Set 1 Structure of the atoms & Chemical Equation Perfect Score F Matter is anything that. and has.

Size: px
Start display at page:

Download "Set 1 Structure of the atoms & Chemical Equation Perfect Score F Matter is anything that. and has."

Transcription

1 STRUCTURE OF THE ATOMS 1. Matter is anything that. and has. 2. The particle theory of matter state that matter is.. 3. Type of particle Example 4. Property Solid Liquid Gas Diagrammatic representation of the particles in each of the physical states Arrangement of particles. Forces of attraction between particles Movement of particles Energy content 5. Subatomic particles in an atom. Subatomic particle Symbol Relative mass Charge 6. Isotope are atoms with the same but different. 7. The isotopes of an element have same... but different because they have. 8. Compare and contrast the atoms below. 12 C 6 14 C 6 1

2 9. Complete the table below. Isotope Carbon-14 Uses Cobalt-60 Sodium-24 PAPER 2 : STRUCTURE 1. (a) Diagram 1.1 shows the results of an experiment to investigate the movement of bromine particles in air. Diagram 1.1 Air Bromine vapour Gar jar Cover Cover removed Reddish brown vapour spreads throughout both gas jars within 10 minutes (i) (ii) State the name of the process involved in this experiment State the type of particles present in bromine gas.... (iii) Explain the observation in this experiment based on the kinetic theory of matter [3 marks] 2

3 Temperature Diagram R T Time, s Diagram 1.2 shows a graph of temperature against time when solid X is heated? (i) State the melting point of X. (ii) (iii)... What happens to the temperature while the substance changes state? Explain Explain the movement of particles X between R and T during heating Glass wool soaked in concentrated ammonia solution Diagram 2 2. Diagram 2 shows the set-up of apparatus to investigate the reaction between concentrated hydrochloric acid and concentrated ammonia solution to form substance X. Based on the information, answer the following questions. (a) (i) What is the observation in the glass tube? Glass wool soaked in concentrated hydrochloric acid... 3

4 (ii) Name substance X (iii)..... Name the process occurs in the glass tube Which gas diffused faster? Why? Write the chemical equation for the reaction in the experiment Table 3 shows proton number and nucleon number for atom W, X and Y. Atom Proton number Nucleon number W X Y Table 3 (a) (i) What is meant by proton number? (ii) What is the number of neutron in atom W? Which atoms are isotopes? Explain why Write the electron arrangement of atom X [1mark] 4

5 (d) (i) Draw the electron arrangement of atom Y. In your diagram, show the number of proton and the number of neutron in the nucleus. (ii) What is the number of valence electron of atom Y?... (iii) Write the formula of ion Y.... (e) Write the symbol of atom X in the form of A Z X (a) Diagram 4.1 shows the set-up of an experiment to determine the melting point of solid X. Thermometer Water Diagram 4.1 The temperature of X is recorded at 30 seconds intervals as shown below. Time/second Temperature/ o C (i) Plot the graph of temperature against time for the heating of X on the graph paper. [3 marks] 5

6 Graph temperature against time 6

7 (ii) On the graph that you have drawn in (a), label the melting point of substance X. (iii) Explain why the temperature remains constant from 60 s to 120 s?.... (iv)... Draw the arrangement of particles in X at 85 o C [ 1 mark ] Why has the solid X in the boiling tube be stirred constantly with the thermometer during the experiment?... Why solid X is not directly heated without using water bath? Table 5 shows four substances and their respective formulae. Substance Chemical formula Iodine I 2 Copper Cu Ethanol C 2 H 5 OH Potassium chloride KCl Table 5 (a) (d) State 2 substances that consist of molecules.... Which of the following substances has a highest melting point?... State the substance that can conduct electricity in the solid state.... Name the particles present in potassium chloride.... 7

8 PAPER 2 : ESSAY 6. Diagram 6.1 shows an atom of an element based on the model by James Chadwick. Electron Proton Diagram 6.1 Neutron (a) Compare the relative mass and the charge of two of the subatomic particles in diagram 6.1. [4 marks] 7p 7n Diagram 6.2 Diagram 6.2 shows an atom of element X. (i) Describe fully the atomic structure shown in diagram 7.2. [4 marks] (ii) Write a symbol for the element in the form of Graph 6.3 shows the heating curve of element Y. A Z X Temperature / o C Melting point Graph 6.3 t o t 1 t 2 t 3 Time, minutes Describe the graph in term of states of matter, particles arrangements and changes in energy. [10 marks] 8

9 7 (a) What is meant by melting point? During the melting of naphthalene, the temperature remains constant even though heat is applied. Explain why. Condensation is the process where a gas changes to its liquid state at a certain temperature and pressure when it is cooled. [4 marks] Describe the change of the kinetic energy, arrangement and the forces of attraction between the particles at the following states: (i) Before condensation (ii) During condensation (iii) After condensation Diagram 7 shows the electron arrangement of ion Y 3+. [10 marks] e e e e e 14 n e e e e e 3+ n neutron e electron Diagram 7 (i) Calculate the nucleon number of atom Y. (ii) Y reacts with oxygen to form oxide Y, with the formula Y 2 O 3. The chemical equation for reaction Y with oxygen is show as: 4Y + 3O 2 2Y 2 O 3. Given that the relative atomic mass of Y = 27 and O = 16. Calculate the mass of oxide Y, Y 2 O 3 formed when 10.8 g Y is completely burnt in oxygen. PAPER 3 : STRUCTURE [4 marks] Gas jar cover Gas jar Bromine vapour Water Potassium manganate(vii) Jelly A B C Diagram 8 9

10 8. A group of students set up the apparatus for an experiment as shown in diagram 8. The result is obtained by the students are shown in table 8. Experiment A B C Observation After a few minutes the gar jar was filled with a reddish brown gas. After a few hours, the water turns purple. After a few days, the jelly turns purple. (a) State the aim of the experiments carried out.... State the hypothesis of the experiments State (i) (ii) (iii) The manipulated variable.... The responding variable.... The fixed variable of the experiments.... (d) (e) Based on the observation, arrange the three states of mater in a sequence to show their speed in increasing order.... Based on the rate of the movement of the particles, describe the arrangement of the particles in the three states of matter (f) Give the daily application of the process in one of the above experiment

11 CHEMICAL FORMULA AND EQUATION 1. Write the chemical formula of the compound in the table below. Ion Chloride Nitrate Hydroxide Sulphate Carbonate oxide Sodium Magnesium Lead(II) Copper (II) Iron (II) Iron (III) Aluminium 2. Write balanced chemical equation for the following chemical reactions. (a) Heat solid of copper (II) carbonate (d) (e) (f). Nitric acid reacts with sodium hydroxide. Hydrochloric acid reacts with zinc metal. Copper(II)nitrate reacts with magnesium. Chlorine gas reacts with lithium hydroxide. Hydrogen gas reacts with lead(ii) oxide. 3. Avogadro constant, N A is defined as the number of particles in one mole of a substance [1 Mol any substance consist of 6.02 X particles]. Calculate the number of particles in: (a) 0.1 mol of calcium 1.5 mol of iron 2.0 mol of oxygen gas (d) 1.5 mol of helium (e) 2.0 mol hydrogen chloride 11

12 4. Calculate the number of moles of the following substances. (a) 6.0 x aluminium 1.8 x argon 1.2 x bromine gas (d) 2.4 x carbon dioxide (e) 3.0 x ammonia 5. Calculate the mass of following substances. a) 1.5 mol of chlorine gas b) 2.5 moles of oxygen gas c) 2.0 moles of sulphuric acid d) 0.5 moles of ammonia, NH 3 e) 2.5 moles of lead (II) carbonate f) 0.5 moles copper(ii) nitrate, Cu(NO 3 ) 2 Molar volume: The volume of one mole of the gas [22.4 dm 3 mol -1 at STP, standard temperature and pressure] [24 dm 3 mol -1 at Room condition] 6. Calculate the volume of gases below. (a) 0.5 mol of chlorine at STP. 0.2 mol of carbon dioxide at Room condition. 1.5 mol of methane at room condition. (d) 0.5 mol of helium at room condition. (e) 2.5 mol of ammonia at STP 12

13 7. Calculate the number of moles of the gases below. (a) 250 cm 3 of carbon dioxide in room temperature. 500 cm 3 of hydrogen sulfide at STP. 200 cm 3 of hydrogen chloride in room temperature. (d) 750 cm 3 of neon in room temperature. (e) 300 cm 3 of ammonia at STP. 8. Magnesium powder reacts with hydrochloric acid to produce salt and hydrogen gas. (a) Write the balance chemical equation for this reaction.. If 2.4 g of magnesium powder is added into excess hydrochloric acid, calculate, (i) The mass of salt formed. (ii) The volume of hydrogen gas liberated at room temperature. 9. Lead is extracted according to the following equation. C + PbO CO 2 + Pb (a) Write the balanced chemical equation for the reaction. Determine the number of moles of lead extracted from 0.5 mole of lead (II) oxide. Calculate the number of moles of carbon required to extracts 0.5 mole of lead(ii) oxide. (d) What is the mass of lead are produced if 44.6 g of lead (II) oxide is heated with excess carbon. [ RAM : Pb = 207, O = 16, C = 12 ] 13

14 10. Excess sodium carbonates is added into 50 cm 3 of 0.5 mol dm -3 copper(ii) chloride. The chemical equation for the reaction is as follows: CuCl 2 + Na 2 CO 3 NaCl + CuCO 3 (a) Balance the chemical equation for the reaction. Calculate the mass of copper(ii)carbonate g of calcium carbonate is added to excess hydrochloric acid. (a) Write balanced chemical equation for the reaction... Determine the volume of carbon dioxide gas evolved at room temperature 12. When sodium bicarbonate is heated, it decomposed to sodium carbonate, carbon dioxide and water. (a) Write a balanced chemical equation for the decomposition of sodium bicarbonate on heating.... If 8.4 g of sodium bicarbonate decomposes, calculate (i) The volume of carbon dioxide gas evolved at room temperature. (ii) The mass of sodium carbonate formed. 14

15 Concentration of acids and alkalis (STOICHEIOMETRY) The concentration of a solution is the mass (in gram) or the number of mole of solute dissolved in a solvent to form 1.00 dm 3 of solution. Concentration, g dm -3 Concentration, mol dm -3 / molarity Mass of solute, g Volume of solution, dm 3 Number of mole of solute, mol Volume of solution, dm 3 Titration Formula M a V 2 = a b MbVb M a = Concentration of the acid, M b = Concentration of the alkali V a = Volume of used acid, V b = Volume of used alkali a = the number of mole of acid, b = the number of mole of alkali Dilution M 1 V 1 = M 2 V cm 3 of HCl 2.0 mol dm -3 reacts completely with excessive zinc powder. Calculate the volume of gas released at room temperature? (Molar volume = 24 dm 3 at room temperature) g of Calcium carbonates dissolves in 100 cm 3 of nitric acid 0.5 mol dm -3 to produce salt, carbon dioxide gas and water. (i) Write out the equation... (ii) Calculate the moles of calcium carbonates used. (RAM Ca =40, C = 12, O = 16). (iii) Calculate the moles of acid. (iv) Calculate the volume of gas produced. 15

16 15. X g sodium carbonate reacts completely with 100 cm 3 hydrochloric acid 1.0 moldm -3 to produce sodium chloride, carbon dioxide and water. Find X. (relative atomic mass: Na =23, C = 12, O = 16) g of copper(ii) oxide reacts completely with 100 cm 3 hydrochloric acid to form copper(ii) chloride and water. Calculate the molarity of acid used. (JAR Cu =64, O = 16 ) 17. The concentration of sodium hydroxide solution is 8.0 g dm -3. (a) What is the molarity of the solution? What is the molarity of the solution produced when 100 cm 3 of distilled water is added to 50 cm 3 of this solution? 18. In the titration experiment, 25.0 cm 3 of 2.0 mol dm -3 sodium hydroxide solution is titrated with sulphuric acid from a burette cm 3 of sulphuric acid is needed for complete neutralization. (a) Write a balanced chemical equation for the neutralization. Calculate the number of mole of sodium hydroxide used in this experiment. Calculate the number of moles of sulfphuric acid needed to exactly neutralize 25.0 cm 3 of 2.0 mol dm - 3 sodium hydroxide. (d) Calculate the molarity of sulphuric acid mol dm -3 hydrochloric acid reacts completely with 25.0 cm 3 of 1.0 mol dm -3 sodium carbonate. (a) Write a balanced chemical equation for this reaction. Calculate the number of mole of sodium carbonate used in this experiment. Calculate the volume of hydrochloric acid needed to exactly neutralize 25.0 cm 3 of 1.0 mol dm -3 sodium carbonate. 16

17 PAPER 2: STRUCTURE 1. Diagram 1 shows the set-up of the apparatus for an experiment to determine the empirical formula of an oxide of copper. Oxide of copper Dry hydrogen gas Heat Diagram 1 Table 1 shows the results of an experiment after heating, cooling and weighing are repeated until a constant weight is obtained. Substance Mass of combustion tube + porcelain dish Mass of combustion tube + porcelain dish + oxide of copper Mass of combustion tube + porcelain dish + copper Mass(g) g g g (a) What is meant by empirical formula? Table 1... Based on Table 5 results, (i) Calculate the mass of copper and the mass of oxygen used in the experiment. (ii) Calculate the mole ratio of copper atoms to oxygen atoms. Given that the relative atomic mass of Cu, 64; O,16. (iii) State the empirical formula of this oxide of copper. (iv). Write the chemical equation for the reaction in this experiment

18 Describe the steps that should be taken to ensure that all the air in the combustion tube has been expelled, before any heating is carried out [3 marks] 2. (a) Culculate the relative molecular or formula masses of the following substances. (i) Ethanol, C 2 H 5 OH. Given that relative atomic mass of H = 1, C = 12, O = 16. (ii) Zinc nitrate, Zn(NO 3 ) 2 Given that relative atomic mass of O = 16, N = 14, Zn = 65. A closed glass bottle contains 4 mol molecules of oxygen, O 2. (i) What is the number of oxygen molecules in the bottle? (ii) How many oxygen atoms are there in the bottle? Find the number of moles of atoms in a sample containing atoms of copper. (d) Calculate the mass, in gram, of 3.5 moles of copper(ii) carbonate, CuCO 3. Given that relative formula mass of CuCO 3 = 124 (e) When silver carbonate, Ag 2 CO 3 is heated, it will decompose to produce silver metal, carbon dioxide gas and oxygen gas as shown in the equation below. 2Ag 2 CO 3 (s) 4Ag(s) + 2CO 2 (g) + O 2 (g) 18

19 A student heats 8.28 g silver carbonate. Calculate the volume of carbon dioxide gas, CO 2 collected at room temperature. Given that relative atomic mass of C = 12, O =16, Ag = 108, 3. Diagram 3 shows 3.1 g of copper (II) carbonate being heated strongly in attest tube. The gas given out is passed into limewater in a test tube through a delivery tube. [3 marks] Copper(II) carbonate Heat strongly Lime water Diagram 3 (a) State the observation made when copper(ii)carbonate powder is heated until the reaction is complete. Write the chemical equation to represent the reaction that takes place.. Calculate the number of moles of copper(ii)oxide produced. (d) Calculate the volume of gas produced at STP. (e) (i) What can be observed if the product is heated in a stream of hydrogen gas? (ii).. Calculate the mass of the substance produced. 19

20 PAPER 2 : ESSAY 4. (a) The information below is regarding substance X Carbon 85.70% Hydrogen 14.30% Relative molecular mass = 56 (i) Determine the empirical formula of substance X. [Given that the relative atomic mass of C = 12, H = 1] (ii) Determine the molecular formula of substance X. (iii) Based on the answers in (a)(i) and (a)(ii), compare and contrast the empirical formula and the molecular formula. [ 8 marks] Magnesium can react actively with oxygen to form magnesium oxide. Describe an activity that can be carried out in the laboratory to determine the empirical formula of magnesium oxide. Include the calculations involved in your answer. Given that the relative atomic mass for O = 16, Mg = 24. [11 marks] 20

21 PAPER 3 : STRUCTURE 5. A student carried out an experiment to determine the empirical formula of magnesium oxide. The steps and set-up of apparatus of the experiment are shown in Diagram The crucible and lid are weighed. lid crucible g digital balance 2. The crucible, lid and magnesium powder are weighed g Magnesium powder 3. The magnesium powder is heated until it reacts completely with oxygen. white fumes heat 4. The crucible, lid and magnesium oxide are weighed when cooled g magnesium oxide powder Diagram 5 21

22 (a) Complete the following table by stating the observations and related inferences in the experiment. Observations (i) Inferences (i) (ii) (iii) ) (ii) (iii) Round off the reading to two decimal places and record it in the table below. [6 marks] The crucible and lid. Description Mass / g The crucible, lid and magnesium powder. The crucible, lid and magenesium oxide. (i) Calculate the mass of magnesium that has been used. (ii) Calculate the mass of oxygen which reacted with magnesium. (iii) Determine the empirical formula of magnesium oxide. Use the information that the relative atomic mass, O = 16, Mg = 24 (d) The student wants to determine the empirical formula of lead(ii) oxide. He used the steps and set-up of apparatus as the experiment before. Predict whether the empirical formula of lead(ii) oxide can be determined. Explain your answer

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. 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 information

Set 1 Marking Scheme: The Structure of the Atom & Chemical Equation Question Explanation Marks

Set 1 Marking Scheme: The Structure of the Atom & Chemical Equation Question Explanation Marks Set Marking Scheme: The Structure of the Atom & Chemical Equation 200 THE STRUCTURE OF THE ATOMS PAPER 2 : STRUCTURE Question Explanation Marks (a)(i) Diffusion Molecules - Made of tiny / discrete particles/

More information

IGCSE (9-1) Edexcel - Chemistry

IGCSE (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 information

PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE

PRACTICE 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

Orchard School. New Document 1 Name: Class: Date: 129 minutes. Time: 126 marks. Marks: Comments: Page 1

Orchard School. New Document 1 Name: Class: Date: 129 minutes. Time: 126 marks. Marks: Comments: Page 1 New Document Name: Class: Date: Time: Marks: 29 minutes 26 marks Comments: Page Q. The ph scale is a measure of the acidity or alkalinity of a solution. (a) Solution Draw one line from each solution to

More information

NATIONAL 5 CHEMISTRY

NATIONAL 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 information

ST EDWARD S OXFORD. Lower Sixth Entrance Assessment. November Chemistry. 1 Hour. Candidates name:... St Edward's School 1

ST EDWARD S OXFORD. Lower Sixth Entrance Assessment. November Chemistry. 1 Hour. Candidates name:... St Edward's School 1 ST EDWARD S OXFORD Lower Sixth Entrance Assessment November 2013 Chemistry 1 Hour Candidates name:... St Edward's School 1 St Edward's School 2 1. Complete the table below. Element calcium Symbol Pb S

More information

Quantitative Chemistry. AQA Chemistry topic 3

Quantitative 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 information

Set 4 Marking Scheme: Acid Bases & Salts 2010

Set 4 Marking Scheme: Acid Bases & Salts 2010 Set 4 Marking Scheme: Acid Bases & Salts 00 ACID AND BASES PAPER : STRUCTURE (a) Neutralisation KOH + H SO 4 K SO 4 + H O Correct formulae of reactants and products Balanced equation i. H +, OH -, K +

More information

TOPIC 4: THE MOLE CONCEPTS

TOPIC 4: THE MOLE CONCEPTS TOPIC 4: THE MOLE CONCEPTS INTRODUCTION The mass is gram (g) of 1 mole of substances is called its.. 1 mole of substances has.. particles of a substances The mass of 1 mole of substances is always equal

More information

CHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS

CHEM111 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 information

Draw one line from each solution to the ph value of the solution. Solution ph value of the solution

Draw 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 information

Stoichiometry Part 1

Stoichiometry 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 information

London Examinations IGCSE

London 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 information

CHAPTER 8 SALTS. NaCl. A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion.

CHAPTER 8 SALTS. NaCl. A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion. CHAPTER 8 SALTS A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion. The salt consists of two parts, cation from base and anion from acid.

More information

Quantitative chemistry Atomic structure Periodicity

Quantitative chemistry Atomic structure Periodicity IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States

More information

Identification of ions and gases

Identification of ions and gases For more awesome GSE and level resources, visit us at www.savemyexams.co.uk/ Identification Of ions nd Gases Question Paper Level Subject Exam oard Topic Sub-Topic ooklet O Level hemistry ambridge International

More information

Chapter 5 Chemical Calculations

Chapter 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 information

CHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS

CHEM111 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 information

Formulae of simple compounds

Formulae of simple compounds 4. Stoichiometry Formulae of simple compounds Formulae of simple compounds can be deduced from their ions but there are some that you should know off by heart. You must learn the following formulae: Carbon

More information

London Examinations IGCSE

London Examinations IGCSE Centre No. Candidate No. Paper Reference(s) 4335/1F London Examinations IGCSE Chemistry Paper 1F Foundation Tier Monday 10 November 2008 Afternoon Time: 1 hour 30 minutes Materials required for examination

More information

4.4. Revision Checklist: Chemical Changes

4.4. 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 information

1.21. Formulae, equations and amounts of substance

1.21. Formulae, equations and amounts of substance 1.21. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as

More information

(2) (1) (2) The isotopic composition of a sample of sulphur is found using a mass spectrometer.

(2) (1) (2) The isotopic composition of a sample of sulphur is found using a mass spectrometer. 1. (a) State the meaning of the terms relative atomic mass......... mass number...... (iii) isotopes......... The isotopic composition of a sample of sulphur is found using a mass spectromer. Explain how

More information

Year 10 Chemistry Exam June 2011 Multiple Choice. Section A Mulltiple Choice

Year 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 information

Quantitative Chemistry

Quantitative 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 information

9.1 Qualitative Analysis

9.1 Qualitative Analysis Chemistry Form 4 Page 44 Ms. R. Buttigieg Test for positive Ions (Cations) 9.1 Qualitative Analysis 1) Flame Tests Nichrome wire is dipped in concentrated hydrochloric acid, then in the salt being tested.

More information

mohd 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)

mohd 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 information

KENYA NATIONAL EXAMINATION COUNCIL REVISION MOCK EXAMS 2016 TOP NATIONAL SCHOOLS KAPSABET BOYS CHEMISTRY PAPER 1 TIME: 2 HOURS

KENYA NATIONAL EXAMINATION COUNCIL REVISION MOCK EXAMS 2016 TOP NATIONAL SCHOOLS KAPSABET BOYS CHEMISTRY PAPER 1 TIME: 2 HOURS KENYA NATIONAL EXAMINATION COUNCIL REVISION MOCK EXAMS 2016 TOP NATIONAL SCHOOLS KAPSABET BOYS CHEMISTRY PAPER 1 TIME: 2 HOURS SCHOOLS NET KENYA Osiligi House, Opposite KCB, Ground Floor Off Magadi Road,

More information

Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. ... [3] ...

Describe 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 information

Year 10 Chemistry Exam June 2011 Multiple Choice. Section A Multiple Choice

Year 10 Chemistry Exam June 2011 Multiple Choice. Section A Multiple Choice Year 10 Chemistry Exam June 2011 Multiple Choice Section A Multiple Choice 1 An aqueous solution is obtained when: a. a substance dissolves in any liquid b. a substance is dissolved in water c. when a

More information

London Examinations IGCSE

London Examinations IGCSE Centre No. Candidate No. Paper Reference(s) 4437/2F London Examinations IGCSE Science (Double Award) Chemistry Paper 2F Foundation Tier Monday 10 November 2008 Afternoon Time: 1 hour 15 minutes Materials

More information

Year 10 Science Chemistry Examination November 2011 Part A Multiple Choice

Year 10 Science Chemistry Examination November 2011 Part A Multiple Choice Year 10 Science Chemistry Examination November 2011 Part A Multiple Choice Answer these questions on the multiple choice answer sheet provided 2 Isotopes have been found as variations of atoms. Which of

More information

Year 10 Chemistry. Practice questions. Topics

Year 10 Chemistry. Practice questions. Topics Year 10 Chemistry Practice questions Topics 1 Group 1 2 Group 7 3 Reactivity series 4 Air and Water 5 Rates of reaction 6 Electrolysis 7 Acids, Alkali and Salts Objective: Evaluate group 1 & 7 reactivity

More information

London Examinations IGCSE

London Examinations IGCSE Centre No. Candidate No. Paper Reference(s) 4437/5H London Examinations IGCSE Science (Double Award) Chemistry Paper 5H Higher Tier Tuesday 16 November 2010 Afternoon Time: 1 hour 30 minutes Materials

More information

ICSE Board Class X Chemistry Board Paper Time: 1½ hrs Total Marks: 80

ICSE Board Class X Chemistry Board Paper Time: 1½ hrs Total Marks: 80 ICSE Board Class X Chemistry Board Paper 2011 Time: 1½ hrs Total Marks: 80 General Instructions: 1. Answers to this paper must be written on the paper provided separately. 2. You will NOT be allowed to

More information

National 4/5 Chemistry

National 4/5 Chemistry National 4/5 Chemistry Homework Unit 1 Chemical Changes and Structure Please do not write on these booklets questions should be answered in homework jotters. Part 1 Introduction to Unit 1 1. Which box

More information

NCERT Solutions for Atoms and Molecules

NCERT 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 information

For More Free KCSE Past Papers & Answers Visit K.C.S.E CHEMISTRY PAPER 1

For More Free KCSE Past Papers & Answers Visit   K.C.S.E CHEMISTRY PAPER 1 K.C.S.E. 2011 CHEMISTRY PAPER 1 1 What name is given to the process by which alcohol is formed from a carbohydrate? (1 mark) Explain why the solubility of ethane in water is lower than that of ethanol.

More information

THE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION. Instructions

THE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION. Instructions THE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION 032/1 CHEMISTRY 1 (For Both School and Private Candidates) TIME: 3 Hours Thursday, 05 th October

More information

MR. D HR UV AS HE R I.C.S.E. BOA RD PAP ER

MR. D HR UV AS HE R I.C.S.E. BOA RD PAP ER MR D HR UV AS HE R ICSE BOA RD PAP ER 200 6 1 ICSE-2006 Section 1 (40 Marks) (Attempt all questions from this section) Question 1 (a) Select from the list given below (A to F), the o0ne substance in each

More information

Cambridge International Examinations Cambridge Ordinary Level

Cambridge International Examinations Cambridge Ordinary Level Cambridge International Examinations Cambridge Ordinary Level *6377602299* CHEMISTRY 5070/42 Paper 4 Alternative to Practical October/November 2015 1 hour Candidates answer on the Question Paper. No Additional

More information

burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3

burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3 1 Crystals of sodium sulphate-10-water, Na 2 SO 4.10H 2 O, are prepared by titration. burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3 (a)

More information

THE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION

THE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION THE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION 032/1 CHEMISTRY 1 (For Both School and Private Candidates) Time: 3 Hours Thursday, 06 th November

More information

ST EDWARD S OXFORD 16+ ENTRANCE EXAMINATION. For entry in September Chemistry. Use of a calculator is permitted.

ST EDWARD S OXFORD 16+ ENTRANCE EXAMINATION. For entry in September Chemistry. Use of a calculator is permitted. ST EDWARD S OXFORD 16+ ENTRANCE EXAMINATION For entry in September 2017 Chemistry Use of a calculator is permitted Time: 1 hour Candidate s Name: Total marks available: 60 St Edward's School 16+ Entrance

More information

MARAKWET WEST DISTRICT 233/1 CHEMISTRY PAPER 1 JULY/AUGUST 2015 TIME: 2 HOURS

MARAKWET WEST DISTRICT 233/1 CHEMISTRY PAPER 1 JULY/AUGUST 2015 TIME: 2 HOURS MARAKWET WEST DISTRICT 233/1 CHEMISTRY PAPER 1 JULY/AUGUST 2015 TIME: 2 HOURS 1. State two reasons why we use the non- luminous flame for heating in the laboratory instead of using luminous flame. 2. The

More information

MAHESH TUTORIALS I.C.S.E.

MAHESH TUTORIALS I.C.S.E. MAHESH TUTORIALS I.C.S.E. GRADE - X (2017-2018) Exam No. : MT/ICSE/SEMI PRELIM - II - SET -A 020 Periodic Table, Chemical bonding, Acid, Bases and Salts, Practical Work, Mole Concept, Electrolysis Chemistry

More information

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4 Honors Chemistry Practice Final 2017 KEY 1. Acetylene gas, C 2, is used in welding because it generates an extremely hot flame when combusted with oxygen. How many moles of oxygen are required to react

More information

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg? 1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams

More information

1.21. Formulae, equations and amounts of substance

1.21. Formulae, equations and amounts of substance 1.21. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as

More information

ICSE Chemistry Model Paper-9

ICSE Chemistry Model Paper-9 ICSE Chemistry Model Paper-9 Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading the

More information

PURE SUBSTANCES AND MIXTURES. Substance = form of a matter consisting of a great number of elementary particles: atoms, ions and...

PURE SUBSTANCES AND MIXTURES. Substance = form of a matter consisting of a great number of elementary particles: atoms, ions and... PURE SUBSTANCES AND MIXTURES Substance = form of a matter consisting of a great number of elementary particles: atoms, ions and... Substances differ in the kind of the particles they consist of. The type

More information

Chemistry Final Exam Sample Items

Chemistry Final Exam Sample Items Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons

More information

Gozo College Boys Secondary Victoria - Gozo, Malta Ninu Cremona

Gozo College Boys Secondary Victoria - Gozo, Malta Ninu Cremona Gozo College Boys Secondary Victoria - Gozo, Malta Ninu Cremona Half Yearly Examination 2012-2013 Form 3 J.L. Chemistry Time: 1½ Hours Name: Class: Marks Grid [For Examiners use only] Question number Max

More information

Name Pd SN Date Chemistry Review Packet- Spring 2014

Name Pd SN Date Chemistry Review Packet- Spring 2014 Name Pd SN Date Chemistry Review Packet- Spring 2014 1.1.1 Draw pictures to illustrate the differing isotopes and ions of a given element. 1.1.1 Which atomic symbol represents an isotope of sulfur with

More information

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is

More information

Unit 8 Chemical Reactions- Funsheets

Unit 8 Chemical Reactions- Funsheets Part A- Balancing Equations and Types of Reactions Balance AND identify the following reactions: Unit 8 Chemical Reactions- Funsheets 1) Mg + Zn(NO 3) 2 Zn Mg(NO 3) 2 2) Ba + AgNO 3 Ag + Ba(NO 3) 2 3)

More information

THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY AT Myton School

THE 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 information

3. Atoms and Molecules. Mark (1) Mark (1) Mark (1) Mark (1) Mark (1) Mark (1) Marks (2)

3. Atoms and Molecules.  Mark (1) Mark (1) Mark (1) Mark (1) Mark (1) Mark (1) Marks (2) 3. Atoms and Molecules Q 1 144 grams of pure water is decomposed by passing electricity. 16 grams of hydrogen and 128 grams of oxygen are obtained. Which chemical law is illustrated by this statement?

More information

Identification of Ions and Gases

Identification of Ions and Gases Identification of Ions and Gases Question Paper 1 Level IGSE Subject hemistry (0620/0971) Exam oard ambridge International Examinations (IE) Topic cids, bases and salts Sub-Topic Identification of ions

More information

Kenya Certificate of Secondary Education (K.C.S.E.)

Kenya Certificate of Secondary Education (K.C.S.E.) Name: School:. Date:... 233/1 CHEMISTRY PAPER 1 JULY /AUGUST 2011 TIME: 2 HOURS Index No. Candidate s Sign.... Kenya Certificate of Secondary Education (K.C.S.E.) Chemistry Paper 1 INSTRUCTIONS TO THE

More information

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters] 1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?

More information

2. 2 Complete this table of the parts of an atom: Particle Charge Location in atom Proton. Negative

2. 2 Complete this table of the parts of an atom: Particle Charge Location in atom Proton. Negative Q Outcome 1. 1 Give a definition of the term matter 2. 2 Complete this table of the parts of an atom: Particle Charge Location in atom Proton In the nucleus Negative 3. 2 Draw an atom and label all particles.

More information

GIRLS JUNIOR LYCEUM L-IMRIEĦEL HALF YEARLY EXAMINATIONS 2016/2017

GIRLS JUNIOR LYCEUM L-IMRIEĦEL HALF YEARLY EXAMINATIONS 2016/2017 1 GIRLS JUNIOR LYCEUM L-IMRIEĦEL HALF YEARLY EXAMINATIONS 2016/2017 FORM: 4 CHEMISTRY Time: 1hr30min Name: Class: One mole of electrons carries a charge of 96500C or 1 Faraday One mole of any gas occupies

More information

4.4. Revision Checklist: Chemical Changes

4.4. 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 information

Centre Number Candidate Number Candidate Name UNIVERSITY OF CAMBRIDGE LOCAL EXAMINATIONS SYNDICATE General Certificate of Education Ordinary Level CHEMISTRY 5070/4 PAPER 4 Alternative to Practical MAY/JUNE

More information

(DO NOT WRITE ON THIS TEST)

(DO NOT WRITE ON THIS TEST) Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation

More information

ESA Study Guide Year 10 Science

ESA Study Guide Year 10 Science Then and now Questions from pages 26, 27 of ESA Study Guide Year 10 Science 1. Which early scientist thought atoms would combine to form new substances? 2. Which New Zealand scientist found that most of

More information

Stoichiometric relationships 1

Stoichiometric relationships 1 Stoichiometric relationships 1 Chapter outline Describe the three states of matter. Recall that atoms of diff erent elements combine in fi xed ratios to form compounds which have diff erent properties

More information

Jawapan. Chemistry. Chemistry Paper 1(4541/1) SOALAN ULANGKAJI SPM 2010 [4541/1] [4541/2] [4541/3]

Jawapan. Chemistry. Chemistry Paper 1(4541/1) SOALAN ULANGKAJI SPM 2010 [4541/1] [4541/2] [4541/3] SOALAN ULANGKAJI SPM 00 37 Jawapan Chemistry [454/] [454/] [454/3] Chemistry Paper (454/) A A 3 A 4 B 5 D 6 C 7 D 8 B 9 C 0 A B D 3 B 4 A 5 C 6 D 7 C 8 D 9 B 0 A A D 3 D 4 C 5 B 6 C 7 D 8 A 9 A 30 A 3

More information

SARALA BIRLA ACADEMY BANGALORE FINAL EXAMINATIONS Chemistry (One and Half Hours) Grade VII Tuesday, 17/032/2009

SARALA BIRLA ACADEMY BANGALORE FINAL EXAMINATIONS Chemistry (One and Half Hours) Grade VII Tuesday, 17/032/2009 SARALA BIRLA ACADEMY BANGALORE FINAL EXAMINATIONS 2008 2009 Chemistry (One and Half Hours) Grade VII Tuesday, 17/032/2009 Answers to this Paper must be written on this paper itself. You will not be allowed

More information

For the element X in the ionic compound MX, explain the meaning of the term oxidation state.

For the element X in the ionic compound MX, explain the meaning of the term oxidation state. 1. (a) By referring to electrons, explain the meaning of the term oxidising agent.... For the element X in the ionic compound MX, explain the meaning of the term oxidation state.... (c) Complete the table

More information

Personalised Learning Checklists AQA Chemistry Paper 1

Personalised 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 information

A 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: 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 information

IGCSE Double Award Extended Coordinated Science

IGCSE Double Award Extended Coordinated Science IGCSE Double Award Extended Coordinated Science Chemistry 4.1 - The Mole Concept The Atomic Mass Unit You need to know the atomic mass unit and the relative atomic mass. In Unit C3.3, 1 atomic mass unit

More information

AQA Chemistry GCSE. Topic 3: Quantitative Chemistry. Flashcards.

AQA 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 information

5. What is the name of the compound PbO? 6. What is the name of HCl(aq)?

5. What is the name of the compound PbO? 6. What is the name of HCl(aq)? 1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole

More information

YEAR 10- Chemistry Term 1 plan

YEAR 10- Chemistry Term 1 plan YEAR 10- Chemistry Term 1 plan 2016-2017 Week Topic Learning outcomes 1 1. The particulate nature of matter State the distinguishing properties of solids, liquids and gases. Describe the structure of solids,

More information

Paper Reference. Sample Assessment Material Time: 2 hours

Paper 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 information

Q1. Ammonia is used in the production of fertilisers. The flow diagram shows the main stages in the manufacture of ammonia.

Q1. Ammonia is used in the production of fertilisers. The flow diagram shows the main stages in the manufacture of ammonia. Q1. Ammonia is used in the production of fertilisers. The flow diagram shows the main stages in the manufacture of ammonia. Study the flow diagram and then answer the questions. (a) What is the purpose

More information

THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY Birchwood High School

THE 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 information

Questions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:..

Questions 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 information

Mark scheme Answers Marks (a) (i) 2.8.4 4 (b) (i) Decreases // Become smaller Proton number / Positive charges increases // Forces of attraction increases (c) Achieved octet electron arrangement // Has

More information

Trilogy Quantitative chemistry

Trilogy Quantitative chemistry Trilogy Quantitative chemistry Foundation revision questions Name: Class: Date: Time: 6 minutes Marks: 6 marks Comments: Page of 23 (a) Formulae and equations are used to describe chemical reactions. Aluminium

More information

Lesson (1) Mole and chemical equation

Lesson (1) Mole and chemical equation Lesson (1) Mole and chemical equation 1 When oxygen gas reacts with magnesium, magnesium oxide is formed. Such Reactions are described by balanced equations known as "chemical equations" Δ 2Mg(s) + O2(g)

More information

Cambridge International Examinations Cambridge Ordinary Level

Cambridge International Examinations Cambridge Ordinary Level Cambridge International Examinations Cambridge Ordinary Level *0594498264* CHEMISTRY 5070/42 Paper 4 Alternative to Practical October/November 2016 1 hour Candidates answer on the Question Paper. No Additional

More information

A-LEVEL TRANSITION COURSE SUMMER 2018 PART 2: USING CHEMICAL EQUATIONS

A-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 information

Chapter 6: Chemical Bonding

Chapter 6: Chemical Bonding Chapter 6: Chemical Bonding Learning Objectives Describe the formation of ions by electron loss/gain to obtain the electronic configuration of a noble gas. Describe the formation of ionic bonds between

More information

Dushan [δβ] BOODHENA 1

Dushan [δβ] BOODHENA 1 CHEMISTRY SUMMARY FOR THE FORM 3 NATIONAL ASSESSMENT 1. Define the term element. An element is a pure substance that cannot be broken down into simpler substances by any ordinary chemical process. 2. Define

More information

Year 8 Chemistry Knowledge Organiser Topic 1: Periodic Table

Year 8 Chemistry Knowledge Organiser Topic 1: Periodic Table KPI 1.1: Identify, with reasons, differences between atoms, elements and compounds Key Terms Element Mixture Compound Elements Definitions A substance that contains only one type of atom A substance that

More information

Paper Reference. London Examinations IGCSE. Foundation Tier. Tuesday 10 November 2009 Afternoon Time: 1 hour 30 minutes

Paper Reference. London Examinations IGCSE. Foundation Tier. Tuesday 10 November 2009 Afternoon Time: 1 hour 30 minutes Centre No. Candidate No. Paper Reference(s) 4335/1F London Examinations IGCSE Chemistry Paper 1F Foundation Tier Tuesday 10 November 2009 Afternoon Time: 1 hour 30 minutes Materials required for examination

More information

Spring Semester Final Exam Study Guide

Spring 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 information

ICSE-Science 2(Chemistry) 2009

ICSE-Science 2(Chemistry) 2009 ICSE-Science 2(Chemistry) 2009 Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading

More information

Answers for UNIT ONE NAT 5 Flash Cards

Answers 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 information

NITROGEN AND ITS COMPOUNDS Q30 (i) Explain how the following would affect the yield of ammonia. An increase in (i). Pressure.

NITROGEN AND ITS COMPOUNDS Q30 (i) Explain how the following would affect the yield of ammonia. An increase in (i). Pressure. NAME SCHOOL INDEX NUMBER DATE NITROGEN AND ITS COMPOUNDS 1. 1990 Q30 (i) Explain how the following would affect the yield of ammonia. An increase in (i). Pressure. (2 marks) marks)... (ii) Temperature

More information

All you need to know about Additional Science

All you need to know about Additional Science All you need to know about Additional Science Chapters in this unit 1. Structures and bonding 2. Structures and properties 3. How much? 4. Rates of reaction 5. Energy and reactions 6. Electrolysis 7. Acids,

More information

Silver nitrate solution is added to sodium dichromate solution

Silver nitrate solution is added to sodium dichromate solution Chem. 110 50 Points Final Exam Part 1 Practice Write the chemical names or formulas for the following a H 2 SO 4 b NiNO 2 c Aluminum thiosulfate d Plumbic acetate e Ag 2 C 2 O 4 f P 2 O 5 g Cyanic acid

More information

Ammonium Chloride and sodium hydrogen carbonate. Step II

Ammonium Chloride and sodium hydrogen carbonate. Step II K.C.S.E 2000 CHEMISTRY PAPER 233/1 QUESTIONS 1. Explain the change in mass that occurs when the following substances are separately heated in open crucibles (a) Copper metal (b) Copper (II) nitrate 2.

More information

CHEMISTRY 135 REVISION OF NAMES, FORMULAE AND EQUATIONS

CHEMISTRY 135 REVISION OF NAMES, FORMULAE AND EQUATIONS CHEMISTRY 135 REVISION OF NAMES, FORMULAE AND EQUATIONS Answer the following questions as if you were going to hand them in for marking. You will be tested on them in class time. 1) Give the correct chemical

More information

...[1] (ii) Name two elements from group 0....[2] (b)(i) Which box best represents particles from group 0 elements?...[1]......[1]

...[1] (ii) Name two elements from group 0....[2] (b)(i) Which box best represents particles from group 0 elements?...[1]......[1] High Demand Questions QUESTIONSHEET 1 The boxes represent particles of different gases. One box shows the particles of elements in group 0 (group 8). A B C D What name is given to group 0 (8) elements?

More information