Pre-course task for 2015 entry.
AS Chemistry
Why do I need to complete a pre-course task?
The task serves two purposes. Firstly, it allows you to carry out a little bit of preparation before
starting your studies in September. Secondly, the task is designed to allow the college to
assess important skills at the start of the course, which they can use for planning student
activities, identifying where support might be needed and to help in the assessment of your
suitability for the AS level course.
We have found that some students elect to take an AS level without recognising the skills
needed to receive a high grade in an examined course; such students may be better suited to a
vocational qualification, which is only assessed by coursework. Your performance in the task
will allow your teachers to support you fully to ensure you are on the right course to maximise
your performance.
When should I hand it in?
You should have completed this task by the first lesson in September. You should hand it in to
your subject teacher on that day.
How will I be given feedback on how well I have done?
Feedback will be given in written and verbal form and will outline your strengths and areas for
development. This work comprises an element of the assessment used during induction.
Task In Detail
You should complete questions 1-12 fully. A periodic table and a table of common ions has
been provided.
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
Course: AS Chemistry
Student name:
Date submitted:
1. Complete the following table. The first few have been done for you
element
symbol
atomic
number
hydrogen
H
1
helium
He
lithium
Li
mass
number
1
number
of
protons
1
number
of
neutrons
0
number
electron
of
arrangement
electrons
1
1
2
4
2
2
2
2
3
7
3
4
3
2,1
beryllium
4
9
boron
5
11
carbon
6
12
nitrogen
7
14
oxygen
8
16
fluorine
9
19
neon
10
20
sodium
11
23
magnesium
12
24
aluminium
13
27
silicon
14
28
phosphorus
15
31
sulphur
16
32
chlorine
17
35
argon
18
40
potassium
19
39
calcium
20
40
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
2. Neatly draw diagrams to show the electron arrangement of an atom for the
following elements.
a. nitrogen
b. carbon
c. potassium
d. phosphorus
e. argon
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
3. Ionic bonding.
Draw a dot and cross diagram that shows the ionic bonding in the following
compounds.
Lithium Fluoride (LiF)
Calcium Fluoride (CaF2)
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
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Aluminium Oxide (Al2O3)
4. Using the Periodic Table, write the symbol for the ion formed (including its charge)
from each of the following elements:
element
symbol of ion
formed
element
lithium
fluorine
rubidium
iodine
calcium
astatine
strontium
selenium
gallium
phosphorus
symbol of ion
formed
5. Fill in the table to show the electron arrangements for the following ions:
ion
electron
arrangement
ion
K+
F-
S2-
Mg2+
Al3+
N3-
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
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electron
arrangement
6. Formulae: Using the table of common ions provided complete the following table by
writing in the symbols for all the ions, positive (cations) and negative (anions), which
are part of the named compounds. Hence work out the formulae of the compounds.
You are permitted to use a Periodic Table.
Name of Compound
Symbol for
Symbol for
Formula of
positive ion
negative ion
Compound
(cation)
(anion)
potassium iodide
rubidium oxide
sodium nitride
beryllium fluoride
magnesium oxide
aluminium oxide
sodium nitrate
magnesium hydroxide
magnesium nitrate
calcium phosphate
ammonium sulphate
copper(II) carbonate
iron(II) sulphate
sodium hydrogencarbonate
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
Covalent bonding and properties of covalent compounds
7. Draw ‘dot and cross’ diagrams showing all the electrons in the following molecules:
Fluorine (F2)
Hydrogen sulphide (H2S)
Carbon dioxide (CO2)
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
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Phosphine (PH3)
Nitrogen (N2)
8. Balancing Equations.
Balance the following equations:
C2H6(g) +
O2 (g) →
Fe(s) +
Na(s) +
KI(aq) +
CaCO3(s) +
O2(g) →
H2O(l) →
→
→
PbI2(s) +
CaCl2(aq)
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
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H2O(l)
Fe2O3(s)
NaOH(aq) +
Pb(NO3)2(aq)
HCl(aq)
CO2 (g) +
+
H2(g)
KNO3(aq)
CO2(g)
+
H2O(l)
Question 9, 10, and 11 involve chemical calculations
9. Rubidium forms an ionic compound with silver and iodine. This compound has a
potential use in miniaturised batteries because of its high electrical
conductivity.
The empirical formula of this ionic compound can be calculated from its
percentage composition by mass: Rb, 7.42%; Ag, 37.48%; I, 55.10%.
(i)
Define the term empirical formula.
.........................................................................................................................
.........................................................................................................................
.........................................................................................................................
(ii)
Calculate the empirical formula of the compound showing your working
clearly.
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
10. Barium metal can be extracted from barium oxide, BaO, by reduction with
aluminium.
6BaO + 2Al
3Ba + Ba3Al2O6
Calculate the mass of barium metal that could be produced from reduction of
500 g of barium oxide using this method.
Answer = ............................... g
11.
(a) Balance the following equation.
CaCO3 +
HNO3

Ca(NO3)2
+
CO2
+
H2O
(b) What mass of calcium nitrate would be obtained from 40grams of calcium
carbonate in the above reaction.
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
12. Giant Covalent Structures formed by carbon atoms. (Fill in the blanks and answer
the questions.)
Diamond
In the structure each carbon is joined to _________
other carbon atoms by ___________________ bonds
consisting of _____________________ electrons.
The arrangement around each carbon is
__________________________and the
angles are all _______ degrees.
http://www.hull.ac.uk/chemistry/intro_inorganic/Diamond.htm
Explain why diamond has a high melting temperature
Explain why diamond does not conduct electricity
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
C-C-C bond
Graphite
http://facweb.bhc.edu/academics/science/harwoodr/GEOL101/study/minerals.htm
Each carbon atom is bonded to __________________ other carbon atoms by
_______________ bonds, forming hexagonal rings. The fourth outer electron of each
carbon atom is delocalised between the sheets of hexagons. The interactions between the
layers of hexagons are _________________ so the layers can slip over each other.
Explain why graphite has a high melting temperature
Explain why graphite conducts electricity
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
www.huddnewcoll.ac.uk
Table of common ions
+1
+2
+3
-3
-2
-1
lithium
Li+
beryllium
Be2+
aluminium
Al3+
nitride
N3-
oxide
O2-
fluoride
F-
sodium
Na+
magnesium
Mg2+
iron(III)
Fe3+
phosphide
P3-
sulphide
S2-
chloride
Cl-
potassium
K+
calcium
Ca2+
phosphate
PO43-
carbonate
CO32-
bromide
Br-
rubidium
Rb+
strontium
Sr2+
sulphate
SO42-
iodide
I-
caesium
Cs+
barium
Ba2+
hydroxide
OH-
silver
Ag+
iron(II)
Fe2+
nitrate
NO3-
copper(I)
Cu+
zinc
Zn2+
hydrogencarbonate HCO3-
hydrogen
H+
Copper(II)
Cu2+
hydrogensulphate
ammonium
NH4+
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
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HSO4-
Huddersfield New College, New Hey Road, Huddersfield, HD3 4GL
Telephone: 01484 652341 email: info@huddnewcoll.ac.uk
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