Groby Community College. A LEVEL CHEMISTRY: OCR Chemistry A INDUCTION HANDBOOK

Transcription

1 Groby Community College A LEVEL CHEMISTRY: OCR Chemistry A INDUCTION HANDBOOK 1

2 Introduction to the Course This course is intended to provide, through well designed studies of theoretical and practical chemistry, a worthwhile educational experience for candidates whether or not they go on to study Chemistry at a higher level. Advanced Subsidiary AS level This course has been developed for candidates who wish to continue with a study of chemistry after GCSE. You may wish to follow the course for one year in order to broaden your curriculum. The AS course does, however, provide a sound foundation for the second year of the Advanced GCE award. A summary of the scheme of work is given below:- Unit F321 Atoms, Bonds and Groups a) Atoms and Reactions b) Electrons, bonding and structure c) The periodic table Unit F322 Chains, Energy and Resources a) Basic Concepts and Hydrocarbons b) Alcohols c) Energy d) Resources e) Halogenoalkanes and Analysis Chemistry is a practical subject, and many of the lessons will use practical work to enhance and embed key concepts. In addition such work will help you develop practical skills which will be teacher-assessed in Unit F322 Practical Skills in Chemistry. A planner for the year, including what is taught when, as well as key assessment dates will be issued when the course starts in September A2 Chemistry The A2 course leads to an Advanced GCE qualification, which enables you to progress to degree level studies at University, particularly chemistry, medicine or medical science; or to enter employment where knowledge of chemistry would be useful. The course also provides an interesting and stimulating experience for anyone who does not wish to purse the subject further. Unit F324- Rings, Polymers and Analysis a) Rings, acids and amines b) Polymers and synthesis c) Analysis Unit F325 Equilibria, Energetics and Elements a) Rates, Equilibria and ph b) Energy c) Transition elements Once again practical work will be at the heart of the course and will be teacher-assessed in Unit F326 Practical skills in Chemistry 2.

3 Module Level Name Duration Mode of Assessment Atoms, bonds and F321 AS groups 1hr Written Exam Weighting R/U A Level 60 R 90 U 15% F322 AS Chains, energy and resources 1hr 45mins Written Exam 100R 150U 25% F323 AS Practical skills in chemistry 1 Internally assessed tasks 40R 60U 10% F324 A2 Rings, polymers and analysis 1hr 15 mins Written Exam 60 R 90 U 15% F325 A2 Equilibria, energetics and elements 2 hours Written Exam 100R 150U 25% F326 A2 Practical skills in chemistry 2 Internally assessed tasks 40R 60U 10% In 2014, AS students will take Units 1 & 2 (F321 & F322) during May or June (dates yet to be confirmed). Unit 3 tasks (F323) will be taken throughout the year from September to May. Resources For each year of the course there are Student Books, written specifically for the course. You will have the chance to buy your own copy of the Chemistry AS text book, which was written specifically for this course and is fully endorsed by the Awarding Body OCR. You should bring this to every lesson as you may need to refer to it at any time. We also recommend you use alternative texts to supplement your notes and enhance your study skills. Useful texts are available in both in the chemistry lab (room 21) and in the LRC. Notes

4 Student File and Lab Book You should separate your file into sections, one for each chapter. You are not required to bring your complete file to each lesson but you will be asked to submit it for review at key points during the year. It is expected that you will make your own notes to supplement the work in each lesson depending on the learning activity. We will provide a checklist for each unit to help you structure your notes Practical Work Practical work is at the heart of the course. The experimental work has been designed, as far as possible, to support the theory content you will cover in the various units, as well as to ensure that you develop the experimental skills which will be required for the practical skills tasks in units F323 and F326. We expect to see written reports for all practical tasks that include; Aim of activity Results tables and observations Analysis of results including percentage differences and uncertainties Conclusion Evaluation Answers to any supplementary questions Homework A paper copy of homework questions will be given and these should be included in the relevant section of your file. You can print out your own copies of extra questions which you have tried and these should be included. It is essential that deadlines are met at all times. Internal assessment In the AS course an assessment comprising AS-Level questions will be set after 3 weeks. There will be similar assessments at the end of every half term. These will be graded in line with A level grade boundaries and will be used to monitor your progress throughout the year. PRELIMINARY WORK It is vital that you build on the skills you have developed during GCSE, as year 12 builds on many of these skills. Examples of the kind of tasks we expect you to be able to do are illustrated in the activities below. Please complete these clearly laid out on A4 paper before your first lesson and bring to hand in. Your will also find it helpful to refer to the Chemistry Kick Start book available to buy from the school shop. ACTIVITY ONE Balance the equations below 1. C3H8 + O2 CO2 + H2O 2. Al2(SO3)3 + NaOH Na2SO3 + Al(OH)3 3. Al2O3 + Fe Fe3O4 + Al 4. KClO3 KCl + O2 5. NH4NO3 N2O + H2O 6. NaHCO3 Na2CO3 + H2O + CO2 7. P4O10 + H2O H3PO4 8. Al + H2SO4 Al2(SO4)3 + H2 9. Be2C + H2O Be(OH)2 + CH4

5 ACTIVITY TWO Relative atomic mass - atomic mass of the element (see periodic table). Element Sodium Oxygen Magnesium Sulphur Calcium Chlorine Aluminium Hydrogen Potassium Nitrogen Relative atomic mass Relative formula mass Mass of compound (Mr) - add up the atomic mass of each element in the compound. Compound NaOH KNO3 SO2 CaSO4 MgCO3 CuCO3 HNO3 Ca(OH)2 Na2CO3 H2SO4 Relative formula mass Moles A mole of any substance always contains same number of particles. One mole of any substance is the relative atomic (or formula) mass of that substance in grams. Mass = moles x relative atomic (or formula) mass Substance Mass of substance Number of moles Sodium 1 Magnesium 1 Lead 1 Barium 0.1 Chromium 0.1 Tin 0.1 HNO3 1 CuO 2 O2 1 H2O 0.5

6 Percentage mass (%) = Relative atomic mass of substance A x number of atoms of A x 100 Relative molecular mass of compound Find the percentage by mass of: a) Lithium and oxygen in lithium oxide, Li2O. b) Carbon and hydrogen in ethane, C2H6. c) Sodium, hydrogen and oxygen in sodium hydroxide, NaOH. d) Sodium and chlorine in sodium chloride, NaCl. Percentage yield This is the amount of product produced (in grams) divided by the maximum amount possible multiplied by 100 to produce a percentage. a) A reaction produces a theoretical yield of 200g but only makes 150g. What is the percentage yield? b) A reaction produces 60g of product but in theory makes 80g. What is the percentage yield? c) How much of reactant A is needed to make 80g of product D if the percentage yield is 75%? Empirical formulae From the mass of each element present in a sample we can find the formula of the compound. 1. Sodium (2.3g) combine with oxygen (0.8g). How many moles of sodium and oxygen are there? How many moles of sodium combine with 1 mole of oxygen? What is the formula of sodium oxide? 2. Magnesium (0.27g) combine with nitrogen (0.28g). How many moles of magnesium and nitrogen are there? How many moles of magnesium combine with 1 mole of nitrogen? What is the formula of Magnesium nitride? 3. Iron (1.68g) combine with oxygen (0.64g). How many moles of each element are there? How many moles of Iron combine with 1 mole of oxygen? What is the formula for this Iron oxide? 4. A compound contains 55.5% mercury; 44.5% bromine. How many grams of mercury and bromine are there in 100g of the compound? How many moles of mercury and bromine are there in 100g of the compound? What is the ratio of moles of bromine to moles of mercury. What is the formula? More balancing equations Remember that the number of atoms of each element on one side of the arrow must equal the other side of the arrow. Don t forget the state symbols 1. Na2O(s) + H2O(l) NaOH(aq) 2. KClO3(s) KCl(s) + O2(g) 3. Fe(s) + O2(g) Fe2O3(s) 4. Mg(s) + O2(g) MgO(s) 5. H2S(g) + O2(g) H2O(g) + SO2(g)