St. Thomas More High School A-LEVEL CHEMISTRY INDUCTION DAY INFORMATION and PRE-COURSE ACTIVITIES

St. Thomas More High School A-LEVEL CHEMISTRY INDUCTION DAY INFORMATION and PRE-COURSE ACTIVITIES

CHEMISTRY A-LEVEL A-level Chemistry goes into much more detail than GCSE. It attempts to answer the big question what is the world made of and it is the search for this answer that makes this subject so fascinating. From investigating how one substance can be changed drastically into another, to researching a new wonder drug to save millions of lives, the opportunities that chemistry provides are endless. What we study in A-Level Chemistry: A-level Chemistry lasts two years, with exams at the end of the second year. The table below shows what you can expect to learn in each year. Physical Chemistry Inorganic Chemistry First year of A-level Atomic Structure, Amount of Substance, Bonding, Energetics, Kinetics, Chemical Equilibrium Le Chatelier s Principle Periodicity, Group 2 - the Alkaline Earth Metals, Group 7 - the halogens Second year of A-level Thermodynamics, Rate Equations, The Equilibrium Constant, Electrode Potentials, Electrochemical Cells Properties of Period 3 elements and their oxides, Transition Metals, Reactions of ions in Aqueous Solution Organic Chemistry Introduction to Organic Chemistry, Alkanes, Halogenoalkanes, Alkenes, Alcohols, Organic analysis Optical Isomerism, Aldehydes and Ketones, Carboxylic Acids and derivatives, Aromatic Chemistry, Amines, Polymers, Amino Acids, Proteins and DNA, Organic Synthesis, NMR spectroscopy, Chromatography

Practicals Chemistry, like all sciences, is a practical subject. Throughout the course you will carry out practical activities including: measuring energy changes in chemical reactions tests for identifying different types of compound different methods for measuring rates of reaction studying electrochemical cells preparation of organic solids and liquids an advanced form of chromatography for more accurate results. These practicals will be assessed and your knowledge and understanding of these procedures will also be tested as part of your PAPER 3 examination at the end of the course. Exams The exam board is AQA. The course is split into 3 units: Unit 1 PHYSICAL CHEMISTRY Unit 2 INORGANIC CHEMISTRY Unit 3 ORGANIC CHEMISTRY These units are assessed in 3 papers that will all be sat at the end of the A2 year. Paper 1 Physical & Inorganic Chemistry inc. relevant practical skills (2hours, 105marks, 35% of A-Level). Paper 2 Physical & Organic Chemistry inc. relevant practical skills (2hours, 105marks, 35% of A-Level). Paper 3 Synoptic Any content and practical skills from the A-Level course can be assessed in this paper (2hours, 90marks, 30% of A-Level). The three exams at the end of the two years are all 2 HOURS long. There is no coursework on this course. However, your performance during practicals will be assessed. At least 15% of the marks for A-level Chemistry are based on what you learned in your practicals.

Entry Requirements To ensure you are able to meet the demands of this challenging A-Level course the entry requirements are as follows: GCSE Double Science at grade 77 or above OR GCSE Separate (Triple) Science at grade 777. GCSE Maths at grade 6 or above is also required. To study A-Level Chemistry you also need to be: Interested in Chemistry Willing to work extremely hard A good time manager Organised Able to persevere when faced by difficult/challenging topics. Who teaches the course? Currently A-Level Chemistry at St. Thomas More is taught by: MRS HARDIMAN If you have any further questions after today, please do not hesitate to contact me via the school email: office@st-thomasmore.southend.sch.uk Just mark the email FAO: Mrs Hardiman Preparing to Study A-Level Chemistry In the first 2 weeks of the course, all students will be required to sit a chemistry induction test on the topics covered at GCSE

Resources for Chemistry For all A-level chemistry lessons you will need: An A4 Lever-Arch Folder with Dividers A copy of the specification (this will be provided). A CGP revision guide (these can be purchased from the school in September). A scientific calculator. A Practical Book (this will be provided at the start of the course). Assessments in Chemistry An assessment will take place following the completion of every topic in chemistry and will be based on past examination questions. Your performance in these assessments will be regularly reviewed and used to determine your continuation on the course and/or examination entry.

What can you do once you have finished studying A-Level Chemistry? Possible Degree Options Currently, the most popular types of degree courses taken by students who have an A- level in Chemistry are: Chemistry Biology Medicine Mathematics Pharmacology Forensic Science Veterinary Science Dentistry Chemical Engineering Pharmacy Biochemistry Biomedical Sciences Possible career options Studying an A-level Chemistry related degree at university gives you all sorts of exciting career options, including: Doctor Vet Dentist Analytical chemist Chemical engineer Clinical biochemist Pharmacologist Research scientist (physical sciences) Toxicologist Chartered certified accountant Environmental consultant Higher education lecturer Patent attorney Science writer Secondary school teacher!!

A-Level Chemistry Induction Activities These questions are a combination of revision and past examination paper questions. They should be started during your induction session and completed and submitted in your first Chemistry lesson in September. Structure of the ATOM 1. Draw a labelled diagram of an atom. Include all of the SUB-ATOMIC PARTICLES and annotate with their RELATIVE CHARGES and RELATIVE MASSES. 2. Why is an atom electrically neutral? Refer to the diagram above in your answer.

3. Define the following terms: Atomic Number: Mass Number: Relative Atomic Mass (Ar): Relative Molecular Mass (Mr): 4. What is a MOLE in Chemistry? 5. What are the masses of one mole of the following: Chemical Sodium Potassium Lithium Oxygen gas Carbon Dioxide Water Calcium Carbonate Mass of one Mole

6. Follow the steps to find the percentage of iron in iron oxide. Relative atomic masses: O 16; Fe 56. (i) Step 1 Calculate the relative formula mass of iron oxide, Fe2O3....... (1) (ii) Step 2 Calculate the total relative mass of just the iron atoms in the formula, Fe2O3.... (1) (iii) Step 3 Calculate the percentage (%) of iron in the iron oxide, Fe2O3....... Percentage of iron... % (1)

7. (a) Nitric acid, HNO3, is made from ammonia by the Ostwald Process. There are three stages in this Process. Stage 1: Stage 2: Stage 3: ammonia reacts with oxygen, O2, from the air in the presence of a catalyst to form nitrogen oxide, NO. nitrogen oxide and oxygen react to form nitrogen dioxide, NO2. nitrogen dioxide, oxygen and water react together to form nitric acid. The equation for stage 1 is: 4NH3 + 5O2 4NO + 6H2O (i) (ii) Name the catalyst used in stage 1... Complete and balance the equations for the reactions taking place in stages 2 and 3. (1) Stage 2: 2NO + O2... (1) Stage 3:... NO2 +... H2O + O2... HNO3 (1) (b) Ammonium nitrate is an important fertiliser. It is made by reacting nitric acid with the alkali ammonia. (i) State the type of reaction taking place.... (1) (ii) The equation for this reaction is: NH3 + HNO3 NH4NO3 Calculate the number of tonnes of ammonium nitrate that can be made from 68 tonnes of ammonia. (Relative atomic masses: H = 1, N = 14, O = 16)............ (3) (Total 7 marks) 8. Titanium is a transition metal used as pins and plates to support badly broken bones. Titanium is extracted from an ore that contains the mineral titanium oxide. This oxide is converted into titanium chloride. Titanium chloride is heated with sodium to form titanium metal. This reaction takes place in an atmosphere of a noble gas, such as argon. 4Na(s) + TiCl4(l) Ti(s) + 4NaCl(s) Calculate the mass of titanium that can be extracted from 570 kg of titanium chloride. Relative atomic masses: Cl 35.5; Ti 48.......... Mass of titanium =... kg (Total 3 marks)

Q9. A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. In both reactions one of the products is copper chloride. (a) Describe how a sample of copper chloride crystals could be made from copper carbonate and dilute hydrochloric acid. (4) (b) A student wanted to make 11.0 g of copper chloride. The equation for the reaction is: CuCO3 + 2HCl CuCl2 + H2O + CO2 Relative atomic masses, Ar: H = 1; C = 12; O = 16; Cl = 35.5; Cu = 63.5 Calculate the mass of copper carbonate the student should react with dilute hydrochloric acid to make 11.0 g of copper chloride. Mass of copper carbonate = g (4) (c) The percentage yield of copper chloride was 79.1 %. Calculate the mass of copper chloride the student actually produced. Actual mass of copper chloride produced = g (2)

(d) Look at the equations for the two reactions: Reaction 1 Reaction 2 CuCO3(s) + 2HCl(aq) CuCl2(aq) + H2O(l) + CO2(g) CuO(s) + 2HCl(aq) CuCl2(aq) + H2O(l) Reactive formula masses: CuO = 79.5; HCl = 36.5; CuCl2 = 134.5; H2O = 18 The percentage atom economy for a reaction is calculated using: Calculate the percentage atom economy for Reaction 2. Percentage atom economy = % (3) (e) The atom economy for Reaction 1 is 68.45 %. Compare the atom economies of the two reactions for making copper chloride. Give a reason for the difference. (1) (Total 14 marks)

Q10. Sodium hydroxide neutralises sulfuric acid. The equation for the reaction is: 2NaOH + H2SO4 Na2SO4 + 2H2O (a) Sulfuric acid is a strong acid. What is meant by a strong acid? (2) (b) Write the ionic equation for this neutralisation reaction. Include state symbols. (2) (c) A student used a pipette to add 25.0 cm 3 of sodium hydroxide of unknown concentration to a conical flask. The student carried out a titration to find out the volume of 0.100 mol / dm 3 sulfuric acid needed to neutralise the sodium hydroxide. Describe how the student would complete the titration. You should name a suitable indicator and give the colour change that would be seen. (4)

Mean volume = cm 3 (2) Concentration = mol / dm 3 (4) (d) The student carried out five titrations. Her results are shown in the table below. Titration 1 Titration 2 Titration 3 Titration 4 Titration 5 Volume of 0.100 mol / dm 3 sulfuric acid in cm 3 27.40 28.15 27.05 27.15 27.15 Concordant results are within 0.10 cm 3 of each other. Use the student s concordant results to work out the mean volume of 0.100 mol / dm 3 sulfuric acid added. (e) The equation for the reaction is: 2NaOH + H2SO4 Na2SO4 + 2H2O Calculate the concentration of the sodium hydroxide. Give your answer to three significant figures.

(f) The student did another experiment using 20 cm 3 of sodium hydroxide solution with a concentration of 0.18 mol / dm 3. Relative formula mass (Mr) of NaOH = 40 Calculate the mass of sodium hydroxide in 20 cm 3 of this solution. Mass = g (2) (Total 16 marks)