +___ H2SO4  ___Na2SO4 +___ H2O
f) ___Fe + ___O2  ___Fe2O3
5. Write a balanced chemical equation for EACH of following reactions:
a) The reaction between calcium and hydrochloric acid (HCl) aqueous to form
calcium chloride and hydrogen.
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[2]
b) Zinc hydrogen carbonate reacting with nitric acid (HNO3) to form zinc nitrate,
carbon dioxide and water
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[2]
c) The reaction between aluminium and chlorine gas to make aluminium chloride.
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[2]
d) The reaction occurring when chlorine gas is bubbled into aqueous potassium
iodide, which forms potassium chloride and iodine.
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[2]
e) The formation of copper (II) oxide, nitrogen dioxide and oxygen when copper (II)
nitrate is heated.
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[2]
2
6. Write the ionic equation for each of the following reactions:
a) Pb(NO3)2(aq) + 2NaCl(aq) PbCl2(s) + 2NaNO3(aq)
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[2]
b) KOH(aq) + HNO3(aq) KNO3(aq) + H2O(l)
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[2]
c) Mg (s) + 2HCl(aq) MgCl2(aq) + H2(aq)
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[2]
d) Aqueous aluminium nitrate reacting with aqueous sodium hydroxide to form
insoluble aluminium hydroxide and soluble sodium nitrate.(include state
symbols)
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[3]
e) The reaction between lead (II) nitrate solution and sodium chloride solution to
form insoluble lead (II) chloride and sodium nitrate solution. (include state
symbols)
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[3]
3
7. State whether EACH of the following ionic compound is soluble or insoluble in water:
Compound
Silver nitrate
Soluble /Insoluble
Potassium phosphate
Zinc hydroxide
aluminium sulphate
Lead(II) chloride
Copper (II) oxide
Calcium carbonate
Sodium ethanoate
[8]
Total 60 marks
4