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

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1 New Document Name: Class: Date: Time: Marks: 29 minutes 26 marks Comments: Page

2 Q. The ph scale is a measure of the acidity or alkalinity of a solution. (a) Solution Draw one line from each solution to the ph value of the solution. ph value of the solution 5 Acid 7 9 Neutral 3 (2) (b) Which ion in aqueous solution causes acidity? Tick one box. H + Na + O 2 OH () (c) When sulfuric acid is added to sodium hydroxide a reaction occurs to produce two products. The equation is: Page 2

3 H 2 SO 4 + 2NaOH Na 2 SO 4 + 2H 2 O How many elements are in the formula H 2 SO 4? Tick one box () (d) What is this type of reaction? Tick one box. Decomposition Displacement Neutralisation Reduction () (e) Name the salt produced. () Page 3

4 (f) Describe how an indicator can be used to show when all the sodium hydroxide has reacted with sulfuric acid. (3) (Total 9 marks) Q2. The table below shows information about some elements. Element Melting point in C Boiling point in C Fluorine Chlorine 0 35 Bromine 7 59 Iodine 4 84 Astatine (a) Look at the table above. Describe the trend in melting point from fluorine to astatine. () (b) Estimate the boiling point of astatine. Use the table above to help you. Boiling point of astatine = C () Page 4

5 (c) Room temperature is 20 C. Which element in the table above is a liquid at room temperature? () (d) To which group of the periodic table do the elements in the table above belong? Tick one box. Group 0 Group Group 5 Group 7 () (e) A chlorine atom has 7 electrons. On the figure below, use crosses to show the arrangement of electrons in the outer shell of a chlorine atom. () (f) Chlorine reacts with sodium bromide solution to produce bromine and sodium chloride solution. Page 5

6 Complete the symbol equation for the reaction. Cl 2 + NaBr + (2) (g) Which element in the table above will react with sodium chloride solution? Give a reason for your answer. (2) (Total 9 marks) Q3. This question is about metals. Tick ( (a) Which unreactive metal is found in the Earth as the metal itself? ) one box. aluminium gold magnesium () (b) Complete the sentence. Aluminium is an element because aluminium is made of Page 6

7 only one type of. () (c) Figure shows the electronic structure of an aluminium atom. (i) Use the correct words from the box to complete the sentence. electrons ions protons neutrons shells The nucleus of an aluminium atom contains and. (2) (ii) Complete the sentence. In the periodic table, aluminium is in Group. () (d) Aluminium is used for kitchen foil. Figure 2 shows a symbol on a box of kitchen foil. Page 7

8 The symbol means that aluminium can be recycled. It does not show the correct chemical symbol for aluminium. (i) What is the correct chemical symbol for aluminium?. () (ii) Give two reasons why aluminium should be recycled. (2) (e) Aluminium has a low density, conducts electricity and is resistant to corrosion. Which one of these properties makes aluminium suitable to use as kitchen foil? Give a reason for your answer. (2) (Total 0 marks) Page 8

9 Q4. The three states of matter are solid, liquid and gas. (a) Lithium reacts with water to produce lithium hydroxide solution and hydrogen. Use the correct state symbols from the box to complete the chemical equation. aq g l s 2Li(s) + 2H 2 O(l) 2LiOH( ) + H 2 ( ) lithium + water lithium hydroxide + hydrogen (2) (b) Figure shows the melting points and the boiling points of four substances, A, B, C and D. Figure Which substance is liquid over the greatest temperature range? Tick one box. A Page 9

10 B C D () (c) Which two substances are gases at 50 C? Tick one box. A and B B and C C and D A and D () (d) A different substance, E, has: a melting point of 50 C a boiling point of +20 C Plot these two values on Figure. (2) (e) Figure 2 shows the apparatus a student used to determine the melting point and the boiling point of substance B in Figure. Figure 2 Page 0

11 Explain why the student could not use this apparatus to determine the boiling point of substance B. (2) (f) Suggest one reason why the student could not use this apparatus to determine the exact melting point of substance B. () (Total 9 marks) Q5. In 866 John Newlands produced an early version of the periodic table. Part of Newlands periodic table is shown below. Column H Li Be B C N O F Na Mg Al Si P S Cl K Ca Cr Ti Mn Fe Page

12 Newlands periodic table arranged all the known elements into columns in order of their atomic weight. Newlands was trying to show a pattern by putting the elements into columns. (a) Iron (Fe) does not fit the pattern in column 7. Give a reason why. () (b) In 869 Dmitri Mendeleev produced his version of the periodic table. Why did Mendeleev leave gaps for undiscovered elements in his periodic table? () (c) Newlands and Mendeleev placed the elements in order of atomic weight. Complete the sentence. The modern periodic table places the elements in order of. () (d) Lithium, sodium and potassium are all in Group of the modern periodic table. Explain why. (2) (Total 5 marks) Page 2

13 Q6. Five elements, V, W, X, Y and Z, are shown in the periodic table. The letters are not the chemical symbols of the five elements. Use the correct letter, V, W, X, Y or Z, to answer each question. (a) Which element is a transition metal? () (b) Which element is in Group 2? () (c) Which element is a noble gas? () Page 3

14 (d) Which element has an atomic (proton) number of 4? () (e) Which element forms only + ions? () (Total 5 marks) Q7. The structures of four substances, A, B, C and D, are represented in Figure. (a) Use the correct letter, A, B, C or D, to answer each question. (i) Which substance is a gas? () (ii) Which substance is a liquid? () (iii) Which substance is an element? () Page 4

15 (iv) Which substance is made of ions? () (b) Figure 2 shows the bonding in substance C. (i) What is the formula of substance C? SO 2 SO 2 S 2 O Draw a ring around the correct answer. () (ii) Use the correct answer from the box to complete the sentence. delocalised shared transferred When a sulfur atom and an oxygen atom bond to produce substance C, electrons are () (iii) What is the type of bonding in substance C? Draw a ring around the correct answer. covalent ionic metallic () (Total 7 marks) Page 5

16 Q8. (a) A particle of ammonia is represented by the formula NH 3 or as: (i) How many different elements are there in a particle of ammonia? () (ii) Draw a ring around the correct answer to complete the sentence. A particle of ammonia is called an atom. an ion. a molecule. () (iii) Complete the dot and cross bonding diagram for ammonia. Show only electrons in the outer energy level of each atom. (2) (b) Ammonia gas reacts with hydrogen chloride gas to produce a white solid. The formula of the white solid is NH 4 Cl (i) Complete the equation by adding the correct state symbols. Page 6

17 NH 3 (g) + HCl( ) NH 4 Cl( ) () (ii) The white solid has the formula NH 4 Cl Complete the name of the white solid. Ammonium () (c) Concentrated ammonia solution gives off ammonia gas. Concentrated hydrochloric acid gives off hydrogen chloride gas. Apparatus was set up as shown in Diagram. Diagram Cotton wool soaked in concentrated hydrochloric acid Cotton wool soaked in concentrated ammonia solution (i) Concentrated hydrochloric acid is corrosive. Give one safety precaution you should take when using concentrated hydrochloric acid. () (ii) After 3 minutes a white solid was seen in the glass tube, as shown in Diagram 2. Diagram 2 Page 7

18 Cotton wool soaked in concentrated hydrochloric acid Cotton wool soaked in concentrated ammonia solution White solid formed here Suggest why the white solid is seen nearer the concentrated hydrochloric acid than the concentrated ammonia. () (iii) The experiment was repeated at a higher temperature. Explain why the white solid was produced in less than 3 minutes. (2) (Total 0 marks) Q9. There are several different forms of carbon and many different carbon compounds. (a) Figure shows a 3D model of a molecule of methane (CH 4 ). Figure Page 8

19 Draw the 2D structure of a methane molecule. () (b) Different forms of carbon have different bonding and structure. Draw one line from the form of carbon to the bonding and structure. Form of carbon Bonding and structure (3) (c) Crude oil is a mixture of many different carbon compounds. Crude oil can be separated into useful fractions by fractional distillation. Figure 2 shows a column used to separate crude oil. Figure 2 Page 9

20 Complete the sentences. Use words from the box. condense evaporate freeze Crude oil is heated so that most of the compounds At different temperatures the compounds cool and (2) (d) Which fraction is the most viscous? Tick one box. Engine oil Diesel oil Kerosene Petrol () Page 20

21 (e) Which fraction is the most flammable? Tick one box. Diesel oil Kerosene Petrol Refinery gas () (f) Why does kerosene separate out of the mixture before diesel oil? () (Total 9 marks) Q0. The picture shows a student filling in a multiple choice answer sheet using a pencil. Cihan Ta?k?n/iStock The pencil contains graphite. Graphite rubs off the pencil onto the paper. Diagrams and 2 show how the atoms are arranged in graphite. Page 2

22 (a) Use the diagrams to help you explain why graphite can rub off the pencil onto the paper. (2) (b) Draw a ring around the type of bond which holds the atoms together in each layer. covalent ionic metallic () (Total 3 marks) Q. Formulae and equations are used to describe chemical reactions. (a) Aluminium reacts with sulfuric acid (H 2 SO 4 ) to produce aluminium sulfate, Al 2 (SO 4 ) 3 and hydrogen (H 2 ). Complete and balance the equation for this reaction. Al + + (2) Page 22

23 (b) Calcium carbonate reacts with nitric acid to produce calcium nitrate. Calculate the relative formula mass ( M r ) of calcium nitrate, Ca(NO 3 ) 2 Relative atomic masses ( A r ): N = 4; O = 6; Ca = 40 Relative formula mass ( M r ) = (2) (c) Zinc carbonate decomposes when heated. A student heated 25 g zinc carbonate (ZnCO 3 ). The figure below shows how he set up the apparatus. The balanced chemical equation for the decomposition reaction is: ZnCO 3 (s) ZnO (s) + CO 2 (g) The student measured the mass of solid product after heating until there was no further change in mass. The student did the experiment four times. The table below shows the results. Experiment Mass of solid product in g Calculate the mean mass of the solid product. Do not use any anomalous results in your calculation. Page 23

24 Mean mass = g (2) (Total 6 marks) Q2. This question is about lithium and sodium. (a) Use the Chemistry Data Sheet to help you to answer this question. In which group of the periodic table are lithium and sodium? Group () (b) A lithium atom can be represented as The diagram represents the lithium atom. (i) Some particles in the nucleus have a positive charge. What is the name of these particles? () (ii) Some particles in the nucleus have no charge. What is the name of these particles? () Page 24

25 (iii) Use the correct answer from the box to complete the sentence The mass number of this atom of lithium is () (c) Sodium reacts with chlorine to produce sodium chloride. sodium + chlorine sodium chloride The diagram shows how the reaction happens. Only the outer electrons are shown. Draw a ring around the correct answer to complete each sentence. gaining (i) A sodium atom changes into a sodium ion by losing an electron. sharing () a negative (ii) A sodium ion has no charge. a positive () Page 25

26 (iii) The ions in sodium chloride are held together by covalent strong electrostatic forces. magnetic () (d) Sodium chloride is an ionic compound. Tick ( ) two properties of ionic compounds. Property Tick ( ) Do not dissolve in water High melting points Low boiling points Strong bonds (2) (e) (i) The formula of sodium chloride is NaCl Calculate the relative formula mass of sodium chloride. Relative atomic masses: Na = 23; Cl = 35.5 Relative formula mass = () (ii) Draw a ring around the correct answer to complete each sentence. The relative formula mass of a substance, in grams, Page 26

27 ion is one isotope of the substance. mole () (f) Nanoparticles of sodium chloride (salt) are used to flavour crisps. What are nanoparticles? () (Total 2 marks) Q3. How a metal is used depends on its properties. A teacher demonstrated some of the properties of sodium (an alkali metal) and iron (a transition element) by placing a small cube of each metal into water. A student observed that: Sodium floated on the surface of the water melted to form a molten ball of sodium reacted to produce a gas no sodium was left after 5 minutes Iron sank to the bottom of the water did not melt did not react the cube of iron remained after 5 minutes (a) Tick ( ) two properties of sodium compared with iron that are shown by the student s observations. Sodium compared with iron Tick( ) sodium has a higher boiling point Page 27

28 sodium has a lower density sodium is harder sodium is more reactive sodium is softer (2) (b) Draw a ring around the correct answer to complete the word equation. carbon dioxide sodium + water sodium hydroxide + hydrogen oxygen () (c) Draw a ring around the correct answer to complete the sentence. H + (aq) Sodium hydroxide is an alkali because it produces OH - (aq) ions Na + (aq) in aqueous solution. () (Total 4 marks) Q4. This question is about the reactions of acids. (a) When dilute hydrochloric acid is reacted with sodium hydroxide solution there is a temperature change. Explain how the temperature changes. Page 28

29 (2) (b) Acids produce hydrogen ions in aqueous solutions. What is the ionic equation for neutralisation reactions? Tick one box. H + (aq) + H 2 O(l) H 3 O + (aq) H + (aq) + OH (aq) H 2 O(l) 2 H 2 O(l) H 3 O + (aq) + OH (aq) H 2 O(l) 2 H + (aq) + O 2 (aq) () (c) Sulfuric acid reacts with copper carbonate to produce a salt, water and carbon dioxide. H 2 SO 4 + CuCO 3 CuSO 4 + H 2 O + CO 2 What is the name of the salt produced? () (d) A student reacted four metals with water and with a dilute acid to work out the order of reactivity of the metals. Metal The table below shows some of the observations. Reaction with water Reaction with dilute acid Calcium Bubbles of gas X Copper Y No bubbles of gas Magnesium Few bubbles of gas Bubbles of gas Zinc No bubbles of gas Bubbles of gas Page 29

30 Write the observations for X and Y. Observation at X Observation at Y (2) (e) Write the four metals, calcium, copper, magnesium and zinc, in order of reactivity. Start with the most reactive metal. (2) (f) Some gases given off in reactions can be identified by chemical tests. Draw one line from each chemical test to the name of the gas. Chemical test Gas (3) (g) Acids react with bases to produce salts and water (H 2 O). The electronic structure of a hydrogen atom is 2, The electronic structure of an oxygen atom is 2,6 Page 30

31 Draw a diagram to show the arrangement of the outer shell electrons in a molecule of water. (2) (Total 3 marks) Q5. This question is about the electrolysis of two compounds. Figure shows the electrolysis of molten lead bromide. Figure (a) The electrolyte contains lead ions (Pb 2+ ) and bromide ions (Br ). Complete the sentences. Use words from the box. atoms bromide bromine ions lead molecules oxygen At the positive electrode the gas produced is At the negative electrode lead gain electrons and. (3) Page 3

32 (b) A student measured the volumes of each gas produced during the electrolysis of water. The table below shows the student s results. Time in minutes Volume of gas produced in cm 3 Hydrogen Oxygen The student plotted a graph of the results for oxygen. Figure 2 shows the graph. The student did not put a scale on the y axis. On the graph in Figure 2 : complete the scale for the y axis plot the results for hydrogen include a line of best fit. Figure 2 Page 32

33 (3) (c) Use the graph to calculate the mean volume of oxygen produced per second. Mean volume of oxygen produced = cm 3 / s (3) (Total 9 marks) Q6. A student investigates the energy released when zinc powder reacts with copper sulfate solution. The student uses the apparatus shown in Figure. Page 33

34 The student: measures 00 cm 3 copper sulfate solution into a beaker measures the temperature of the copper sulfate solution puts g zinc powder into the beaker stirs the mixture with a thermometer measures the highest temperature. The student s results were: Starting temperature = 2 C Highest temperature = 32 C (a) (i) Calculate the change in temperature. Change in temperature = C () (ii) Calculate the energy released in the reaction. energy released in J Use the equation = volume of solution in cm temperature change in C Energy released = J (2) (b) The reaction of zinc with copper sulfate is exothermic. Page 34

35 How can you tell from the student s results that the reaction is exothermic? () (c) The energy diagram for the reaction is shown in Figure 2. (i) How can you tell from the energy diagram that the reaction is exothermic? () (ii) Which arrow shows the activation energy in Figure 2? Tick ( ) one box. A B C () (Total 6 marks) Page 35

36 M. (a) extra lines from solution negate the mark 2 (b) H + (c) 3 (d) Neutralisation (e) (f) sodium sulfate Add indicator to sodium hydroxide solution allow add indicator to sulfuric acid Add sulfuric acid (gradually) allow add sodium hydroxide solution (gradually) allow ph probe until indicator just changes (colour) or until universal indicator turns green or shows ph7 [9] M2. (a) the melting point increases Page 36

37 (b) 337 C allow an answer in the range 278 C to 337 C (c) bromine (d) Group 7 (e) 7 electrons in outer shell (f) Cl NaBr Br NaCl correct formulae for products correct balancing (g) fluorine Page 37 (because it is) more reactive than chlorine allow because it is the most reactive element

38 [9] M3. (a) gold (b) atom (s) (c) (i) protons any order allow proton neutrons allow neutron (ii) 3 / three (d) (i) Al ignore any numbers / charges (ii) any two from: limited resource expensive in terms of energy / mining effects on the environment, such as, landfill, atmospheric pollution, quarrying allow uses a lot of energy to extract. 2 (e) resistant to corrosion does not react (with water or food) allow one mark for low density with a suitable reason given [0] Page 38

39 M4. (a) LiOH (aq) this order H 2 (g) (b) C (c) A and D (d) point x at 0 C point at +50 C (e) substance B will not reach its boiling point of 90 C because the boiling point of water is only 00 C (f) there is too much substance B to melt instantly. allow answers based on thermal conductivity or temperature gradient from the wall of the test tube to the thermometer [9] Page 39

40 M5. (a) (iron) is a metal accept transition element allow (iron) had different properties (to oxygen and sulfur) ignore electrons (b) so that elements with similar properties could be placed together allow to make the pattern fit ignore undiscovered elements (c) atomic number(s) allow proton number(s) (d) all have one electron in the outer shell (highest energy level) allow same number of electrons in the outer shell (highest energy level) (so they) have similar properties or react in the same way allow specific reactions e.g. with water [5] M6. (a) Y (b) W (c) V (d) W (e) X [5] Page 40

41 M7. (a) (i) C (ii) (iii) (iv) B A D (b) (i) SO 2 (ii) shared (iii) covalent [7] M8. (a) (i) two (ii) a molecule (iii) one pair of electrons between nitrogen and each of 3 hydrogens rest correct second mark dependent on first (b) (i) (g) (s) Page 4

42 (ii) chloride ignore formulae (c) (i) any one from: wear goggles wear gloves do not breathe in fumes wipe up spills immediately work in a fume cupboard (ii) (particles of) ammonia move faster than (particles of) hydrogen chloride allow diffuses faster allow hydrochloric acid (iii) particles / molecules have more energy do not accept atoms / ions so they move faster ignore references to rate of reaction [0] M9. (a) (b) Form of carbon Bonding and structure Page 42

43 extra lines from the left negate the mark 3 (c) evaporate condense (d) Engine oil (e) Refinery gas (f) because its boiling point is lower [9] M0. (a) layers which have weak forces / attractions / bonds between them second mark must be linked to layers Page 43

44 or which can slide over each other or separate ignore references to rubbing (b) covalent [3] M. (a) 2Al + 3H 2 SO 4 Al 2 (SO 4 ) 3 + 3H 2 formulae correct balancing correct (b) (4 + (3 6)) = 64 allow 64 with no working shown for 2 marks (c) ( ) / 3 = 7.3 allow 7.3 with no working shown for 2 marks [6] M2. (a) / one (b) (i) protons (ii) neutrons Page 44

45 (iii) 7 (c) (i) losing (ii) a positive (iii) electrostatic (d) high melting points strong bonds (e) (i) 58.5 (ii) mole (f) very small (particles) or ignore tiny / small / smaller / microscopic etc. -00nm in size or (particle with a) few hundred atoms [2] Page 45

46 M3. (a) sodium has a lower density sodium is more reactive (b) hydrogen (c) OH (aq) [4] M4. (a) it goes up / increases because the reaction is exothermic or transfers energy to the surroundings allow gives out thermal / heat energy (b) H + (aq) + OH (aq) H 2 O(l) (c) copper sulfate (d) (e) X bubbles of gas Y no bubbles of gas calcium>magnesium>zinc>copper if not all correct allow mark for at least two metals in the correct position 2 Page 46 (f) Chemical test Gas

47 extra lines from a test negate the mark 3 (g) two pairs of shared electrons oxygen has four other electrons not bonded [3] M5. (a) bromine ions atoms (b) correct scale on y axis Page 47 points correctly plotted using the scale

48 ± ½ small square best-fit line drawn (c) value for oxygen divided by corresponding time 60 = 0.05 (cm 3 / s) allow 0.05 with no working shown for 3 marks [9] M6. (a) (i) (ii) 4620 (J) correct answer gains 2 marks with or without working allow 4.62kJ for 2 marks if answer is incorrect: gains mark or (their temp. rise) gains mark or (their temp. rise) correctly calculated gains 2 marks 2 (b) the temperature increases allow gets hotter allow heat / energy is given off Page 48

49 (c) (i) (energy of) products lower than (energy of) reactants allow converse allow arrow C points downwards (ii) A [6] Page 49