Name: DEADLINE: 1 st lesson back, September term
|
|
- Tamsyn Foster
- 5 years ago
- Views:
Transcription
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
12
Please hand your completed booklet to your Chemistry tutor when you begin A Level Chemistry in September
#THIS I S TH E P L AC E A-LEVEL CHEMSITRY NAME: You should complete this work ready for starting Year 1 A Level Chemistry. If there are any questions that you cannot do, even after using your GCSE notes
More informationWhat is this booklet for: This is simply designed to be a bridging Chemistry booklet. It has work to prepare you for the A level you are starting in
1 What is this booklet for: This is simply designed to be a bridging Chemistry booklet. It has work to prepare you for the A level you are starting in September. It contains a series of topics that you
More informationRevision Checklist :4.3 Quantitative Chemistry
Revision Checklist :4.3 Quantitative Chemistry Conservation of Mass The law of conservation of mass states that no atoms are lost or made during a chemical reaction so the mass of the products equals the
More informationCHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS
Lesson 1 1. (a) Deduce the number of protons, neutrons and electrons in the following species: (i) 37 Cl - (ii) 1 H + (iii) 45 Sc 3+ (b) Write symbols for the following species: (i) 8 protons, 8 neutrons,
More informationIGCSE (9-1) Edexcel - Chemistry
IGCSE (9-1) Edexcel - Chemistry Principles of Chemistry Chemical Formulae, Equations and Calculations NOTES 1.25: Write word equations and balanced chemical equations (including state symbols): For reactions
More informationSIXTH FORM AES CHEMISTRY TRANSITION UNIT. Name: Secondary School
SIXTH FORM AES CHEMISTRY TRANSITION UNIT Name: Secondary School 0 1 Contents Introduction 2 Task 1: The structure of atoms 3 Task 2: Atoms and ions 4 Task 3: Writing formulas 5 Task 4: Relative masses
More informationQuantitative Chemistry. AQA Chemistry topic 3
Quantitative Chemistry AQA Chemistry topic 3 3.1 Conservation of Mass and Balanced Equations Chemical Reactions A chemical reaction is when atoms are basically rearranged into something different. For
More informationA level Chemistry Preparation Work
A level Chemistry Preparation Work This booklet is designed to help you prepare for you re A level studies in chemistry. Tasks have been selected to improve your grounding in key skills and concepts that
More informationCHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS
Lesson 1 1. (a) Deduce the number of protons, neutrons and electrons in the following species: (i) 37 Cl - (ii) 1 H + (iii) 45 Sc 3+ (b) Write symbols for the following species: (i) 8 protons, 8 neutrons,
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationC4 Quick Revision Questions
C4 Quick Revision Questions H = Higher tier only SS = Separate science only Question 1... of 50 Write the equation which shows the formation of iron oxide Answer 1... of 50 4Fe + 3O 2 2Fe 2 O 3 Question
More informationAtoms, Elements, Atoms, Elements, Compounds and Mixtures. Compounds and Mixtures. Atoms and the Periodic Table. Atoms and the.
Atoms, Elements, Compounds and Mixtures Explain how fractional distillation can be used to separate a mixture. 1 Atoms, Elements, Compounds and Mixtures Fractional distillation is used to separate components
More informationQuestions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:..
Level 3 Applied Science UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION Questions Booklet Name:.. Teacher:.. Level 3 Applied Science 2017-2018 Unit 1 (Chemistry) 1 1. State the relative
More informationYear 12 Chemistry Transition Work - QPHS
Year 12 Chemistry Transition Work - QPHS Contents Task 1: Task 2 Task 3 Task 4 Task 5 Task 6 Task 7 Task 8 The structure of atoms Writing formulae Relative masses Balancing equations Writing symbol equations
More informationPractice I: Chemistry IGCSE
Practice I: Chemistry IGCSE cristian.obiol@gmail.com 1) Explain the following processes related to changes of states of matter. -Melting:... -Vaporization:... -Freezing:... -Condensation:... -Sublimation:...
More informationName... Requirements for the task and Chemistry lessons
Name... HAUTLIEU SCHOOL CHEMISTRY Pre AS and IB Diploma Task Expectations All sections of the task will be attempted please check you have answered all questions (even those on the back page) Answers should
More informationQ1. As the world population increases there is a greater demand for fertilisers.
Q1. As the world population increases there is a greater demand for fertilisers. (a) Explain what fertilisers are used for............. (b) The amount of nitrogen in a fertiliser is important. How many
More informationTHE BRIDGING COURSE TO SIXTH FORM CHEMISTRY AT Myton School
THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY AT Myton School Introduction Before you start the AS Chemistry course in September you should have completed this new bridging course for Chemists. It has been
More informationmohd faisol mansor/chemistry form 4/chapter 7 CHAPTER 7 ACIDS AND BASES HCl (g) H 2 O H + (aq) + Cl - (aq) NaOH(s) H 2 O Na + (aq) + OH - (aq)
CHAPTER 7 ACIDS AND BASES Arrhenius Theory An acid is a chemical compound that produces hydrogen ions, H + or hydroxonium ions H3O + when dissolve in water. A base defined as a chemical substance that
More informationRevision Checklist :4.3 Quantitative Chemistry
Revision Checklist :4.3 Quantitative Chemistry Conservation of Mass The law of conservation of mass states that no atoms are lost or made during a chemical reaction so the mass of the products equals the
More informationTHE BRIDGING COURSE TO SIXTH FORM CHEMISTRY Birchwood High School
THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY Birchwood High School Mrs Ryan Chemistry Please also access the website below which is a link to a really good PPT that will help to bridge the gap between GCSE
More informationF321: Atoms, Bonds and Groups Structure & Bonding
F321: Atoms, Bonds and Groups Structure & Bonding 1. This question is about different models of bonding and molecular shapes. Magnesium sulfide shows ionic bonding. What is meant by the term ionic bonding?
More informationGCSE (9 1) Combined Science (Chemistry) A (Gateway Science) J250/09 Paper 9, C1 C3 and CS7 (PAGs C1 C5)
Oxford Cambridge and RSA GCSE (9 1) Combined Science (Chemistry) A (Gateway Science) Paper 9, C1 C3 and CS7 (PAGs C1 C5) (Higher Tier) Year 11 Test Time allowed: 1 hour 10 minutes H You must have: a ruler
More informationSpring Semester Final Exam Study Guide
Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous
More informationComplete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion.
1 This question is about the elements with atomic numbers between 58 and 70 (a) Cerium, atomic number 58, is a metal Complete the table to show the relative charge of each particle and the number of each
More information1.24 Calculations and Chemical Reactions
1.24 Calculations and Chemical Reactions Converting quantities between different substances using a balanced equation A balanced chemical equation tells us the number of particles of a substance which
More informationF321: Atoms, Bonds and Groups Acids
F321: Atoms, Bonds and Groups Acids 49 Marks 1. A student carries out experiments using acids, bases and salts. Calcium nitrate, Ca(NO 3 ) 2, is an example of a salt. The student prepares a solution of
More informationWrite the ionic equation for this neutralisation reaction. Include state symbols.
Q1.Sodium hydroxide neutralises sulfuric acid. The equation for the reaction is: 2NaOH + H 2 SO 4 Na 2 SO 4 + 2H 2 O (a) Sulfuric acid is a strong acid. What is meant by a strong acid? (b) Write the ionic
More informationNATIONAL 5 CHEMISTRY
Farr High School NATIONAL 5 CHEMISTRY Unit 1 Chemical Changes and Structure Question Booklet 1 Rates of Reaction 1. Explain how the following would affect the rate of the reaction between 1.0 g of magnesium
More informationPart 7- Quantitative Chemistry Application Questions Triple Science
Part 7- Quantitative Chemistry Application Questions Triple Science How bonding and structure are related to the properties of substances A simple model of the atom, symbols, relative atomic mass, electronic
More informationThe drawing shows a container of a compound called magnesium chloride. How many elements are joined together to form magnesium chloride?
Bonding part 5 Q1. The drawing shows a container of a compound called magnesium chloride. How many elements are joined together to form magnesium chloride? Magnesium chloride is an ionic compound. What
More informationStoichiometry Part 1
Stoichiometry Part 1 Formulae of simple compounds Formulae of simple compounds can be deduced from their ions/valencies but there are some that you should know off by heart. You will learn these and more
More informationAngel International SchoolManipay
Grade OL Angel International SchoolManipay 2 nd Term Examination March, 2016 Chemistry Duration: 3 Hours 1. Which property is common to calcium, potassium and sodium? a) Their atoms all lose two electrons
More informationQuantitative Chemistry
Quantitative Chemistry When we do experiments to measure something in Chemistry, we: Repeat experiments (usually 3 times) to improve the reliability of the results, by calculating an average of our results.
More informationA Level Chemistry. Ribston Hall High School. Pre Course Holiday Task. Name: School: ii) Maths:
A Level Chemistry Ribston Hall High School Pre Course Holiday Task Name: School: GCSE Grades in i) Chemistry or Science: ii) Maths: 1 The following are a series of questions on topics you have covered
More information2 Answer all the questions.
2 Answer all the questions. 1 A sample of the element boron, B, was analysed using a mass spectrometer and was found to contain two isotopes, 10 B and 11 B. (a) (i) Explain the term isotopes. Complete
More information4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
More informationName: C4 TITRATIONS. Class: Question Practice. Date: 97 minutes. Time: 96 marks. Marks: GCSE CHEMISTRY ONLY. Comments:
C4 TITRATIONS Question Practice Name: Class: Date: Time: 97 minutes Marks: 96 marks Comments: GCSE CHEMISTRY ONLY Page of 3 Sodium hydroxide neutralises sulfuric acid. The equation for the reaction is:
More informationCHEMICAL EQUATIONS WHAT BALANCING AN EQUATION MEANS
17 CHEMICAL EQUATIONS WHAT BALANCING AN EQUATION MEANS WHAT IS A CHEMICAL EQUATION? A chemical equation is a way of representing a chemical reaction in symbolic form. For example, when hydrochloric acid
More informationC2.6 Quantitative Chemistry Foundation
C2.6 Quantitative Chemistry Foundation 1. Relative masses Use the periodic table to find the relative masses of the elements below. (Hint: The top number in each element box) Hydrogen Carbon Nitrogen Oxygen
More information2 Answer all the questions. How many neutrons are there in an atom of chlorine-37?... [1] How many electrons are needed to fill one orbital?
2 Answer all the questions 1 The answer to each part of this question is a number (a) (i) How many neutrons are there in an atom of chlorine-37? [1] (ii) How many electrons are needed to fill one orbital?
More informationChemical measurements QuestionIT
Chemical measurements QuestionIT 1. What is the law of conservation of mass? Mass of reactants = mass products. 2. Why might some reactions appear to show a change in mass? A reactant or a product is a
More informationA LEVEL CHEMISTRY PRE-COURSE MATERIALS AND NOTES
A LEVEL CHEMISTRY PRE-COURSE MATERIALS AND NOTES Name: Submission Deadline: Friday 8 th September 2017 Dear Student Welcome to A level Chemistry. A level Chemistry involves the study of substances and
More informationSecondary School, Kirkop
KULLEĠĠ SAN BENEDITTU Secondary School, Kirkop Mark HALF YEARLY EXAMINATION 2017/18 Level: 5,6,7,8 YEAR 9 Chemistry TIME: 2 hours Question 1 2 3 4 5 6 7 8 9 Global Mark Max. Mark 12 6 12 7 14 9 20 20 20
More informationNational 5 Chemistry. Unit 1 Chemical Changes and Structure Summary Notes
National 5 Chemistry Unit 1 Chemical Changes and Structure Summary Notes Success Criteria I am confident that I understand this and I can apply this to problems? I have some understanding but I need to
More informationWrite down everything that the word equation tells you about the reaction (Total 4 marks)
Q1. Here is a word equation for a chemical reaction. copper oxide + sulphuric acid copper sulphate + water Write down everything that the word equation tells you about the reaction.......... (Total 4 marks)
More informationSCIENCE JSUNIL TUTORIAL CLASS 9. Activity 1
Activity Objective To understand, that there is a change in mass when a chemical change takes place. (To understand law of conservation of mass experimentally). Procedure. Take one of the following sets,
More informationAnswers for UNIT ONE NAT 5 Flash Cards
Answers for UNIT ONE NAT 5 Flash Cards 1. (a) rate increases (b) rate increases (c) rate increases (d) rate increases 2. Average rate = change in property / change in time Where property = concentration,
More informationFormulae and Equations
Formulae and Equations 1 of 41 Boardworks Ltd 2016 Formulae and Equations 2 of 41 Boardworks Ltd 2016 Forming different compounds 3 of 41 Boardworks Ltd 2016 Elements are made up of just one type of atom.
More informationAQA Chemistry GCSE. Topic 3: Quantitative Chemistry. Flashcards.
AQA Chemistry GCSE Topic 3: Quantitative Chemistry Flashcards What is the law of conservation of mass? What is the law of conservation of mass? The law of conservation of mass states that no atoms are
More informationBullers Wood School. Chemistry Department. Transition to A Level Chemistry Workbook. June 2018
Bullers Wood School Chemistry Department Transition to A Level Chemistry Workbook June 2018 This booklet contains questions for you to work through and answer over the summer to prepare for the A level
More informationCombined Science Chemistry Academic Overview
Combined Science Chemistry Academic Overview 2018-2019 Science Term 1.1 Term 1.2 Term 2.1 Term 2.2 Term 3.1 Term 3.2 Year 9 States of Matter Methods of Separating and Purifying Substances Atomic Structure
More informationWorksheet 2.1: Pre-check
Worksheet 2.1: Pre-check Complete these questions to check your understanding of some of the basic skills and ideas you will learn about. 1 Understanding matter and energy a If a single atom of an element
More informationLondon Examinations IGCSE
Centre No. Candidate No. Paper Reference 4 3 3 5 2 H Paper Reference(s) 4335/2H London Examinations IGCSE Chemistry Paper 2H Higher Tier Wednesday 21 May 2008 Afternoon Time: 2 hours Surname Signature
More informationClass IX Chapter 3 Atoms and Molecules Science
Class IX Chapter 3 Atoms and Molecules Science Question 1: In a reaction, 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of
More informationA-LEVEL TRANSITION COURSE SUMMER 2018 PART 2: USING CHEMICAL EQUATIONS
A-LEVEL TRANSITION COURSE SUMMER 2018 PART 2: USING CHEMICAL EQUATIONS MASS AQUEOUS VOLUME ` MOLAR MASS GASEOUS VOLUME MOLES CONCENTRATION REVISION FROM LESSON 1 How many moles? 1) Jahin weighs a sample
More informationUnit 5 A3: Energy changes in industry
1. ENTHALPY CHANGES Unit 5 A3: Energy changes in industry 1.1 Introduction to enthalpy and enthalpy changes 2 1.2 Enthalpy profile diagrams 2 1.3 Activation energy 3 1.4 Standard conditions 5 1.5 Standard
More informationGCSE Chemistry 3 Summary Questions
GCSE Chemistry 3 Summary Questions Q1 Q2 Q3 Q4 Q5 Q6 Q7 Q8 Q9 Q10 Q11 Q12 Q13 Q14 Q15 Q16 Q17 Q18 Q19 C3.1.1 The early Periodic table (p73) Explain Newlands law of Octaves. Explain why Newlands law was
More informationPaper Reference. Sample Assessment Material Time: 2 hours
Centre No. Candidate No. Paper Reference(s) 4CH0/1C Edexcel IGCSE Chemistry Chemistry Paper 1 Sample Assessment Material Time: 2 hours Materials required for examination Nil Items included with question
More informationEdexcel Chemistry Checklist
Topic 1. Key concepts in chemistry Video: Atomic Structure Recall the different charges of the particles that make up an atom. Describe why atoms have no overall charge. Use the periodic table to identify
More informationEdexcel Chemistry Checklist
Topic 1. Key concepts in chemistry Video: Developing the atomic model Describe how and why the atomic model has changed over time. Describe the difference between the plum-pudding model of the atom and
More informationPersonalised Learning Checklists AQA Chemistry Paper 1
AQA Chemistry (8462) from 2016 Topics C4.1 Atomic structure and the periodic table State that everything is made of atoms and recall what they are Describe what elements and compounds are State that elements
More informationDraw one line from each solution to the ph value of the solution. Solution ph value of the solution
1 The ph scale is a measure of the acidity or alkalinity of a solution. (a) Draw one line from each solution to the ph value of the solution. Solution ph value of the solution 5 Acid 7 9 Neutral 11 13
More informationMoles, calcula/ons in gaseous and solu/on and acids and bases
Moles, calcula/ons in gaseous and solu/on and acids and bases Moles and calcula/ons 1 Objec/ves All Define rela/ve molecular mass and rela/ve formula mass Most Describe Avogadro s constant and the terms
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More informationAnswer all questions in the spaces provided. 1 The diagrams show the sub-atomic particles in four different atoms.
2 Answer all questions in the spaces provided. 1 The diagrams show the sub-atomic particles in four different atoms. Atom A Atom B Atom C Atom D Use the Chemistry Data Sheet to help you to answer these
More informationYear 10 Chemistry Exam June 2011 Multiple Choice. Section A Mulltiple Choice
Year 10 Chemistry Exam June 2011 Multiple Choice Section A Mulltiple Choice 1. An aqueous solution is obtained when: a. a substance dissolves in any liquid b. a substance is dissolved in water c. when
More informationThe photograph in the textbook provides evidence that an exothermic chemical reaction is occurring.
Preview Lesson Starter Objectives Indications of a Chemical Reaction Characteristics of Chemical Equations Significance of a Chemical Equation Balancing Chemical Equations Section 1 Describing Chemical
More informationChapter 5 Chemical Calculations
Calculating moles Moles and elements Moles and compounds Moles and gases Moles and solutions Calculating formulae Finding the formula Chapter 5 Chemical Calculations Moles and chemical equations Checklist
More informationD. Ammonia can accept a proton. (Total 1 mark)
1. Which statement explains why ammonia can act as a Lewis base? A. Ammonia can donate a lone pair of electrons. B. Ammonia can accept a lone pair of electrons. C. Ammonia can donate a proton. D. Ammonia
More informationDescribe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. ... [3] ...
3 Gallium is a metallic element in Group III. It has similar properties to aluminium. (a) (i) Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer.
More informationBridging the Gap between GCSE and A level Chemistry
Bridging the Gap between GCSE and A level Chemistry You should use your GCSE revision guide and your class notes to complete the following questions You can check your answers at the end of the power point,
More informationChemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions
Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In
More informationAdditional Science. Chemistry CH2FP. (Jun15CH2FP01) General Certificate of Secondary Education Foundation Tier June 2015.
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials Question Mark Additional Science Unit Chemistry C2 Chemistry Unit Chemistry C2 Thursday 14
More informationGraspIT AQA GCSE Chemical and Energy Changes
A. Reactivity of metals The reactivity series, metal oxides and extractions 1. Three metals, X, Y and Z were put into water. The reactions are shown below: a) Use the diagrams to put metals X, Y and Z
More informationIB Chemistry Solutions Gasses and Energy
Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.
More informationOCR unit 5 revision booklet
OCR unit 5 revision booklet Moles and Molar Mass One mole of any substance contains 6x10 23 particles. For example a mole of carbon atoms would contain 10 x 10 23 carbon atoms. To calculate mole of a substance
More informationChemical Bonds In elements and compounds, the atoms are held together by chemical bonds.
Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they are able to. Bonds are made using
More information... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3
1 Chemists have developed models for bonding and structure which are used to explain different properties. (a) Ammonia, NH 3, is a covalent compound. Explain what is meant by a covalent bond. Draw a dot-and-cross
More informationA student wanted to make 11.0 g of copper chloride
Q1.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
More informationThe following activities and resources will help prepare you to start an A level Chemistry in September at St Joseph s College.
The following activities and resources will help prepare you to start an A level Chemistry in September at St Joseph s College. It is aimed to be used after you complete your GCSE, throughout the remainder
More informationTopic 1.2 AMOUNT OF SUBSTANCE
Topic 1.2 AMOUNT OF SUBSTANCE The mole Reacting masses and atom economy Solutions and titrations The ideal gas equation Empirical and molecular formulae Ionic equations Mill Hill County High School THE
More information(a) Bleach can be made by reacting chlorine with cold aqueous sodium hydroxide. A solution of bleach contains the chlorate compound NaClO. ...
1 The chlor-alkali industry is an important part of the UK chemical industry. The raw material is brine, a concentrated aqueous solution of sodium chloride, NaCl(aq). Two products that can be manufactured
More information2) Solve for protons neutrons and electrons for the bromide ION.
1) Write the formulas for the following a) Calcium nitride c)lithium hydroxide b) Iron (III) sulfide d) sulfuric acid 2) Solve for protons neutrons and electrons for the bromide ION. 3) Write the electron
More information3. Which postulate of Dalton s atomic theory is the result of the law of conservation of mass?
1 1. In a reaction, 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of sodium ethanoate. Show that these observations are in
More informationfor sodium ion (Na + )
3.4 Unit 2 Chemistry 2 Throughout this unit candidates will be expected to write word equations for reactions specified. Higher tier candidates will also be expected to write and balance symbol equations
More information3 rd Year Revision. (from second year: Conservation of Mass Acids, Alkalis and Indicators)
3 rd Year Revision (from second year: Conservation of Mass Acids, Alkalis and Indicators) To revise: Elements, compounds, mixtures. Periodic table names (eg groups, periods, transition metals, alkali metals,
More informationPHYSICAL SCIENCES: PAPER II
NATIONAL SENIOR CERTIFICATE EXAMINATION NOVEMBER 2017 PHYSICAL SCIENCES: PAPER II Time: 3 hours 200 marks PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY 1. This question paper consists of 19 pages, a
More informationFACTFILE: GCSE CHEMISTRY: UNIT 2.6
FACTFILE: GCSE CHEMISTRY: UNIT Quantitative Chemistry Learning outcomes Students should be able to:.1 calculate the concentration of a solution in mol/dm 3 given the mass of solute and volume of solution;.2
More informationSNC2D1: Grade 10 Academic Science
SNC2D1: Grade 10 Academic Science Chemistry Test date: Monday, March 24 Study tips: apple Read through your notes apple Make point form notes to summarize the topics apple Complete the review sheet apple
More informationC2.6 Quantitative Chemistry Foundation
C2.6 Quantitative Chemistry Foundation 1. Relative masses Use the periodic table to find the relative masses of the elements below. (Hint: The top number in each element box) Hydrogen Carbon Nitrogen Oxygen
More informationC1 REVISION 5.1 Atomic Structure
C1 REVISION 5.1 Atomic Structure Draw the symbol for sodium include its mass number and atomic number (what do they tell us) Complete the table Relative Charge Relative Mass Balance the following equation:
More informationReview Chemistry Paper 1
Atomic Structure Topic Define an atom and element. Use scientific conventions to identify chemical symbols Identify elements by chemical symbols Define compound Use chemical formulae to show different
More informationUnit 5 Part 1 Acids, Bases and Salts Properties of Acids, Bases and Salts UNIT 5 ACIDS, BASES AND SALTS PART 1 PROPERTIES OF ACIDS, BASES AND SALTS
UNIT 5 ACIDS, BASES AND SALTS PART 1 PROPERTIES OF ACIDS, BASES AND SALTS Contents 1. Acids, Bases, Salts and Neutralisation 2. Physical Properties of Acids, Bases and Salts 3. Strong and Weak Acids and
More informationF321: Atoms, Bonds and Groups Moles and Equations
F321: Atoms, Bonds and Groups Moles and Equations 108 Marks 1. (a) A student carries out a titration to find the concentration of some sulfuric acid. The student finds that 25.00 cm 3 of 0.0880 mol dm
More informationTransition Pack for A Level Chemistry
Transition Pack for A Level Chemistry Get ready for A-level! A guide to help you get ready for A-level Chemistry, including everything from topic guides to days out and online learning courses. Commissioned
More informationIB Topics 5 & 15 Multiple Choice Practice
IB Topics 5 & 15 Multiple Choice Practice 1. Which statement is correct for this reaction? Fe 2O 3 (s) + 3CO (g) 2Fe (s) + 3CO 2 (g) ΔH = 26.6 kj 13.3 kj are released for every mole of Fe produced. 26.6
More informationNCERT Solutions for Atoms and Molecules
1 NCERT Solutions for Atoms and Molecules Question 1. In a reaction, 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of sodium
More informationPRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE
PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE 1. Nitroglycerine, C 3 H 5 N 3 O 9, is an explosive which, on detonation, decomposes rapidly to form a large number of gaseous molecules. The
More information