HAVANT SIXTH FORM
COLLEGE
2015
CHEMISTRY
GETTING AHEAD
MAKING THE JUMP FROM
GCSE TO A-LEVEL
Introduction
Welcome to Chemistry at Havant Sixth Form College. Many students often regard Chemistry as a difficult
subject. Here at Havant we believe that Chemistry is a logical and perfectly learnable subject but it does
require a lot of consistent hard work. However, most of our students agree that when they put in the
required effort they achieve matching grades in Chemistry. Last year 96% of our students passed their
second year and 43% of them achieved an A or B grade.
To gauge the workload and difficulty of the subject we suggest that you read the answers to our course
survey and listen to the advice from previous students (look for advice snippets on the noticeboards during
induction and the full answers in your classroom).
What to do with this Pack?
Read the advice on the following pages. Print out and do the first round of Test questions under exam
conditions (no textbook or any kind of help, no distractions, timed). Mark your answers. Assess your
strengths and weaknesses. Follow the flow-chart below.
We do recommend that regardless how you have done you do look at the links.
Make sure you bring your printed, marked set of questions with you to the first lesson. Indicate the time it
took you to do them.
What makes a good Chemistry Student?
Getting good grades in Chemistry requires perfect attendance and that you apply yourself in lessons;
perform well in assignments during the 2 years and exams. Everything that you learned about performing
well in athletics or music applies to having a good performance in Chemistry. As in music or athletics, you
must practice regularly and develop a lifestyle that does not get in the way of your performance. Here are
a few examples of how to obtain better performance skills in your courses. Remember that each person
learns a little differently. What works for others may not necessarily work for you. You need to find out
how to maximize your performance. The tips below should help most students.

Make good notes
Take brief notes in class but get in the habit of making thorough notes from the rough notes you have
taken in class, the textbook and our online resources. Make sure you keep these notes organised. If you do
this as you go along you will learn the material more thoroughly and revision will be easier.

Practice daily.
A top footballer doesn’t get good at football by practising football once a week, you need to be looking
through some of the material every day.

Do your best work.
Have you ever heard the expression "how you practice is how you will play the game"? Just as sloppy play
will often lose the game, and sloppy playing will ruin the best piece of music, sloppy work habits will ruin a
good academic performance. The only way to avoid a sloppy performance is to practice not being sloppy.
When working a problem, neatly and clearly write out your answer. Be sure your drawings and figures are
clear and labelled.

Learn the material in small chunks.
There may seem to be an overwhelming amount of material to learn. Instead of going over all the material
many times, break the material into little pieces that you can concentrate on until you master them. You
may feel like you are spending a lot of time on learning a small amount, but if the material is really learned
you will know it the next time you see it, and then, more can be added to it.

Take an active part in class.
Each lesson we will be covering something new. This means that not paying attention for just one class or
missing lessons will result in you falling behind. Miss too many and catching up will be nearly impossible.
Don’t take our word for it, see on the notice board what last year AS students had to say about it!

Use Moodle
We are very proud of our Moodle site and it has a wealth of resources attached to it. Explore our pages
early in the course so you know the range of resources available to you. Make use of it!

Learn from your mistakes.
Many students have a tendency to get back an exam, look at their score, get upset and use that energy to
make them more nervous on the next exam. This is missing a very important opportunity to do some
serious learning. When you get an exam back and after you have gotten over the shock of the grade, it is
time to look at your mistakes and ask yourself what went wrong. Were you concentrating? Were you
nervous? Were you clueless about the material? Did you know the answer but have trouble writing what
you thought you knew? Did you think that all your answers were correct until you got the exam back?
Would you give the same answers if you took the exam again? Whatever the reason we will be able to
figure it out together and help you improve for your next test.
Get help when you need it.
The responsibility for learning the material is YOURS and no one else’s. Talk to your teacher, even when we
are busy we will try to find a way to help you. If you are having trouble understanding the material from
the reading, find another source such as a different textbook that may present the material in a different
style. Find a student who has studied the course last year. Go to Lab 8 and ask a mentor to work through
that section with you. There is an enormous amount of good will and willingness to assist amongst our
staff and students, but you have to be proactive and ask for it. This is YOUR education; you should care
enough to take the initiative.
Decide if you are willing to "pay the price".
As mentioned earlier, getting a superior grade is like winning an athletic or musical competition; it takes
some talent and a lot of hard work. Very often, this comes at a price and those who do the best are
typically the ones who consistently work the hardest. Each student needs to determine the importance of
their academic performance and make the necessary adjustments in their life. I point this out so that you
at least become aware of the importance of your studies in your life. If you are honest with yourself about
the importance of your academic career and make the necessary lifestyle adjustments, your life will be
much less stressful. Think about your long term goals and decide what value your academic performance,
extracurricular activities, and social life will have in the long run. Make the necessary adjustments in your
schedule. Balance does not necessarily mean equal time for all. Remember, there is no room on your final
exam for excuses.
Course requirements
The entry requirements to be accepted for A-level Chemistry are a minimum of a B grade in Core and
Additional Science or Chemistry, as well as a B in GCSE Maths and GCSE English. You will need to
demonstrate that you possess this level of knowledge at the start of the course. Therefore, when you are
revising during the summer look through all your GCSE notes/textbook/revision guide not only the topics
covered below.
Once you have been accepted to the course we preferred if you took either AS Maths or Core Maths to be
successful in achieving a good grade.
You will have Home Learning tasks to do most every day and you will have to be prepared to do them, and
work and practice your new skills at least one hour for each lesson you have.
Topics you need to be proficient at
Think of this material as pre work to help YOU out. It should give an idea of what you know already and
what you don’t. If you are struggling with a lot of this work don’t panic, start looking through some of your
GCSE notes NOW or use the internet to help you out. If all else fails there will be a support pack at the
beginning of term to help you out if you need it.
1.
2.
3.
4.
5.
6.
7.
8.
Atomic structure
Electronic structure
Writing formula
Balancing equations
Ionic bonding
Covalent bonding
Moles
Enthalpy calculations
In order to get off to a good start in your A-level Chemistry studies you need to be fluent in the topics
below before you start the course. For each, we have included links to resources to help you.
Depending on how competent you are in these topics you may not need to watch/read all of them. You
are welcome to find clips/resources that suit you better (please email us the links if you do and why you
found that resource better than the one included here).
Apart from the topic videos below, you can practice your problem solving and exam technique skills
using the Royal Society of Chemistry link:
http://www.rsc.org/learn-chemistry/resources/problem-solving-tutor/
Number of protons, neutrons and electrons in an atom/ion/isotope
https://www.youtube.com/watch?v=lP57gEWcisY
https://www.youtube.com/watch?v=SoMNy2fAoiE
https://www.youtube.com/watch?v=DZGINaRUEkU&list=PL701F0464C7551022
http://www.chemguide.co.uk/atoms/properties/gcse.html
Relative atomic mass, calculating molar masses
https://www.youtube.com/watch?v=aqfQKzbTCVo
https://www.youtube.com/watch?v=guAbb_yBSfs
Dot and cross diagrams for ionic and covalent compounds, diagram for the structure of metallic
compounds
http://www.chemguide.co.uk/atoms/bonding/ionic.html (only the GCSE revision bit)
http://www.chemguide.co.uk/atoms/bonding/covalent.html (only the GCSE revision bit)
http://www.chemguide.co.uk/atoms/bonding/metallic.html
https://www.youtube.com/watch?v=upg-FUHp6ys
https://www.youtube.com/watch?v=T8-zfrcaCfk
https://www.youtube.com/watch?v=fRoc6VU_VKY
Symbols for the first 20 elements – learn them off the Periodic table
Formulae of ionic and covalent compounds
https://www.youtube.com/watch?v=URc75hoKGLY (check out other videos of Tyler, he’s good and he
has videos for most topics you need to know)
https://www.youtube.com/watch?v=NWE4LYkG3po
https://www.youtube.com/watch?v=fpIEkL6cFN8
https://www.youtube.com/watch?v=vKNTspmfNqU
Writing chemical equations (from word equation into formulae equation and vica versa)
https://www.youtube.com/watch?v=bGU6mQ6mC_s (mole ratios = stoichiometry)
https://www.youtube.com/watch?v=wSKfExxpbH8
Balancing equations
https://www.youtube.com/watch?v=UGf60kq_ZDI
Reactions of metals, metal oxides and metal carbonates (with acids or water) – from your GCSE
textbook or BBC bitesize
Substituting into mathematical equations, re-arranging equations – from your GCSE Maths textbook or
BBC bitesize
Moles
https://www.youtube.com/watch?v=JC76NR8EtTQ
https://www.youtube.com/watch?v=wrGhyhgwODo
https://www.youtube.com/watch?v=Ik4zE8lXWs8
https://www.youtube.com/watch?v=QjU6kGaq5-I
Oxidation/reduction
https://www.youtube.com/watch?v=hSNwds-H1_0
https://www.youtube.com/watch?v=lxEvuJPTvew
% by mass
https://www.youtube.com/watch?v=ZyFCIcQyI48
First round of questions
Target Time: 30 mins
Time actually taken to complete:____ min
Marks:____ /30
Helpful information:
For Atomic masses, please use:
H = 1; S = 32.1; Mg = 24.3; O = 16.0; C = 12.0; Ti = 47.9; Na = 23.0; Cl = 35.5; N = 14.0.
Avogadro’s number = 6.02 × 1023.
1 mol of gas molecules occupies 24.0 dm3 at room temperature and pressure, r.t.p.
Questions:
1
Draw a Dot and cross diagram of the bonding in methane
[2]
2
Draw a Dot and cross diagram of the bonding in magnesium chloride
[2]
3
Write balanced equations for the following reactions:
[8]
a)
heating magnesium and sulphur powders together produces solid magnesium sulphide.
b)
sodium hydroxide and hydrochloric acid react to form sodium chloride and water.
c)
hydrogen gas and oxygen gas burn together to form water.
d)
zinc metal and copper sulphate solution react to produce copper and zinc sulphate solution.
4
5
A pint of water weighs 568g. How many molecules of water does that contain?
Show you working
[3]
Natural gallium comprises 60.4% 69Ga and 39.6% 71Ga.
Calculate the relative atomic mass of gallium.
[1]
6
When sodium reacts with titanium chloride (TiCl4), sodium chloride and titanium are produced.
Give all answers to 3 significant figures.
a)
Write the balanced symbol equation for the reaction.
[2]
b)
What mass of titanium is produced from 380 g of titanium chloride?
[2]
c)
What mass of titanium is produced using 46.0 g of sodium?
[2]
7
A student heats 5.29 g of Sr(NO3)2 and collects the gas at room temperature and pressure, RTP.
2Sr(NO3)2(s) → 2SrO(s) + 4NO2(g) + O2(g)
Calculate the volume of gas, in dm3, obtained by the student at RTP.
[3]
Molar mass of Sr(NO3)2 = 211.6 g mol –1.
answer = ............................... dm3
8
The energy from burning 1.5 g of propane, C3H8, was transferred to 200cm3 of water to raise its
temperature by 26 oC.
Calculate the energy change in kJ and then use this to calculate the enthalpy change (per mole).
[5]
The density of water is 1.00g/cm3
Specific heat capacity of water is 4.2 J/mol/K
answer = ...............................kJ/mol
Second round of questions
Target Time: 31 mins
Time actually taken to complete:____ min
Marks:____ /31
Helpful information:
For Atomic masses, please use:
H = 1; S = 32.1; Mg = 24.3; O = 16.0; C = 12.0; Ti = 47.9; Na = 23.0; Cl = 35.5; N = 14.0.
Avogadro’s number = 6.02 × 1023.
1 mol of gas molecules occupies 24.0 dm3 at room temperature and pressure, r.t.p.
Questions:
1.
Draw a dot-and-cross diagram to show the bonding in:
a) carbon dioxide
[2]
b) calcium oxide
[2]
2
Write a balanced equation for each of the following decomposition reactions.
[6]
a
lithium nitrate(V) decomposing to give lithium oxide, nitrogen dioxide and oxygen
b
magnesium hydroxide decomposing to give magnesium oxide and water
c
calcium hydrogencarbonate decomposing to give calcium carbonate, water and
carbon dioxide
3
The naturally occurring isotopes of magnesium and neon are shown in the table below
along with their relative abundance. Calculate the relative atomic mass for each element. [3]
Element
Atomic mass of isotope
Relative abundance %
Neon
20
90.92
21
0.26
22
8.82
4a
Write a balanced symbol equation and a mass equation for the reaction between
copper(II) oxide and nitric acid.
[2]
b
What mass of copper(II) nitrate will be produced when the following masses of
copper(II) oxide react with excess nitric acid?
i
7.95 g
[1]
ii
159 kg
[1]
5
Octane burns completely in oxygen to produce carbon dioxide and water vapour.
2 C8H18
+
25 O2 
16 CO2
+
18 H2O
When 114g of octane burns completely in 400g of oxygen it produces 162g of water vapour.
What mass of carbon dioxide would be produced from burning 114g of octane?
Show clearly how you work out your answer.
[2]
6.
7
How many oxygen molecules are in 12 dm3 of oxygen gas? What would that weigh?
Show your working.
[4]
A student does a titration to find the concentration of a solution of hydrochloric acid.
The student titrates 25.00 cm3 of hydrochloric acid with sodium hydroxide solution of
Concentration 0.200 moles per dm3. The equation for the reaction is:
HCl + NaOH  NaCl + H2O
The student added 28.60 cm3 of sodium hydroxide solution to neutralise the hydrochloric acid.
Calculate the concentration of the hydrochloric acid.
[3]
8.
Concentration = ___________ mol/dm3
The energy from burning 0.5g of propane, C3H8, was transferred to 100cm3 of water to raise its
temperature by 20 oC. Calculate the enthalpy change in kJ and then use this to calculate the
enthalpy change (per mole).
The density of water is 1.00g/cm3
specific heat capacity of water is 4.2 J/mol/K
[5]
Mark Scheme for the First Round of questions
1.
one mark for correct electrons, one mark for CH4 with overlap as shown
[2]
2
One mark for the dot and cross
of each correct ion (number
AND type of electrons AND
charge (magnesium can be all
crosses but then chloride must
have one cross and the rest as
dots))
Even if above is correct, only
one mark if there is only one
chloride ion [2]
or
3.
Mg + S  MgS
NaOH + HCl  NaCl + H2O
2H2 + O22 H2O
Zn + CuSO4  Cu + ZnSO4
for all formulae correct in each equation [1]
for balancing each equation [1]
4x2=8 marks
4
RMM H2O = (1=1=16) = 18g
[1]
568/18 = 31.556 moles
[1]
Each mole contains 6.02 × 1023
31.556 x 6.02 × 1023 = 1.90 x 1025 molecules [1]
5.
[(60.4 x 69 ) + (39.6 x 71)]/100 = 69.792
6
a
b
c
4Na + TiCl4
4NaCl + Ti
[1]
for correct formula [1]
1 mol of TiCl4 gives 1 mol of Ti
189.9 g of TiCl4 47.9 g of Ti
[1]
1 g of TiCl4 47.9 /189.9 g of Ti
380 g of TiCl4 380 ×47.9/189.9
= 95.9 g of Ti
[1]
4 mol of Na give 1 mol of Ti
92.0 g of Na 47.9 g of Ti
[1]
1 g of Na
46 g of Na
[1]
for balancing [1]
g of Ti
46 ×
= 24.0 g of Ti
7
Mol of Sr(NO3)2 =
5.29
 0.0250
211 .6
Mol of gas = 5/2 × 0.0250 = 0.0625
[1]
[1]
Volume of gas = 24.0 × 0.0625 = 1.50 dm3
ALLOW 0.025
ALLOW ECF for first answer × 2.5
[1]
ALLOW ECF for second answer × 24(.0)
ALLOW ECF producing correct volume of NO2 only i.e. 1.2(0) dm3 would give two arks
OR
ALLOW ECF producing correct volume of O2 only i.e. 0.3(0) dm3 would give two
marks
8.
200 x 4.2 x 26 = 21840J
218400J ÷ 1000 = 218.4kJ
Molecular mass of propane = (3x 12) + (8 x 1) =44
Moles of propane burned = 1.5 ÷ 44 = 0.03409
Enthalpy change = 218.4 ÷ 0.03409 = 6406 kJ/mol
[1]
[1]
[1]
[1]
[1]
Mark Scheme for the Second Round of questions
1
a
one mark for correct bonding electrons with overlap as shown, one mark for oxygen’s lone pairs
[2]
b
One mark for the dot and cross of each
correct ion (number AND type of
electrons AND charge (magnesium can
be all dots but then the oxide must have
two dots and the rest as crosses))
[2]
Electrons do not have to be in pairs; the
two different electrons in oxide can be
next to each other
2
a
4LiNO3  2Li2O + 4NO2 + O2
b
Mg(OH)2  MgO + H2O
c
Ca(HCO3)2  CaCO3 + H2O + CO2
for all formulae correct in each equation [1]
for balancing each equation [1]
3 Consider the total mass of 100 atoms.
Neon
Total mass of 100 atoms = (20 × 90.92) + (21 × 0.26) + (22 × 8.82) [1]
= 1818.4 + 5.46 + 194.04= 2017.9
Average (relative atomic mass) = 2017.9 /100= 20.18
[1]
[1]
4
a
CuO + 2HNO3 + Cu(NO3)2 + H2O
[1]

[1]
Mass equation: 79.5 + 126
187.5 + 18.0
bi
ii
18.8 g
375 kg
[1]
[1]
5
(400 +114 -162)/2 = 352 (g)
[2]
400 +114 -162 gains 1 mark
6. One mole of any gas = 24dm3 therefore 12 dm3 = 12/24 = 0.5 moles
One mole contains 6.02 x 10 23 particles therefore 0.5 x 6.02 x 10 23 = 3.01 x 10 23
Mr O2 gas = 16 x 2 =32
therefore 0.5 moles x 32 = 16g
7
0.2288
accept 0.229 or 0.23
[3]
If answer is incorrect:
28.6 x 0.2 ÷ 1000 (=0.00572) gains 1 mark
0.00572 x 1000 ÷ 25 or ecf gains 1 mark
28.6 x 0.2 ÷ 25 gains 2 marks
8
100 x 4.2 x 20 = 8400J
8400J ÷ 1000 = 8.4kJ
Formula mass of propane = (3x 12) + (8 x 1) =44
Moles of propane burned = 0.5 ÷ 44 = 0.01136
Molar enthalpy change = 8.4 ÷ 0.01136 = 739 kJ/mol
[1]
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