Chemistry department

A level induction

A Level Chemistry Preparation Work – Preliminary work

Please click the following link A Level Chemistry Preparation Work 2020 and work through the folder. Markschemes are provided for the preliminary work. Then complete the Induction booklet. No markscheme is provided for the Induction booklet and this must be handed in at the start of the course.

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Chemistry department

A level induction booklet

Name:_____________________________________________

Mark ______ / 100

Please complete the questions in this booklet over the summer break. Hand in your completed booklets to your Chemistry teacher during the first lesson next term. Date to hand in: Thurs 3rd Sept 2020 Please ensure you are confident with all the material covered in this booklet. It contains GCSE material only. If there is anything with which you are struggling, use some of the reference materials listed to do extra preparation in these areas.

If you fail to hand in this completed booklet you may be asked to leave the course, as it is a requirement by the Chemistry Department to start A Level Chemistry. There will be an introductory test within the first two weeks of term. The topics will be the initial A Level work and similar material to this induction booklet.

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General information - Course overview Year 12 Chemistry - The end of Year 12 internal school exams will be arranged in the format

shown below. Highlighted topics are examined in both papers.

1. Physical Chemistry Examined in Paper 1 Examined in Paper 2

3.1.1 Atomic structure √

3.1.2 Amount of substance √ √ 3.1.3 Bonding √ √ 3.1.4 Energetics √ √ 3.1.5 Kinetics √ 3.1.6 Chemical equilibria, Le Chatelier’s and Kc √ √ 3.1.7 Oxidation, reduction and redox reactions √

2. Inorganic Chemistry

3.2.1 Periodicity √

3.2.2 Group 2 – the alkaline earth metals √

3.2.3 Group 7 – the halogens √

3. Organic Chemistry

3.3.1 Introduction to organic chemistry √ 3.3.2 Alkanes √

3.3.3 Halogenoalkanes √

3.3.4 Alkenes √

3.3.5 Alcohols √

3.3.6 Organic analysis √

4. Relevant practical skills √ √

Paper 1 - 1 hour 30 minutes - 80 marks 65 marks of short and long questions 15 marks of multiple choice questions

Paper 2 - 1 hour 30 minutes - 80 marks 65 marks of short and long questions 15 marks of multiple choice questions

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A level - Year 13 - Highlighted topics are examined in all three papers 1. Physical Chemistry Examined in

Paper 1 Examined in Paper 2

Examined in Paper 3

3.1.1 Atomic structure √ √ 3.1.2 Amount of substance √ √ √ 3.1.3 Bonding √ √ √ 3.1.4 Energetics √ √ √ 3.1.5 Kinetics √ √ 3.1.6 Chemical equilibria, Le Chatelier’s and Kc √ √ √ 3.1.7 Oxidation, reduction and redox reactions √ √ 3.1.8 Thermodynamics √ √ 3.1.9 Rate equations √ √ 3.1.10 Equilibrium constant Kp for homogeneous systems √ √ 3.1.11 Electrode potentials and electrochemical cells √ √ 3.1.12 Acids and bases √ √ 2. Inorganic Chemistry

3.2.1 Periodicity √ √ 3.2.2 Group 2 – the alkaline earth metals √ √ 3.2.3 Group 7 – the halogens √ √ 3.2.4 Properties of Period 3 elements & oxides √ √ 3.2.5 Transition metals √ √ 3.2.6 Reactions of ions in aqueous solution √ √ 3. Organic Chemistry

3.3.1 Introduction to organic chemistry √ √ 3.3.2 Alkanes √ √

3.3.3 Halogenoalkanes √ √

3.3.4 Alkenes √ √

3.3.5 Alcohols √ √

3.3.6 Organic analysis √ √ 3.3.7 Optical isomerism √ √ 3.3.8 Aldehydes and ketones √ √ 3.3.9 Carboxylic acids and derivatives √ √ 3.3.10 Aromatic chemistry √ √ 3.3.11 Amines √ √ 3.3.12 Polymers √ √ 3.3.13 Amino acids, proteins and DNA √ √ 3.3.14 Organic synthesis √ √ 3.3.15 Nuclear magnetic resonance spectroscopy √ √ 3.3.16 Chromatography √ √

4. Relevant practical skills √ √ √

Paper 1 - 2 hours - 105 marks - 35% of A level (105 marks of short and long questions)

Paper 2 - 2 hours - 105 marks - 35% of A level (105 marks of short and long questions)

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Paper 3 – 2 hours – 90 marks – 30% of A level (40 marks of questions on practical techniques and data analysis, 20 marks of questions testing across the specification, 30 marks of multiple choice questions) Reading list You are strongly advised to undertake some background reading before and during the course. The course book is the AQA Chemistry A Level Student Book, listed below. You are advised to purchase your own copy of the two year book. Initially you will be issued with a book to cover Year 12, but it is helpful to be able to view the whole course content of the text book. You may also may wish to purchase an additional textbook, calculations book or revision guide to help consolidate your learning, and for background reading. Possibilities include:

Calculations in AS/A Level Chemistry (Jim Clark) ISBN 978-0-582-41127-2

AQA Chemistry A Level Student Book (Ted Lister, Janet Renshaw) ISBN 978-0-19-835182-5

Advanced Chemistry (Michael Clugston, Rosalind Fleming) ISBN 978-0-19-9839291-0

CGP Revisions guides are now published Browse through the books in a good bookshop, and choose the one that appeals to you! You are also advised to subscribe to a scientific journal. ChemNet The Royal Society of Chemistry offers free support and advice for all Chemistry students.

E-magazines – Chemistry World from Royal Society of Chemistry, featuring research and development in chemistry

RSC ChemNet Events – Free visits to industry, universities and talks on careers

RSC ChemNet ReAct – Ask the experts about tricky topics

Monthly e-newsletter

Careers / University advice – Help on applying for universities and jobs Chemistry Review magazine from the University of York, published by Hodder Stoughton has articles useful for A level students. Equipment Practical skills are an integral part of the course and all Chemistry students are expected to have their own clean lab-coat with their name written on the top pocket but no other writing or drawing. Long hair is expected to be tied back. You will also need to bring to lessons:

Pencil, pen and ruler

Calculator

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Resources The student area of the school website contains useful course information, and many of the PowerPoint presentations which will be used in lessons. This booklet will be available on the A level Chemistry site.

Careers You should be starting to think about your next steps in education, in particular what courses to apply for at University. An A level in Chemistry is an extremely versatile and well respected qualification which can provide a stepping stone for a wide variety of careers, both scientific and non-scientific. Chemistry is essential for Medicine, Dentistry and Veterinary Science, as well as very useful for Engineering. Careers information available to Chemistry students includes:

Opportunity to apply for Work Experience placements in the summer term

Guest speakers from a range of different careers to provide ideas

Numerous careers resources for scientists in the careers library When choosing a university course, remember that many courses can lead to careers in a whole array of different disciplines, taking a biochemistry degree does not mean you have to become a biochemist! If you are unsure about your career aspirations the best thing to do is apply for a pure science or engineering degree with a respected university in an area that interests you. If you are planning to go into Medicine you need to enter yourself to do the British Medical Association Test (BMAT) Chemistry teachers are available to offer individual advice and guidance, so please don’t be afraid to come and ask for help with your careers choices. Time management In the past we have found that some students struggle in coping with the jump from GCSE to AS level. You are expected to work the amount of time on homework/private study as you do in class lesson time. i.e. 5 hours of Chemistry homework per week! In this time you are expected to do homework, problems, extended reading etc all to support your learning in class. If you plan to study Medicine you are expected to join and run the school Medical & Veterinary Society where you will be organising guest speakers to come and talk about strange diseases!, read and discuss topical and ethical issues, obtain university interview practice and help in writing your UCAS statement. Extra support There is a weekly Chemistry Clinic provided which you will be asked to attend if you need extra help with any part of the course. It is your responsibility to make sure you are keeping up with the work! Some students need a bit more individual help to understand some of the material, so don’t be afraid to come along. Peer tutors from Year 13 will be available to offer help, as well as Chemistry teachers. Dates & times will be published in September.

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Please take note of the following 2 pages before attempting the questions. You should already know the 6 highlighted compound ions and be able to use these to quickly write correct formulae.All the other ions listed can be worked out. Note for transition element ions, the number after the name refers to the number of

positive charges on the ion eg iron (ii) = Fe2+ .

Charges on ions

Charge

Positive Negative

1+ 2+ 3+ 3- 2- 1-

Group 1 Group 2 Group 3 Group 5 Group 6 Group 7

H+

hydrogen

Cu+ Cu2+

copper (I) copper (ll)

Ag+ Fe2+ Fe3+

silver (I) iron (ll) iron (lll)

NH4 + Zn2+

ammonium zinc

Pb2+ OH-

lead hydroxide

NO3-

nitrate / nitrate (v)

NO2-

nitrite / nitrate (lll)

CO3 2- HCO3-

carbonate hydrogen carbonate

SO42- HSO4

-

sulphate hydrogen sulphate

SO3 2- HSO3-

sulphite hydrogen sulphite

PO43- HPO4

2- H2PO4-

phosphate hydrogen phosphate dihydrogen phosphate

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Naming elements: 1. Metal + non-metal. The metal name is unchanged, non-metal ends in ‘ide’ eg magnesium + oxygen = magnesium oxide 2. Two non-metals. Element to the left of the Periodic Table comes first. eg carbon + oxygen = carbon dioxide 3. Three elements, metal, non-metal + oxygen – name ends in ‘ate’ or ‘ite’ Eg sodium + sulphur + oxygen = sodium sulphate Na2SO4 or sodium sulphite Na2SO3 Naming acids Monoprotic acids (1 H atom per molecule so 1 H+ ion to release into solution) HCl = hydrochloric acid HF = hydrofluoric acid HNO3 = nitric acid Diprotic acids (2 H atoms per molecule so 2 H+ ions to release into solution) H2SO4 = sulphuric acid H2SO3 = sulphurous acid H2CO3 = carbonic acid Triprotic acids (3 H atoms per molecule so 3 H+ ions to release into solution) H3PO4 = phosphoric acid Naming salts formed from reactions with acids

HCl hydrochloric acid → chlorides eg sodium chloride

HNO3 nitric acid → nitrates eg potassium nitrate

H2SO4 sulphuric acid → sulphates eg copper sulphate

H3PO4 phosphoric acid → phosphates eg calcium phosphate Using formulae of acids to work out formulae of products eg salts in a reaction.

Eg. 1. sodium + sulphuric → sodium + water hydroxide acid sulphate

2NaOH + H2SO4 → Na2SO4 + 2H2O Explanation : Sulphuric acid contains a sulphate ion (SO4

2-) ie one with a 2- charge. So when Na+ ions join with an SO4 2- ion there must be 2 Na+ ions to balance the 2- charge on the SO4 2- ion so the formula is Na2SO4.

Eg. 2. sodium + phosphoric → sodium + water

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hydroxide acid phosphate

3NaOH + H3PO4 → Na3PO4 + 3H2O Explanation : Phosphoric acid contains a phosphate ion (PO4

3-) ie one with a 3- charge. So when Na+ ions join with a PO4 3- ion there must be 3 Na+ ions to balance the 3- charge on the PO4 3- ion so the formula is Na3PO4.

Questions 1. Write the formula of the following substances.

Some are ionic, some are atomic and some are molecular.

For the simple molecules or ions make sure you know which Group of the Periodic Table

the elements are in.

For those compounds with a negative compound ion make sure you know the formula

and charge of the negative ion, before stating the formula of the whole compound.

Use the table of Charges on ions and notes on the earlier pages of this booklet.

a) lithium oxide ___________ b) ammonia ____________

c) calcium nitrate ___________ d) nitrogen ____________

e) methane __________ f) argon ____________

g) ammonium sulphate ___________ h) iron (III) hydroxide ____________

i) aluminium oxide ___________ j) calcium phosphate ______________

k) calcium hydrogen carbonate _______ l) potassium dihydrogen phosphate _______ (12)

2. Give the formulas of the following compounds.

a) iron (iii) sulphate _____________ b) iron (ii) nitrate _______________ c) copper (i) iodide _____________ (3)

3. Balance the following equations.

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a) Fe + H2O Fe3O4 + H2 1

b) PCl3 + H2O P(OH)3 + HCl 1

c) sulphuric acid + sodium hydroxide sodium sulphate + water 2

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(4) 4. Complete the following calculations, giving your answers to three significant figures. a) 32420 + 762891 _____________________________________________________________________ b) 12000 ÷ 1000 _____________________________________________________________________ c) 0.06438 + 0.0004378 _____________________________________________________________________ (3) 5. The following results are accurately measured values from experiments. Complete the sum

and give the answer to the most number of significant figures that you think gives an answer that is trustworthy.

a) 1.4567 + 2.3 _____________________________________________________________________ b) 10.5 - 0.145 _____________________________________________________________________ c) 3.000 - 0.056 _____________________________________________________________________ d) 8693.457 + 1.2367 _____________________________________________________________________ (4) 6. Rearrange the following equations to give the letter shown as the subject. a) What does c equal if q = m c ΔT ?

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___________________________________________________________________

b) What does n equal if PV = nRT ?

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c) What does T equal if ΔG = ΔH – TΔS ?

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d) How do you work out the number of moles if ΔH = q / moles?

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7. What mass of hydrogen is produced when 192 g of magnesium is reacted with hydrochloric

acid? Hint: Calculate the number of moles of each substance. Make use of the mole ratio from

the equation. Show all working.

Mg + 2 HCl MgCl2 + H2

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(3)

8. What mass of oxygen is needed to react with 8.5 g of hydrogen sulphide (H2S)? Hint: Calculate the number of moles of each substance. Make use of the mole ratio from

the equation. Show all working.

2 H2S + 3 O2 2 SO2 + 2 H2O ___________________________________________________________________

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(3)

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9. 5.00 g of hydrated sodium sulphate crystals (Na2SO4.nH2O) gave 2.20 g of anhydrous sodium sulphate on heating to constant mass. Work out the relative molecular mass (Mr) of the hydrated sodium sulphate and the value of n.

Hint: Calculate the masses and number of moles of each PRODUCT. Show all working.

Na2SO4.nH2O Na2SO4 + n H2O

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(3)

10. When titrating a strong acid and a strong alkali any indicator may be used. Suggest a suitable indicator for:

a) weak acid and strong alkali ___________________________________________ 1

b) strong acid and weak alkali ___________________________________________ 1 (2)

11. The concentration of a solute may be quoted as the number of moles per cubic decimetre (mol / dm3 or mol dm-3). 1 dm3 = 1000 cm3 25.0 cm3 NaOH of unknown concentration was titrated against 20 cm3 0.5M HCl (0.5M = 0.5 mol / dm3). Calculate the concentration of NaOH. Hint: Write the equation first, work out number of moles of HCl, then use mole ratio to work out moles, then concentration of NaOH. Show all working. _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________

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12. 25.0 cm3 2M NaOH (2 mol / dm3) was titrated against 18.5 cm3 H2SO4. Calculate the

concentration of H2SO4. Hint: Write the equation first, being careful to give the correct formula of products which will allow you to obtain the correct mole ratio for the reacting particles. Work out number of moles of NaOH, then use mole ratio to work out moles, then concentration of H2SO4. Show all working. _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _________________________________________________________________________ (3)

13. 25.0 cm3 NaOH of unknown concentration was titrated against 21 cm3 0.5M (0.5 mol / dm3)

phosphoric acid (H3PO4). Calculate the concentration of NaOH. Hint: Write the equation first, being careful to give the correct formula of products which will allow you to obtain the correct mole ratio for the reacting particles. Work out number of moles of H3PO4 then use mole ratio to work out moles, then concentration of NaOH. Show all working. _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ ________________________________________________________________________ (3)

14. The specific heat capacity of water is 4.2 J/g/°C (Joules per gram per degree Celsius), so it

takes 4.2 Joules of energy to raise the temperature of 1g water by 1 °C.

When 50 cm3 of 1.0 mol / dm3 HCl reacts with 50 cm3 of 1.0 mol / dm3 NaOH the temperature rises by 6.6 °C. Use the equation q = m c ∆T to calculate the energy change during this reaction.

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(The specific heat capacity for the acid / alkali mixture can be taken to be the same as that for water). ____________________________________________________________________________ ____________________________________________________________________________ ____________________________________________________________________________ ____________________________________________________________________________ __________________________________________________________________________ (3)

15. Flame tests can be used to identify positive ions in a compound. A platinum wire loop is dipped in concentrated HCl and heated in a roaring flame. A small amount of each substance may be collected on the wire loop and held in a roaring flame.

Name the elements that givg the following colours: a) bright red ______________________ b) golden yellow _______________________ c) lilac ______________________ d) brick red _______________________ e) green ______________________ (5) 16. Sodium hydroxide NaOH may be added to compounds containing positive ions. Characteristic

precipitates (solids) may be formed. a) Name 3 metal ions that give white precipitates with NaOH. _______________________________________________________________________ _______________________________________________________________________ _____________________________________________________________________3

b) How would you distinguish between the 3 metal ions listed in part a? ________________________________________________________________________ ________________________________________________________________________ ______________________________________________________________________ 2 (5)

17. Which metal ion reacts with NaOH to give:

a) light blue precipitate ________________________________________

b) dirty green precipitate _______________________________________

c) red-brown precipitate _______________________________________ (3)

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18. To test for NH4

+ (ammonium) ions, NaOH is added and the solution is warmed.

What is the result? ___________________________________________________ ____________________________________________________________________ How could you test for it? _____________________________________________ ____________________________________________________________________ (3) 19. Complete the following general equations:

a) acid + metal _________________________________ 1

b) acid + alkali _________________________________ 1

c) acid + carbonate _________________________________ 1 d) How do you test for sulphate (SO4 2-) ions? Describe a positive result?

____________________________________________________________________ ____________________________________________________________________ 2 (5) 20. How do you test for nitrate (NO3 -) ions? Describe the results. ____________________________________________________________________ ____________________________________________________________________ ____________________________________________________________________ (3) 21. How do you test for halide ions (Cl- Br- I-)? Describe the results. ____________________________________________________________________ ____________________________________________________________________ ____________________________________________________________________ (4) 22. This question is about reversible reactions and chemical equilibrium.

(a) Reversible reactions can reach equilibrium in a closed system.

(i) What is meant by a closed system?

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___________________________________________________________ (1)

(ii) Explain why, when a reversible reaction reaches equilibrium, the reaction appears to have stopped.

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(b) In the Haber process, the reaction of nitrogen with hydrogen to produce ammonia is reversible.

N2(g) + 3 H2(g) 2 NH3(g)

The forward reaction is exothermic.

The graph in Figure 2 shows the percentage yield of ammonia using different conditions.

Figure 2

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(i) Use Figure 2 to suggest the conditions that produce the greatest yield of ammonia.

__________________________________________________________________ (1)

State and explain:

(ii) how a decrease in temperature would affect the yield of ammonia

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(2)

(iii) how an increase in pressure would affect the yield of ammonia.

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(2)

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(iv) Use Figure 2 to suggest and explain why the conditions used to produce ammonia in the Haber process are a temperature of 450 °C and a pressure of 200 atmospheres.

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23. (a) An energy level diagram for the reaction between nitrogen and hydrogen is shown

below.

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(i) How does the energy level diagram show this reaction is exothermic?

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____________________________________________________________ (1)

(ii) In the Haber process iron is used as a catalyst.

Draw a line on the energy level diagram to show the effect of adding a catalyst. (1)

(b) The decomposition of hydrogen iodide into hydrogen and iodine is reversible.

2HI(g) H2(g) + I2(g)

The forward reaction is endothermic.

The energy level diagram shown below is for the forward reaction.

(i) Draw an arrow to show the activation energy on the diagram. (1)

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(ii) How does the diagram show that the reaction is endothermic?

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____________________________________________________________ (1)

(iii) Suggest what effect, if any, increasing the temperature will have on the amount of hydrogen iodide at equilibrium.

Give a reason for your answer.

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(2)

(Total 6 marks)