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1 Name: DEADLINE: 1 st lesson back, September term The aim of this preparation work is to revise GCSE chemistry topics that you will need for A Level course. Part A is for everyone to complete. Part B is for pupils who sat ADDITIONAL SCIENCE only. Part C is for pupils who sat GCSE CHEMISTRY. (optional for Additional science students)

2 Course preparation: resources You need to download the specification for the AS/A2 course: You need to buy text books to study support the first year of your A level chemistry study: 1) Recommended for anyone who did not do triple science (but useful to those who did as a refresher): A copy of a bridging revision guide that covers topics from GCSE into AS. We will be testing you on similar content in September. Label it with your name. Head start to A Level Chemistry Product details CGP publishing Publisher: Coordination Group Publications Ltd (CGP) (2 Mar. 2015) ISBN-10: ISBN-13: ) Your own copy of course textbook and label it with your name. This has a very useful online active book log on that you can use to support your studies. OCR AS/A Level Chemistry A Student Book 1 (+ Activebook 2015) Sam Holyman, David Scott and Victoria Stutt Product details Publisher: Pearson; 2 nd edition (26 Jun. 2015) ISBN-10: ISBN-13:

3 Part A: All pupils should complete these exercises Exercise 1: Balancing equations Balance the following formula equations: a K + Cl 2 KCl b Zn + HF ZnF 2 + H 2 c H 2 O 2 H 2 O + O 2 d H 2 O + Na NaOH + H 2 e C 6 H 12 + O 2 H 2 O + CO 2 f HCl + Ca H 2 + CaCl 2 Exercise 2: Atomic structure What is the currently accepted structure of the atom used in chemistry? Draw a labelled diagram including the position, mass and charge of neutrons, protons and electrons. Exercise 3: calculating Mr Use the relative atomic masses (Ar) on the Periodic table to answer the following questions. What is the formula mass of THE FOLLOWING? SHOW YOUR WORKING OUT a) NaCl b) MgO Mr= (Ar) where Ar=relative atomic mass of each element in the compound, =sum of (addition) c) CaSO 4 d) Pb(NO 3 ) 2 e) NH 4 Cl f) (NH4) 2 SO 4

4 Exercise 4: calculating number of moles and mass. 1) A mole contains a specific mass and number of particles of a substance. For example, 1 mole of carbon solid (Ar 12) has a mass of 12 g and contains atoms of carbon. Fill the gaps in the following statements about the mass and number of particles in a mole of a substance. You will need the periodic table to help you. a) 1 mole of sodium metal has a mass of g and contains of sodium. b) 1 mole of water (H2O) has a mass of g and contains 6x10 23 of water. c) 1 mole of oxygen (O2) gas has a mass of g and contains of oxygen. 2) How many moles are in the following? SHOW YOUR WORKING OUT a) 800 g of sodium hydroxide (NaOH) b) 19 g of magnesium chloride (MgCl2) n= mass/mr where Mr=relative molecular mass of the compound, mass is the amount of the substance in grams, n is the number of moles c) 4.24 g of sodium carbonate (Na2CO3) d) g of tin hydroxide (Sn(OH)2) e) 297 g of ammonium sulfate ((NH4)2SO4) f) 9.8 g of sulfuric acid (H2SO4) g) g of barium nitrate (Ba(NO3)2)

5 3) What is the mass of the following? SHOW YOUR WORKING OUT a) 2 moles of ammonia gas (NH3) b) 3 moles of methane gas (CH4) n= mass/mr where Mr=relative molecular mass of the compound, mass is the amount of the substance in grams, n is the number of moles c) 4 moles of carbon dioxide gas (CO2) d) 1.5 moles of sulfur dioxide (SO 2 ) e) 0.5 moles of aluminium sulfate (Al2(SO4)3) f) 2.5 moles of ethene gas (C4H8) g) 0.25 moles of magnesium sulfate (MgSO4) 4) Use the mass equation to work out how much product is made. (Hint: work out number of moles of the reactant, rearrange the equation to get mass then put the number of moles and Mr of product in) a What mass of water is formed by burning 1 g of methane? Show your working. CH 4 + 2O 2 CO 2 + 2H 2 O b Calcium carbonate breaks down when heated. What mass of calcium oxide would be formed by heating 25 g of calcium carbonate? Show your working. CaCO 3 (s) CaO(s) + CO 2 (g)

6 Exercise 5: Calculating volumes and molarities (FROM TRIPLE SCIENCE CHEMISTRY MODULE) n= MV/1000 where M=concentration in mol dm 3, V is volume in cm 3, n is the number of moles 1) Calculate the number of moles in the following solutions: a) 800 cm 3 of 0.5 mol dm 3 of nitric acid b) 25 cm 3 of 2 mol dm 3 of hydrofluoric acid c) 30 cm 3 of 2.5 moldm -3 of nitric acid 2) Calculate the molarity of the following solutions: a) 25cm 3 of 1 mole hydrochloric acid b) 1000cm 3 of 0.5 mole sodium ethanoate c) 250 cm 3 of 0.4 mole potassium bromide 3) A 250 cm 3 bottle of sodium hydrogen carbonate (NaHCO3) solution was found to have a concentration of 8 mol dm 3. How much solid was dissolved to make it? (Hint: work out number of moles of the reactant, rearrange the mass equation to get mass then put the number of moles and Mr of product in).

7 Exercise 6: Structure and bonding Using diagrams and examples, illustrate the range of bonding and structure in molecules that is studied at GCSE. Your diagrams should show the bonding between atoms/molecules and how the structure of a chemical is organised. 1) Giant covalent (include 2 examples) Bonding Structure 2) Simple covalent (include 2 examples including a hydrocarbon) Bonding Structure 3) Ionic (include 2 examples) Bonding Structure 4) Metallic (including one example) Bonding Structure

8 Exercise 7: Acids, Bases and Alkalis 1) What is the difference between a base and an alkali? 2) Complete the following equations by adding the missing chemical formula. Write the word equation underneath for each one. a) 2 (aq) + MgO(s) MgCl 2 (aq) + H 2 O(l) b) H 2 SO 4 (aq) + 2 (aq) Na 2 SO 4 (aq) + 2H 2 O(l) c) (aq) + NH 3 (aq) NH 4 NO 3 (aq) d) HCl (aq) + KOH(aq) (aq) + H 2 O(l) 3) Write balanced symbol equations (including state symbols) for the following reactions. a) Hydrochloric acid reacting with sodium hydroxide. b) Sulfuric acid reacting with copper oxide. c) Nitric acid reacting with magnesium oxide.

9 4) Answer the following questions on titration calculations (from triple science module) n= MV/1000 where M=concentration in mol dm 3, V is volume in cm 3, n is the number of moles n=mass/mr where Mr=relative molecular mass of the compound, mass is the amount of the substance in grams, n is the number of moles a) 22.5 cm 3 of sodium hydroxide solution reacted with 25.0 cm 3 of M hydrochloric acid. Calculate the concentration of the sodium hydroxide. NaOH(aq) + HCl(aq) NaCl(aq) + H 2 O(l) b) 25.0 cm 3 of mol/dm 3 sodium hydroxide solution reacted with 28.7 cm 3 of sulfuric acid. Calculate the concentration of the sulfuric acid. 2NaOH(aq) + H 2 SO 4 (aq) Na 2 SO 4 (aq) + 2H 2 O c) What mass of calcium carbonate is needed to neutralise 2 dm 3 of M hydrochloric acid. CaCO 3 (s) + 2HCl(aq) CaCl 2 (aq) +H 2 O(l) + CO 2 (g)

10 PART B: All ADDITIONAL GCSE SCIENCE pupils MUST complete the following research Research the following topics and record your research/knowledge in your own words. This is to catch you up on Triple science Chemistry topics that you missed so DO NOT COPY AND PASTE INFORMATION, YOU WILL NOT TAKE IT IN. You could present your research as a spider diagram for each topic or notes (bullet points or paragraphs) but cite any sources you use in a bibliography. You can find information in GCSE Chemistry textbooks and revision guides as well as the Head start to A Level book shown at start of this booklet. The following links may also be useful: From C3.1: The Periodic Table 1) How is the periodic table currently organised? 2) Give the name of TWO scientists who were involved in the development of the Periodic table and describe their theory/ input into the current structure. 3) How do group 1 metals react with oxygen and water? Why do they react like this? (must make reference to atomic structure) 4) In what state do group 7 elements occur at room temperature? Why is this? (must make reference to atomic structure and intermolecular forces) From C3.3: Energy changes in reactions 1) How do you calculate energy change in a reaction using specific heat capacity? (give the equation) 2) What is an exothermic reaction? How would you show an exothermic reaction on an energy profile diagram? 3) What is an endothermic reaction? How would you show an endothermic reaction on an energy profile diagram? 4) How can you calculate ta theoretical value for energy change in a reaction using bond energies? From C3.4 Analysis: 1) Describe how each of the following pieces of apparatus is used in the titration of an acid and an alkali: a) burette b) pipette. 2) What colour change occurs when phenolphthalein indicator is used in an acid-base titration? 3) How do you test for a carbonate ion? 4) How do you test for a sulfate ion? 5) How do you test for the three halide ions? 6) How can a flame test and sodium hydroxide solution be used to test for metal ions?

11 From C3.5: Reversible reactions 1) What is a reversible reaction? 2) What is an equilibrium? 3) Give three ways the position of an equilibrium can be changed. From C3.6: Organic compounds 1) Name and draw the first three members of the alcohol homologous series. 2) What is a carboxylic acid? Give one example in your answer 3) What is an ester? Give one example in your answer. YOUR WORK NEEDS TO BE READY TO HAND IN ON THE FIRST LESSON BACK PART C: All TRIPLE SCIENCE pupils MUST complete the following research Research the following topics and record your research/knowledge in your own words. This is to extend some of the work from the Triple science Chemistry units. DO NOT COPY AND PASTE INFORMATION, YOU WILL NOT TAKE IT IN. You could present your research as notes (bullet points or paragraphs) but cite any sources you use in a bibliography. You can find information in AS Chemistry books (module 1) and some in GCSE Chemistry textbooks and revision guides, as well as the Head start to A Level book shown at start of this booklet. Extending C1: 1. As the carbon chain of an alkane gets longer, what happens to it properties as a fuel? (viscosity, flammability and volatility) Why is this? (include intermolecular forces in your answer) Extending C2: 2. Why are the carbon structures of graphite, diamond and carbon dioxide so different? (Refer to structure and bonding in your answer) 3. What are the names of group 7 elements on the Periodic table? 4. How do the group 7 elements react with halide salts? Write word and symbol equations for reactions that would occur. Extending C3: 5. Why does the reactivity of group 7 elements vary down the group compared to group 6 elements? (Answer must refer to atomic structure) 6. How does the melting and boiling point of the group 7 elements change down the group? Why is this? (Link to atomic structure and intermolecular forces?) 7. In C3 you looked at group 1 metals, they have properties very similar to group 2 metals. How do these react with water? Give word and symbol equations for reactions that would occur. 8. Why does the reactivity vary down the group 2? (Answer must refer to atomic structure) YOUR WORK NEEDS TO BE READY TO HAND IN ON THE FIRST LESSON BACK

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