C Atomic Structure and Periodic Table 35 Questions Name: Class: Date: Time: Marks: Comments: Page of 08
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 3 (2) (b) Which ion in aqueous solution causes acidity? Tick one box. H + Na + O 2 OH () Page 2 of 08
(c) When sulfuric acid is added to sodium hydroxide a reaction occurs to produce two products. The equation is: 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. 3 4 6 7 () (d) What is this type of reaction? Tick one box. Decomposition Displacement Neutralisation Reduction () (e) Name the salt produced. () Page 3 of 08
(f) Describe how an indicator can be used to show when all the sodium hydroxide has reacted with sulfuric acid. (3) (Total 9 marks) 2 John Newlands arranged the known elements into a table in order of atomic weight. Figure shows part of Newlands table. Figure Group 2 3 4 5 6 7 H Li Be B C N O F Na Mg Al Si P S Cl K Ca (a) What are the names of the elements in Group 5 of Newlands table? Tick one box. Calcium and sulfur Carbon and silicon Chlorine and silver Chromium and tin () Page 4 of 08
(b) In what order is the modern periodic table arranged? Tick one box. Atomic mass Atomic number Atomic size Atomic weight () (c) Give two differences between Group of Newlands table and Group of the periodic table. (2) Page 5 of 08
(d) In 864, atoms were thought to be particles that could not be divided up into smaller particles. By 898, the electron had been discovered and the plum pudding model of an atom was proposed. Figure 2 shows the plum pudding model of an atom of carbon and the nuclear model of an atom of carbon. Figure 2 Compare the position of the subatomic particles in the plum pudding model with the nuclear model. (4) Page 6 of 08
(e) Models are used to show the differences between elements, compounds and mixtures. Which circle shows a model of a mixture? Tick one box. () (f) Figure 3 shows a model of carbon dioxide. Figure 3 What does each line between the atoms in Figure 3 represent? Tick one box. Covalent bond Intermolecular force Ionic bond Metallic bond () (Total 0 marks) Page 7 of 08
3 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) Page 8 of 08
(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 B C D () Page 9 of 08
(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) Page 0 of 08
(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 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) Page of 08
4 This question is about calcium. (a) What type of compound is calcium oxide? Tick one box. An acid A base A carbonate A salt () (b) Ionic compounds, such as calcium oxide, have high melting points. Complete the sentences. Use words from the box. bonds forces ions layers Calcium oxide has a giant ionic lattice in which there are strong electrostatic of attraction in all directions. () Page 2 of 08
(c) The figure below shows the electronic structure of an oxygen atom and a calcium atom. Describe how the calcium atom and the oxygen atom forms calcium oxide. You should give the charge on each ion formed. (4) (Total 6 marks) Page 3 of 08
5 Figure shows a reactor used to produce titanium from titanium(iv) chloride. Figure The chemical equation for the reaction of titanium(iv) chloride with sodium is: TiCl 4 + 4Na Ti + 4NaCl titanium(iv) chloride + sodium titanium + sodium chloride (a) For one reaction: 65 kg titanium(iv) chloride reacted completely with 782 kg sodium 989 kg sodium chloride was produced. Calculate the mass of titanium produced from this reaction. Mass of titanium = kg () Page 4 of 08
(b) The table below shows the solubility of sodium chloride in 00 cm 3 of aqueous solution at different temperatures. Solubility of sodium chloride in g per 00cm 3 Temperature in C 35.72 0 35.89 20 36.09 30 37.37 40 36.69 50 37.04 60 On Figure 2: plot this data on the grid draw a line of best fit. Figure 2 (3) Page 5 of 08
Volume of water = dm 3 (2) (c) The product sodium chloride is dissolved in water to separate it from titanium. At 30 C the solubility of sodium chloride is 36 kg per 00 dm 3. Calculate the minimum volume of water in dm 3, at 30 C, needed to dissolve 989 kg sodium chloride. (d) Calculate the percentage by mass of titanium in titanium(iv) chloride (TiCl 4 ). Give your answer to 3 significant figures. Relative atomic masses (A r ): Cl = 35.5; Ti = 48 Percentage of titanium by mass = % (3) (e) Suggest why the reaction is done in an atmosphere of dry argon instead of air containing water vapour. (3) Page 6 of 08
(f) Explain why titanium conducts electricity. (3) (Total 5 marks) 6 Elements are made up of atoms. (a) What is the approximate radius of an atom? Tick one box. 0 m 0 m 0 0 m 0 00 m () (b) The figure below shows the atoms of five elements. The letters are not the symbols of these elements. Complete the sentence. All of the elements in the figure above are in Group of the periodic table. () Page 7 of 08
(c) Which two atoms in the figure above are isotopes of the same element? Explain your answer fully. (3) (d) The halogens are in Group 7 of the periodic table. Explain the trend in reactivity of the halogens. (6) (Total marks) Page 8 of 08
7 The apparatus in the figure below is used to separate a mixture of liquids in a fuel. (a) What is apparatus W on above the figure above? Tick one box. Beaker Boiling Tube Flask Jug () Page 9 of 08
(b) What is the name of this method of separation? Tick one box. Crystallisation Electrolysis Filtration Distillation () (c) Name the changes of state taking place at A and B in the figure above. Use words from the box. boiling condensing freezing melting Change of state at A: Change of state at B: (2) Page 20 of 08
(d) Table shows the boiling points of the hydrocarbons in the fuel. Table Hydrocarbon Boiling point in C Pentane 36 Hexane 69 Heptane 98 Octane 25 Which hydrocarbon will be the last to collect in the beaker? Tick one box. Pentane Hexane Heptane Octane () Page 2 of 08
(e) The fuel is a mixture of liquids that has been designed as a useful product. What name is given to this type of mixture? Tick one box. Catalyst Formulation Polymer Solvent () (f) Describe how this fuel is different from crude oil. (2) Page 22 of 08
(g) A student measured the melting point of a solid hydrocarbon four times. The student s results are in Table 2. Table 2 Trial Trial 2 Trial 3 Trial 4 Melting point in C 35 48 37 37 Calculate the mean melting point of the hydrocarbon, leaving out any anomalous result. Give your answer to two significant figures. Mean melting point = C (2) (Total 0 marks) 8 This question is about drinking water. (a) Name two methods of treating water from rivers, lakes or the sea to produce drinking water. Tick two boxes. Anaerobic digestion Cracking Desalination Electrolysis Sterilising (2) Page 23 of 08
(b) The table below shows the amounts of dissolved ions in a sample of drinking water. Dissolved ion Mass in mg per dm 3 Cl 250 Na + 200 NO 3 + 40 What is the name of the ion with the symbol Cl? Tick one box. Calcium ion Carbonate ion Chloride ion Chlorine ion () Page 24 of 08
(c) Use the information in the table above to complete the bar chart in Figure. Figure () (d) Look at the questions labelled A, B, C, D. A How many substances are there in drinking water? B How much fluoride is in drinking water? C Is fluoride soluble in drinking water? D Should fluoride be added to drinking water? Which one of the questions cannot be answered by science alone? Tick one box. A B C D () Page 25 of 08
(e) Give two reasons why the answer you have chosen cannot be answered by science alone.. 2. (2) (f) A sample of drinking water contains.5 mg of fluoride per dm 3 of water. A person drinks dm 3 of this water. The recommended daily amount of fluoride is 4.0 mg. Which calculation gives the percentage of the recommended daily amount of fluoride in dm 3 of this water? Tick one box. () Page 26 of 08
(g) Figure 2 shows the effect of fluoride in drinking water on tooth decay in different age groups. Figure 2 Describe the pattern of tooth decay in Figure 2 for water without fluoride. Use data to justify your answer. (2) (h) Describe the effect of adding fluoride to drinking water for the age groups in Figure 2. (2) (Total 2 marks) Page 27 of 08
9 The figure below shows an atom of boron. (a) When the mass of the boron atom is calculated, the mass of the electrons is ignored. Why is the mass of the electrons ignored? () (b) How many electrons are there in the boron atom? () (c) What is the electrical charge on the nucleus of the boron atom? Tick one box. + +5 +6 + () Page 28 of 08
(d) The mass number of boron is. Use the figure above to calculate the number of neutrons in the nucleus of the boron atom. Explain how you worked out the answer. Number of neutrons = Explanation (3) (e) Phosphorus has a mass number of 3 and has 6 neutrons. What percentage of the mass number of phosphorus is the number of neutrons? Give your answer to two significant figures. Percentage = (2) (Total 8 marks) 0 The figure below shows a simple model of the three states of matter. (a) What is the correct equation to work out the density of a material? () Page 29 of 08
(b) A student explains density to his teacher using the particle model in the figure above. His teacher says there are limitations to the model. Give two limitations of the particle model in the figure above.. 2. (2) (c) When the gas in a container with a fixed volume is heated, the pressure increases as the temperature increases. Explain why the pressure increases. Use the model in the figure above to help you. (4) (Total 7 marks) Page 30 of 08
A student used paper chromatography to identify the pigments in spinach leaves. She used propanone as a solvent. Figure shows the student s results. Figure (a) Name the mobile phase and the stationary phase in the student s experiment. Mobile phase Stationary phase (2) Page 3 of 08
(b) What does Figure tell you about the green pigment from spinach? (3) (c) Write the equation that links distance moved by solvent, distance moved by solute and R f value. () (d) Use Figure to calculate the R f value for pigment B. R f value = (3) Page 32 of 08
(e) Another student set up the apparatus shown in Figure 2. Figure 2 This student did not set up the apparatus correctly. Identify the errors the student made. Explain how the errors she made would affect her results. (4) (Total 3 marks) Page 33 of 08
2 Figure shows the plum pudding model of the atom. This model was used by some scientists after the discovery of electrons in 897. Figure Plum-pudding model In 9 the scientists Geiger and Marsden investigated the effect of firing alpha particles at very thin sheets of gold foil. Their experiment is shown in Figure 2. The arrows show the paths taken by alpha particles in the experiment. Figure 2 (a) Explain why scientists replaced the plum pudding model of the atom with the nuclear model of the atom as a result of the experiment. (4) Page 34 of 08
(b) According to modern measurements: the radius of an atom is about 0 0 m the radius of an atomic nucleus is about 0 4 m Show that these values fit with the nuclear model of the atom. (2) (c) In 93 a scientist discovered that there are hydrogen atoms with mass number 2 as well as hydrogen atoms with mass number. A year later, another scientist discovered neutrons. Explain why the discovery of neutrons could explain the presence of hydrogen atoms with different mass numbers. (3) (d) How would the results of the experiment shown in Figure 2 change if neutrons were used instead of alpha particles to bombard a thin sheet of gold? (2) (Total marks) Page 35 of 08
3 The elements in the periodic table are arranged in groups. (a) What is similar about the elements in the same group? Tick one box. Chemical properties Atomic numbers Relative atomic masses () (b) Figure shows the arrangement of electrons in an atom. Figure What group of the periodic table is this atom in? Group () Page 36 of 08
(c) Why are the elements in Group 0 unreactive? Tick one box. They are all gases at room temperature They all have the same atomic number They are all in the same group of the periodic table They all have a stable arrangement of electrons () Page 37 of 08
(d) A teacher demonstrates the reaction of some alkali metals with water. Look at Figure 2. Figure 2 The students write what they see.. The alkali metals float on water. 2. The alkali metals fizz when they react with water. 3. The universal indicator changes from green to purple. 4. The sodium disappears faster than the lithium. Give a reason for each of the four things that the students see.. The alkali metals float on water. Reason 2. The alkali metals fizz when they react with water. Reason 3. The universal indicator changes from green to purple. Reason 4. The sodium disappears faster than the lithium. Reason (4) (Total 7 marks) Page 38 of 08
4 In 869 there were 60 known elements. Mendeleev arranged the elements in order of their atomic mass (atomic weight). He realised that elements with similar properties occurred at regular intervals. (a) Suggest why one of the groups that is on today s periodic table was not in Mendeleev s periodic system. () (b) Explain the arrangement of the first 20 elements in today s periodic table. You should answer in terms of atomic structure. (2) Page 39 of 08
(c) A student put some potassium bromide solution in a test tube. She added a few drops of chlorine solution and observed the result. She repeated the process using different potassium halide salts and different halogens. The table below shows the student s results. Solution of halogen Potassium chloride solution Potassium bromide solution Potassium iodide solution Chlorine Orange colour forms Brown colour forms Bromine No reaction Brown colour forms Iodine No reaction No reaction Give the order of reactivity of the halogens from the results in the table above. Explain how you used the results to show this order of reactivity. Order Explanation (2) (d) Write a balanced ionic equation for the reaction of chlorine with bromide ions in solution. (3) Page 40 of 08
(e) Explain the order of reactivity of Group 7 elements. Include information about atomic structure. (2) (Total 0 marks) 5 The table below shows information about some elements. Element Melting point in C Boiling point in C Fluorine 202 88 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 () (c) Room temperature is 20 C. Which element in the table above is a liquid at room temperature? () Page 4 of 08
(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. Complete the symbol equation for the reaction. Cl 2 + NaBr + (2) Page 42 of 08
(g) Which element in the table above will react with sodium chloride solution? Give a reason for your answer. (2) (Total 9 marks) 6 The elements in Group of the periodic table are metals. (a) The elements in Group are called the alkali metals. Why are they called the alkali metals? (2) (b) Explain the increase in reactivity of elements further down the group. (4) Page 43 of 08
(c) Lithium oxide is an ionic compound. Draw a dot and cross diagram to show how lithium and oxygen combine to form lithium oxide. Only show the electrons in the outer shell of each atom. Give the charges on the ions formed. (4) (Total 0 marks) 7 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? () (d) Which element has an atomic (proton) number of 4? () Page 44 of 08
(e) Which element forms only + ions? () (Total 5 marks) 8 This question is about magnesium. (a) (i) The electronic structure of a magnesium atom is shown below. Use the correct answer from the box to complete each sentence. electrons neutrons protons shells The nucleus contains protons and The particles with the smallest relative mass that move around the nucleus are called Atoms of magnesium are neutral because they contain the same number of electrons and (3) Page 45 of 08
(ii) A magnesium atom reacts to produce a magnesium ion. Which diagram shows a magnesium ion? Tick ( ) one box. () (b) Magnesium and dilute hydrochloric acid react to produce magnesium chloride solution and hydrogen. Mg(s) + 2 HCl(aq) MgCl 2 (aq) + H 2 (g) (i) State two observations that could be made during the reaction.. 2. (2) Page 46 of 08
(ii) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. Describe a method for making pure crystals of magnesium chloride from magnesium and dilute hydrochloric acid. In your method you should name the apparatus you will use. You do not need to mention safety. (6) (Total 2 marks) 9 This question is about metals. (a) Which unreactive metal is found in the Earth as the metal itself? Tick ( ) one box. aluminium gold magnesium () Page 47 of 08
(b) Complete the sentence. Aluminium is an element because aluminium is made of 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. () Page 48 of 08
(d) Aluminium is used for kitchen foil. Figure 2 shows a symbol on a box of kitchen foil. 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 49 of 08
20 This question is about atomic structure and elements. (a) Complete the sentences. (i) (ii) The atomic number of an atom is the number of The mass number of an atom is the number of () () (b) Explain why an atom has no overall charge. Use the relative electrical charges of sub-atomic particles in your explanation. (2) (c) Explain why fluorine and chlorine are in the same group of the periodic table. Give the electronic structures of fluorine and chlorine in your explanation. (2) Page 50 of 08
(d) The diagram shows the electronic structure of an atom of a non-metal. What is the chemical symbol of this non-metal? Tick ( ) one box. Ar O S Si () (e) When elements react, their atoms join with other atoms to form compounds. Complete the sentences. (i) Compounds formed when non-metals react with metals consist of particles called. () (ii) Compounds formed from only non-metals consist of particles called. () (Total 9 marks) Page 5 of 08
2 This question is about carbon and gases in the air. (a) Carbon atoms have protons, neutrons and electrons. Complete the table by writing the relative mass of a neutron and an electron. Name of particle Relative mass proton neutron electron (2) (b) What is the total number of protons and neutrons in an atom called? Tick ( ) one box. The atomic number The mass number One mole of the atom () (c) An atom of carbon has six electrons. Which structure, A, B or C, represents the electronic structure of the carbon atom? The carbon atom is structure () Page 52 of 08
(d) Carbon reacts with oxygen to produce carbon dioxide (CO 2 ). (i) How many different elements are in one molecule of carbon dioxide? () (ii) What is the total number of atoms in one molecule of carbon dioxide? () (e) Sometimes carbon reacts with oxygen to produce carbon monoxide (CO). (i) Calculate the relative formula mass (M r ) of carbon monoxide. Relative atomic masses (A r ): C = 2; O = 6 M r of carbon monoxide = () (ii) Calculate the percentage by mass of carbon in carbon monoxide. Percentage by mass of carbon in carbon monoxide = % () Page 53 of 08
(f) Carbon dioxide is one of the gases in the air. (i) The graph shows the percentage of argon and the percentage of carbon dioxide in the air. What is the percentage of argon in the air? Percentage of argon = % () (ii) An instrumental method is used to measure the amount of carbon dioxide in the air. Give one reason for using an instrumental method. () (Total 0 marks) Page 54 of 08
22 This question is about atoms and isotopes. (a) Atoms contain protons, neutrons and electrons. A lithium atom has the symbol Explain, in terms of sub-atomic particles, why the mass number of this lithium atom is 7. (3) (b) Amounts of substances can be described in different ways. Complete the sentences. One mole of a substance is the relative formula mass in The relative atomic mass of an element compares the mass of an atom of an element with the mass of an atom of (2) (c) Two isotopes of oxygen are and Describe the similarities and differences between the isotopes and You should refer to the numbers of sub-atomic particles in each isotope. (3) (Total 8 marks) Page 55 of 08
23 The diagram shows the chemical symbols of five elements in the periodic table. (a) Choose the correct chemical symbol to complete each sentence. (i) The element that is an alkali metal is. (ii) The element that is a transition metal is. (iii) The element in Group 4 is. () () () (iv) The element with a full outer energy level (shell) of electrons is. () (b) Which other element goes in the shaded box? () (Total 5 marks) Page 56 of 08
24 In 866 John Newlands produced an early version of the periodic table. Part of Newlands periodic table is shown below. Column 2 3 4 5 6 7 H Li Be B C N O F Na Mg Al Si P S Cl K Ca Cr Ti Mn Fe 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. () Page 57 of 08
(d) Lithium, sodium and potassium are all in Group of the modern periodic table. Explain why. (2) (Total 5 marks) 25 This question is about the halogens (Group 7). (a) How do the boiling points of the halogens change down the group from fluorine to iodine? () (b) Sodium bromide is produced by reacting sodium with bromine. Sodium bromide is an ionic compound. (i) Write down the symbols of the two ions in sodium bromide. () (ii) Chlorine reacts with sodium bromide solution to produce bromine and one other product. Complete the word equation for the reaction. chlorine + sodium bromide bromine + () (iii) Why does chlorine displace bromine from sodium bromide? () (iv) Use the Chemistry Data Sheet to help you to answer this question. Suggest which halogen could react with sodium chloride solution to produce chlorine. () (Total 5 marks) Page 58 of 08
26 The positions of eight elements in the modern periodic table are shown below. Choose the correct chemical symbols to complete each sentence. (a) The two metals that react vigorously with water are and. (b) The element used as a catalyst in the Haber process is. () () (c) The two elements with five electrons in their outer shell (highest energy level) are and. () (d) Iron has ions with different charges. The other metal that has ions with different charges is. () (Total 4 marks) 27 The diagram shows a carbon atom. Page 59 of 08
(a) (i) A proton is labelled. Use the correct answer from the box to label each of the other sub-atomic particles. electron ion molecule neutron (2) (ii) The atom of carbon is represented as: What is the mass number of this carbon atom? Draw a ring around the correct answer. 6 3 9 () (iii) Complete the sentence. Atoms of carbon have no overall electrical charge because the number of protons is the same as the number of. () (b) Butane is represented as: (i) Use the correct answer from the box to complete each sentence. bond compound helium hydrogen mixture oxygen Butane is a. Butane contains atoms of carbon and. Each line between the atoms in butane represents a chemical. (3) Page 60 of 08
(ii) Which is the correct formula for butane? Tick ( ) one box. C 4 H 4 C 4 H 8 C 4 H 0 () (Total 8 marks) 28 Sulfur is a non-metal. Sulfur burns in the air to produce sulfur dioxide, SO 2 (a) Why is it important that sulfur dioxide is not released into the atmosphere? Tick ( ) one box. Sulfur dioxide causes acid rain. Sulfur dioxide causes global dimming. Sulfur dioxide causes global warming. () (b) Sulfur dioxide dissolves in water. What colour is universal indicator in a solution of sulfur dioxide? Give a reason for your answer. (2) Page 6 of 08
(c) Sulfur dioxide is a gas at room temperature. The bonding in sulfur dioxide is covalent. Explain, in terms of its structure and bonding, why sulfur dioxide has a low boiling point. (3) (d) In this question you will be assessed on using good English, organising information clearly and using specialist terms where appropriate. Sulfur dioxide is produced when fossil fuels are burned. It is important that sulfur dioxide is not released into the atmosphere. Three of the methods used to remove sulfur dioxide from gases produced when fossil fuels are burned are: wet gas desulfurisation ( W) dry gas desulfurisation ( D) seawater gas desulfurisation ( S). Information about the three methods is given in the bar chart and in Table and Table 2. Method of removing sulfur dioxide Page 62 of 08
Table Method Material used How material is obtained W Calcium carbonate, CaCO 3 Quarrying D Calcium oxide, CaO Thermal decomposition of calcium carbonate: CaCO 3 CaO + CO 2 S Seawater From the sea Table 2 Method W D S What is done with waste material Solid waste is sold for use in buildings. Carbon dioxide is released into the atmosphere. Solid waste is sent to landfill. Liquid waste is returned to the sea. Page 63 of 08
Evaluate the three methods of removing sulfur dioxide from waste gases. Compare the three methods and give a justified conclusion. (6) (Total 2 marks) Page 64 of 08
29 (a) Figure shows an atom of element G. Figure Draw a ring around the correct answer to complete each sentence. (i) Label A shows an electron an ion a nucleus () (ii) The particle labelled B is an isotope a molecule a neutron () (iii) The mass number of element G is 5 6 () (iv) Use the periodic table to identify element G. Element G is boron carbon sodium () Page 65 of 08
(b) Figure 2 shows a compound of G and hydrogen. Figure 2 Draw a ring around the correct answer to complete each sentence. (i) The formula of the compound in Figure 2 is GH 3 G 3 H 3HG () (ii) The type of bonding shown in Figure 2 is covalent ionic metallic () (Total 6 marks) Page 66 of 08
30 (a) The symbols for seven different elements are shown in Figure. Figure He Be Na S Ar Ca Fe Choose the correct symbol from Figure to answer each question. You may use each symbol once, more than once or not at all. Write the symbol that represents: (i) a Group element () (ii) a transition metal () (iii) an element with electrons in the same number of energy levels as an atom of argon (Ar) () (iv) an element which forms an oxide that dissolves in water to form an acidic solution () (v) an element that forms a chloride with the formula XCl () Page 67 of 08
(b) A teacher put a cube of sodium metal into water containing universal indicator, as shown in Figure 2. Figure 2 The equation for the reaction is: 2Na(s) + 2H 2 O(l) 2NaOH (aq) + H 2 (g) sodium + water sodium hydroxide + hydrogen (i) The sodium floated on the surface of the water. The universal indicator turned purple. Give three other observations that would be seen during the reaction.. 2. 3. (3) (ii) Name the ion that made the universal indicator turn purple. () Page 68 of 08
(c) Figure 3 represents the electronic structure of a sodium atom. Figure 3 In the space below, draw the electronic structure of a sodium ion. Include the charge on the ion. (2) (Total marks) 3 A student investigated the conductivity of different concentrations of sodium chloride solution. The student set the apparatus up as shown in Figure. Figure Page 69 of 08
The student measured the conductivity of the pure water with a conductivity meter. The reading on the conductivity meter was zero. (a) The student: added sodium chloride solution one drop at a time stirred the solution recorded the reading on the conductivity meter. The student s results are shown in the table below. Number of drops of sodium chloride solution added Relative conductivity of solution 0 0 00 2 20 3 30 4 400 5 50 6 590 7 70 8 800 Page 70 of 08
(i) The student plotted the results on the grid shown in Figure 2. Plot the four remaining results. Draw a line of best fit, ignoring the anomalous result. Figure 2 Number of drops of sodium chloride added (3) (ii) One of the points is anomalous. Suggest one error that the student may have made to cause the anomalous result. () Page 7 of 08
(iii) The student wanted to compare the conductivity of sodium chloride solution with the conductivity of potassium chloride solution. State one variable he should keep constant when measuring the conductivity of the two solutions. () (b) (i) Explain, in terms of bonding, why pure water does not conduct electricity. (2) (ii) Explain why sodium chloride solution conducts electricity. (2) (iii) After he had added sodium chloride solution, the student noticed bubbles of gas at the negative electrode. Complete the sentence. The gas produced at the negative electrode is () (Total 0 marks) Page 72 of 08
32 Use the periodic table and the information in the table below to help you to answer the questions. The table shows part of an early version of the periodic table. Group Group 2 Group 3 Group 4 Group 5 Group 6 Group 7 H Li Be B C N O F Na Mg Al Si P S Cl (a) Hydrogen was placed at the top of Group in the early version of the periodic table. The modern periodic table does not show hydrogen in Group. (i) State one similarity between hydrogen and the elements in Group. () (ii) State one difference between hydrogen and the elements in Group. () (b) Fluorine, chlorine, bromine and iodine are in Group 7, the halogens. The reactivity of the halogens decreases down the group. Bromine reacts with a solution of potassium iodide to produce iodine. Br 2 + 2KI 2KBr + I 2 (i) In the reaction between bromine and potassium iodide, there is a reduction of bromine to bromide ions. In terms of electrons, what is meant by reduction? () (ii) Complete the half equation for the oxidation of iodide ions to iodine molecules. 2I (2) Page 73 of 08
(iii) Explain, in terms of electronic structure, why fluorine is the most reactive element in Group 7. (3) (Total 8 marks) 33 A student was trying to produce hydrogen gas. Figure shows the apparatus she used. Figure (a) No gas was produced. The student s teacher said that this was because the substances in the flask did not react. (i) Suggest why the substances in the flask did not react. () Page 74 of 08
(ii) Which two substances could the student have put in the flask to produce hydrogen safely? Tick ( ) one box. Gold and dilute hydrochloric acid Potassium and dilute hydrochloric acid Zinc and dilute hydrochloric acid () (b) Another student did produce hydrogen from two substances. Figure 2 shows the apparatus the student used to collect and measure the volume of the hydrogen gas. Figure 2 Give the name of the apparatus labelled X. () Page 75 of 08
Mean volume = cm 3 (2) (c) The student did the experiment four times. Her results are shown in the table below. Experiment Volume of hydrogen collected in one minute in cm 3 49 2 50 3 35 4 48 (i) One of the results is anomalous. Which result is anomalous? Write your answer in the box. Give a reason for your choice. (2) (ii) Calculate the mean volume of hydrogen collected in one minute. (iii) Give a reason why the experiment should be repeated several times. () Page 76 of 08
(d) A teacher collected two tubes full of hydrogen gas, as shown in Figure 3. Figure 3 She tested tube A with a lighted splint as soon as she took the bung out. She tested tube B with a lighted splint a few seconds after taking the bung out. (i) Suggest why tube B gave a much louder pop than tube A. () (ii) Complete and balance the chemical equation for the reaction that takes place when the hydrogen reacts in this test. H 2 + O 2 (2) (Total marks) Page 77 of 08
34 Fossil fuels contain carbon. (a) The figure below represents a carbon atom. Draw a ring around the correct answer to complete each sentence. (i) The name of the particle with a positive charge is an electron. a neutron. a proton. () (ii) The centre of the atom is called the energy level. molecule. nucleus. () (iii) Use the Chemistry Data Sheet to help you to answer this question. Use the correct number from the box to complete each sentence. 4 6 8 0 2 The mass number of this carbon atom is In the periodic table, carbon is in Group Page 78 of 08
(b) Coal is a fossil fuel. A piece of coal contains: 80% carbon 9% oxygen % sulfur 5% hydrogen. The rest of the coal is other elements. (i) What is the percentage of other elements in this piece of coal? % () (ii) Coal burns in air to produce carbon dioxide, sulfur dioxide and water. Draw one line from each product to the type of pollution caused by each product. Product Type of pollution Acid rain Carbon dioxide Global dimming Sulfur dioxide Global warming Water No pollution (3) (Total 8 marks) Page 79 of 08
35 Glass is made from silicon dioxide. Velirina/iStock/Thinkstock (a) Silicon dioxide has a very high melting point. Other substances are added to silicon dioxide to make glass. Glass melts at a lower temperature than silicon dioxide. Suggest why. () (b) Sodium oxide is one of the substances added to silicon dioxide to make glass. (i) Sodium oxide contains Na + ions and O 2 ions. Give the formula of sodium oxide. () (ii) Sodium oxide is made by heating sodium metal in oxygen gas. Complete the diagram to show the outer electrons in an oxygen molecule (O 2 ). (2) Page 80 of 08
(c) Glass can be coloured using tiny particles of gold. Gold is a metal. Describe the structure of a metal. (3) (Total 7 marks) Page 8 of 08
Mark schemes (a) extra lines from solution negate the mark 2 (b) H + (c) 3 (d) (e) (f) Neutralisation 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] 2 (a) Carbon and silicon (b) Atomic number (c) Hydrogen / fluorine / chlorine are not in Group of the periodic table or Hydrogen and fluorine / chlorine are not in the same group of the periodic table Page 82 of 08
Lithium / sodium / potassium are in Group of the periodic table (d) plum pudding model has a single ball of positive charge and nuclear model has positive charges in the centre / nucleus plum pudding model has electrons in random positions and nuclear model has electrons in fixed positions plum pudding model has no nucleus and the nuclear model has a nucleus plum pudding model has no neutrons and the nuclear model has neutrons in the nucleus (e) (f) Covalent bond [0] 3 (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 Page 83 of 08
(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] 4 (a) A base (b) forces (c) calcium loses electrons and oxygen gains electrons max 3 for incorrect reference to atom / ion or to oxygen / oxide two electrons are transferred calcium has a 2 + charge oxide has a 2 charge [6] 5 (a) 408 kg (b) all points correct ± ½ small square allow mark if 5 points correct 2 best fit line (c) 5525 dm 3 (d) relative formula mass of TiCl 4 is 90 25.26 % Answer given to 3 significant figures = 25.3 % 25.23% with or without working gains 3 marks (e) argon is unreactive Page 84 of 08
(f) water (vapour) would react with sodium allow water (vapour) would react with titanium(iv) chloride and air contains oxygen that would react with reactants allow and air contains oxygen that would react with products (titanium conducts electricity) because electrons in the outer shell of the metal atoms are delocalised and so electrons are free to move allow the delocalised electrons in the metal carry electrical charge through the metal through the whole structure [5] 6 (a) 0 0 m (b) / one allow alkali metals (c) R and S because they have the same number of protons allow same atomic number, different mass number and a different numbers of neutrons Page 85 of 08
(d) Level 3 (5 6 marks): A relevant and coherent explanation of the trend in reactivity. The response makes logical links between the points raised and considers both the number of energy levels and the distance between the nucleus and the outer energy level. Level 2 (3 4 marks): Statements that are linked to provide a simple explanation of the trend in reactivity using either the number of energy levels or the distance between the nucleus and the outer energy level. Level ( 2 marks): Simple statements made about the halogens or the trend in reactivity. 0 marks: No relevant comment Indicative content Simple statements / descriptions have 7 electrons in the outer shell need to gain an electron form ions with a - charge halogens further down the group are less reactive (or vice versa) halogens further down the group have more shells or energy levels (or vice versa) Linked statements / explanations have 7 electrons in the outer shell so need to gain an electron to have the electronic structure of a noble gas halogens further down the group are less reactive because they have more shells or energy levels (or vice versa) halogens further down the group have more shells or energy levels so less attractive force on the incoming electron (or vice versa) halogens further down the group have more shells or energy levels so more shielding against the incoming electron (or vice versa) outer electrons of halogens further down group are further away from the attractive force of the nucleus (or vice versa) an electron is less easily gained because there are more shells or energy levels (or vice versa) an electron is less easily gained because the outer electrons are further from the attractive force of the nucleus (or vice versa) 6 [] 7 (a) Flask (b) Fractional distillation (c) A boiling in this order Page 86 of 08
(d) (e) (f) B condensing Pentane Formulation the fuel is a pure compound and crude oil is a mixture or the fuel is made up of four hydrocarbons allow crude oil contains a large number of compounds and the fuel contains four and crude oil could have many more (g) (35 + 37 + 37 / 3) = 36.33 36 allow (35 + 48 + 37 + 37 / 4 =) 39(.25) for mark [0] 8 (a) Desalination Sterilising (b) Chloride ion (c) correct bar for NO 3 - (d) (e) D any two from: people have the right to choose (opinion) ethical / moral question cannot be tested by experiment 2 (f) Page 87 of 08
(g) (h) the percentage tooth decay increases with age by 4 % for each increasing age group reduces tooth decay (for all age groups) greater reduction in older people [2] 9 (a) because the mass of an electron is very small do not accept has no mass (b) 5 / five (c) +5 (d) 6 (because) mass number = no. protons + no. electrons allow atomic number = 5 (so the number of) neutrons = 5 allow mass number number of protons (e) (6 / 3) 00 = 5.6 = 52 incorrect sig. figs max mark [8] 0 (a) density = mass / volume (b) any two from: no forces shown between spheres atoms / molecules / ions are not solid spheres not all the same size. 2 (c) at higher temperatures particles have more kinetic energy (so) the (average) speed of the particles increases Page 88 of 08
(so there are) more frequent collisions with the wall of the container which apply a greater force on wall of container (so pressure rises) [7] (a) mobile phase propanone stationary phase paper (b) any three from: contains chlorophyll a, b and carotene contains Pigment B does not contain pheophytin contains (at least) one unknown substance contains five substances contains a substance that does not dissolve in the solvent 3 (c) (d) both measurements correct solvent front = 9.0 cm and pigment B distance = 5.0 cm R f = 5.0 / 9.0 = 0.56 allow ecf from incorrect measurements (e) origin line drawn in ink so it will run or dissolve in the solvent or split up spots under solvent or solvent above spots / origin line so they will mix with solvent or wash off paper or colour the solvent or dissolve in the solvent [3] 2 (a) most alpha particles went straight through, suggesting lots of empty space a few alpha particles bounced back, suggesting small central nucleus Page 89 of 08
with all the positive charge the plum pudding model does not explain the results because it shows the whole atom as a ball of positive charge with no empty space (b) (c) (d) the figures show that the radius of an atom is 0 000 times bigger than the nucleus consistent with the nuclear model, which says that the atom has a tiny nucleus at the centre of the atom all hydrogen atoms have just one proton (in the nucleus) some hydrogen atoms also have one neutron protons and neutrons have the same relative mass so mass number of these atoms is 2 neutrons are not attracted or repelled by a positive nucleus so the neutrons would all pass through the foil [] 3 (a) Chemical properties (b) three / 3 (c) (d) They all have a stable arrangement of electrons less dense than water allow lighter than water gas / hydrogen produced an alkali / hydroxide is produced sodium is more reactive than lithium [7] 4 (a) did not appear because they had not been discovered or they are unreactive or they did not form compounds Page 90 of 08
(b) (c) arranged in order of atomic / proton number elements in the same group have the same number of electrons in the outer shell chlorine>bromine>iodine table shows that chlorine displaces bromine and iodine and bromine displaces iodine (d) Cl 2 (aq) + 2 Br (aq) Br 2 (aq) + 2 Cl (aq) correct formulae correct balancing correct state symbol (e) the further down the group, the halogen becomes less reactive because outer electrons are further from the nucleus so less attractive force on an incoming electron [0] 5 (a) the melting point increases (b) 337 C allow an answer in the range 278 C to 337 C (c) bromine (d) Group 7 Page 9 of 08
(e) 7 electrons in outer shell (f) Cl 2 + 2NaBr Br 2 + 2NaCl correct formulae for products correct balancing (g) fluorine (because it is) more reactive than chlorine allow because it is the most reactive element [9] 6 (a) because they form hydroxides that give alkaline solutions (in water) (b) the atoms have more electron shells (as move down the group) so the electron in the outer shell is further away from the nucleus which reduces the attraction to the nucleus so the electron is lost more easily from the atom (c) electronic structure of lithium drawn correctly Page 92 of 08
electronic structure of oxygen drawn correctly correct charge on ions (Li + and O 2 ) correct number of each ion (2 lithium, oxygen) [0] 7 (a) Y (b) W (c) V (d) W (e) X [5] 8 (a) (i) neutrons this order only electrons protons (ii) box on the left ticked (b) (i) effervescence / bubbling / fizzing / bubbles of gas do not accept just gas alone magnesium gets smaller / disappears allow magnesium dissolves allow gets hotter or steam produced ignore references to magnesium moving and floating / sinking and incorrectly named gases. Page 93 of 08
(ii) Marks awarded for this answer will be determined by the Quality of Communication (QC) as well as the standard of the scientific response. Examiners should also refer to the information in the Marking Guidance and apply a best fit approach to the marking. 0 marks No relevant content Level ( 2 marks) There are simple statements of some of the steps in a procedure for obtaining magnesium chloride. Level 2 (3 4 marks) There is a description of a laboratory procedure for obtaining magnesium chloride from dilute hydrochloric acid and magnesium. The answer must include a way of ensuring the hydrochloric acid is fully reacted or a method of obtaining magnesium chloride crystals. Level 3 (5 6 marks) There is a well organised description of a laboratory procedure for obtaining magnesium chloride that can be followed by another person. The answer must include a way of ensuring the hydrochloric acid is fully reacted and a method of obtaining magnesium chloride crystals. examples of the points made in the response: hydrochloric acid in beaker (or similar) add small pieces of magnesium ribbon until magnesium is in excess or until no more effervescence occurs * filter using filter paper and funnel filter excess magnesium pour solution into evaporating basin / dish heat using Bunsen burner leave to crystallise / leave for water to evaporate / boil off water decant solution pat dry (using filter paper). *Student may choose to use a named indicator until it turns a neutral colour, record the number of pieces of magnesium added then repeat without the indicator. 6 [2] 9 (a) gold (b) atom (s) Page 94 of 08
(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] 20 (a) (i) protons allow protons or electrons, but do not allow protons and electrons (ii) protons plus / and neutrons (b) (because the relative electrical charges are) () for an electron and +() for a proton allow electrons are negative and protons are positive and the number of electrons is equal to the number of protons if no other mark awarded, allow mark for the charges cancel out Page 95 of 08
(c) (the electronic structure of) fluorine is 2,7 and chlorine is 2,8,7 allow diagrams for the first marking point (so fluorine and chlorine are in the same group) because they have the same number of or 7 electrons in their highest energy level or outer shell if no other mark awarded, allow mark for have the same / similar properties (d) S (e) (i) ions (ii) molecules [9] 2 (a) must be in this order very small accept negligible, / 2000 allow zero (b) (c) The mass number C (d) (i) 2 (ii) 3 (e) (i) 28 (ii) 42.9 accept ecf from (e)(i) accept 42-43 Page 96 of 08
(f) (i) 0.9 (ii) any one from: accurate sensitive rapid small sample. [0] 22 (a) because this lithium atom has 3 protons and 4 neutrons mass number is total of neutrons and protons accept protons and neutrons have a mass of accept number of neutrons = 7-3(protons) ignore mass of electron is negligible (b) grams accept g 2 C allow carbon-2 or C-2 ignore hydrogen or H (c) any three from: max 2 if no numbers given numbers if given must be correct both have 8 protons accept same number of protons 8 O has 0 neutrons 6 O has 8 neutrons accept different number of neutrons or 8 O has two more neutrons for mark both have 8 electrons. accept same number of electrons 3 [8] Page 97 of 08
23 (a) (i) Na allow sodium (ii) Cu allow copper (iii) C allow carbon (iv) He allow helium (b) H allow hydrogen do not allow H 2 [5] 24 (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] 25 (a) increase Page 98 of 08
(b) (i) Na + and Br both required (ii) (iii) (iv) sodium chloride allow NaCl do not allow sodium chlorine chlorine is more reactive than bromine fluorine allow converse argument allow symbols Cl, Cl 2, Br and Br 2 allow chlorine / it is more reactive do not allow chloride or bromide allow F / F 2. do not allow fluoride. [5] 26 (a) Li and K either order allow lithium and potassium (b) Fe allow iron (c) N and As either order allow nitrogen and arsenic (d) Cu allow copper [4] 27 (a) (i) Neutron (top label) (ii) 3 Electron (bottom label) (iii) electrons Page 99 of 08