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YEAR 11 Chemistry Topic Test Assessment
2006 20%
Name: __________________
1. Briefly describe an experiment you carried out to separate a dissolved solid from its solution.
4 marks
Name the: solution: _______________ solute:______________ solvent: _________________
Aim:_______________________________________________________________________
Method: ____________________________________________________________________
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____________________________________________________________________________Diagram (labeled):
2.Water of crystallization in a compound can be removed by heating the compound in a
crucible. Determine the percentage of water of crystallization in a compound using the
following experimental results: Mass of empty crucible: 23.64g; mass of crucible plus
compound: 27.72g; mass of crucible plus compound after heating: 26.56g. 2 marks
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3.a) Explain the difference between boiling and electrolysis of water in terms of chemical and
physical change. 1 mark
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b) Describe the process of electrolysis as evidence that water is a compound. 2 marks
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4.Place the following elements in a table to show whether they belong to metals, non-metals
and semi-metals: selenium, zirconium, osmium, germanium, rubidium, xenon and
antinomy.
3 marks
5.Complete the table: 3 marks
Name Formula Metallic, Ionic or
Covalent
Solid, Liquid or
Gas
Sodium Fluoride
CH4
Sulpher Trioxide
CaCO3
Iron (III) hydroxide
Hg
6.Draw Lewis electron dot diagrams to show the bonding structure in: 3marksa) water, H2O b) oxygen, O2 c) ethane, C2H6
7.Show the formation of ions in terms of gaining or losing electrons (use half equations) by
the following substances: 2 marks
a) Ca ________________________________________________b) F ________________________________________________
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8.The table below gives the melting points of the chlorides of seven consecutive elements A to G in
aperiod of the Periodic Table.Element A B C D E F G
Melting point of chloride (C) 801 712 193 -68 -91 -80 -101
(a) Give one element, A to G, which could be a metal._________________________ 1 mark
(b) Name the type of banding which would exist in the chlorides of elements A and B. 1 mark
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(c) Explain, in terms of the bonding, the low melting points of the chlorides of elements D to G.
1 mark
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9.2.1 g solid calcium metal reacts with excess dilute hydrochloric acid to give calcium chloridesolution and hydrogen gas.
(a) Write down the ionic equation for the reaction. 1 mark
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(b) Calculate the moles of calcium used. 1 mark
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(c) How many moles of hydrogen gas were produced? 1 mark
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(d) Determine the volume of this hydrogen gas at 25C 1 mark
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10.A molecule of a certain gaseous oxide of nitrogen can be represented by the formula NxOy.
In a series of experiments, various volumes of NxOy gas were decomposed into nitrogen gas (N2)
and oxygen gas (O2). The table shows the results of the experiments. All volumes were measured atthe same temperature and pressure.
ExperimentVolume of NxOv gas
decomposed (L)
Volume of nitrogen
gas produced (L)
Volume of oxygen gas
produced (L)
1 6.0 6.0 3.0
2 1.0 1.0 0.50
3 0.40 0.40 0.20
(a) Show how these results agree with Gay-Lussac's Law. 2 mark
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(b) Use the results from any one of the three experiments to determine the molecular formula of
this oxide of nitrogen. Show your reasoning. 2 marks.
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11.Methane burns according to the following reaction:
( ) ( ) ( ) ( )g2224 OH2COO2CH ++ ggg
(a) Determine the volume of 32.0 g methane at 25 C and 100kPa 1 marks
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(b) If 32.0 g methane and 2.0 moles oxygen are reacted, not all of the gases are used up.
Determine which one will be left over, and the mass of carbon dioxide produced. 4 marks
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12.Identify why there are more metals available for people to use now than there were 200 years
ago. 2 marks
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13.Explain why ores are non-renewable resources. 2marks
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1. Solution: Salt Water
Solute: Salt
Solvent: Water
Aim: To separate salt from salt water.
Method: Heat the salt water until all the water has evaporated leaving behind only
the salt.Diagram:
2. 28.43%
7. a) + + 22 CaeCa
b) + FeF
8. a) A b) Ionic
9.a) 222 HCaHCa ++ ++
b) 0.052 moles
c) 0.052 moles
d) 1.300L11.a) 49.45L