3.1.3.4 States of matter 261 minutes 257 marks Page 1 of 30
Q1. (a) Describe the bonding in a metal. Explain why magnesium has a higher melting point than sodium. (4) (b) Why do diamond and graphite both have high melting points?............ (c) Why is graphite a good conductor of electricity?... (d) Why is graphite soft?......... (Total 10 marks) Q2. (a) The diagram below represents a part of the structure of sodium chloride. The ionic charge is shown on the centre of only one of the ions. On the diagram, mark the charges on the four negative ions. Page 2 of 30
What change occurs to the motion of the ions in sodium chloride when it is heated from room temperature to a temperature below its melting point? (b) Sodium chloride can be formed by reacting sodium with chlorine. Write an equation for this reaction. A chloride ion has one more electron than a chlorine atom. In the formation of sodium chloride, from where does this electron come? (c) In some ionic compounds the chloride ions are polarised. What is a polarised chloride ion? What feature of a cation causes a chloride ion to become polarised? (d) What is a covalent bond? What property of the atoms joined by a covalent bond causes the bond to be polar? (Total 9 marks) Page 3 of 30
Q3. The table below shows some values of melting points and some heat energies needed for melting. Substance I 2 NaCl HF HCl HI Melting point/k 387 1074 190 158 222 Heat energy for melting /kj mol 1 7.9 28.9 3.9 2.0 2.9 (a) Name three types of intermolecular force. Force 1... Force 2... Force 3... (b) Describe the bonding in a crystal of iodine. Name the crystal type which describes an iodine crystal. (iii) Explain why heat energy is required to melt an iodine crystal. (4) (c) In terms of the intermolecular forces involved, suggest why hydrogen fluoride requires more heat energy for melting than does hydrogen chloride, hydrogen iodide requires more heat energy for melting than does hydrogen chloride. (5) Page 4 of 30
(d) Explain why the heat energy required to melt sodium chloride is large. The heat energy needed to vaporise one mole of sodium chloride (171 kj mol 1 ) is much greater than the heat energy required to melt one mole of sodium chloride. Explain why this is so. (e) In terms of its structure and bonding, suggest why graphite has a very high melting point.......... (Total 17 marks) Q4. (a) Predict the shapes of the SF 6 molecule and the ion. Draw diagrams of these species to show their three-dimensional shapes. Name the shapes and suggest values for the bond angles. Explain your reasoning. (8) (b) Perfume is a mixture of fragrant compounds dissolved in a volatile solvent. When applied to the skin the solvent evaporates, causing the skin to cool for a short time. After a while, the fragrance may be detected some distance away. Explain these observations. (4) (Total 12 marks) Q5. (a) The table below gives the melting point for each of the Period 3 elements Na Ar. Element Na Mg Al Si P S Cl Ar Melting point / K 371 923 933 1680 317 392 172 84 In terms of structure and bonding, explain why silicon has a high melting point, and why the melting point of sulphur is higher than that of phosphorus. (7) Page 5 of 30
(b) Draw a diagram to show the structure of sodium chloride. Explain, in terms of bonding, why sodium chloride has a high melting point. (4) (c) Give the conditions under which, if at all, beryllium and magnesium react with water. For any reaction that occurs, state one observation you would make and write an equation. (4) (Total 15 marks) Q6. (a) Iodine and graphite crystals both contain covalent bonds and yet the physical properties of their crystals are very different. For iodine and graphite, state and explain the differences in their melting points and in their electrical conductivities. (9) (b) Draw the shape of the BeCl 2 molecule and explain why it has this shape. State and explain the effect that an isolated Be 2+ ion would have on an isolated Cl ion and explain how this effect would lead to the formation of a covalent bond. Give one chemical property of Be(OH) 2 which is atypical of the chemistry of Group II hydroxides. (6) (Total 15 marks) Q7. Iodine and diamond are both crystalline solids at room temperature. Identify one similarity in the bonding, and one difference in the structures, of these two solids. Explain why these two solids have very different melting points. (Total 6 marks) Q8. Diamond and graphite are both forms of carbon. Diamond is able to scratch almost all other substances, whereas graphite may be used as a lubricant. Diamond and graphite both have high melting points. Explain each of these properties of diamond and graphite in terms of structure and bonding. Give one other difference in the properties of diamond and graphite. (Total 9 marks) Page 6 of 30
Q9. Phosphorus exists in several different forms, two of which are white phosphorus and red phosphorus. White phosphorus consists of P 4 molecules, and melts at 44 C. Red phosphorus is macromolecular, and has a melting point above 550 C. Explain what is meant by the term macromolecular. By considering the structure and bonding present in these two forms of phosphorus, explain why their melting points are so different. (Total 5 marks) Q10. The table below shows the electronegativity values of some elements. Fluorine Chlorine Bromine Iodine Carbon Hydrogen Electronegativity 4.0 3.0 2.8 2.5 2.5 2.1 (a) Define the term electronegativity.......... (b) The table below shows the boiling points of fluorine, fluoromethane (CH 3 F ) and hydrogen fluoride. F F H F Boiling point/k 85 194 293 Name the strongest type of intermolecular force present in: Liquid F 2... Liquid CH 3 F... Liquid HF... Explain how the strongest type of intermolecular force in liquid HF arises. (6) Page 7 of 30
(c) The table below shows the boiling points of some other hydrogen halides. HCl HBr HI Boiling point / K 188 206 238 Explain the trend in the boiling points of the hydrogen halides from HCl to HI. Give one reason why the boiling point of HF is higher than that of all the other hydrogen halides. (Total 11 marks) Q11. (a) The diagram below shows the melting points of some of the elements in Period 3. On the diagram, use crosses to mark the approximate positions of the melting points for the elements silicon, chlorine and argon. Complete the diagram by joining the crosses. By referring to its structure and bonding, explain your choice of position for the melting point of silicon. Page 8 of 30
(iii) Explain why the melting point of sulphur, S 8, is higher than that of phosphorus, P 4 (8) (b) State and explain the trend in melting point of the Group II elements Ca Ba. Trend... Explanation......... (Total 11 marks) Q12. At room temperature, both sodium metal and sodium chloride are crystalline solids which contain ions. (a) On the diagrams for sodium metal and sodium chloride below, mark the charge for each ion. (b) Explain how the ions are held together in solid sodium metal. Explain how the ions are held together in solid sodium chloride. (iii) The melting point of sodium chloride is much higher than that of sodium metal. What can be deduced from this information? Page 9 of 30
(c) Compare the electrical conductivity of solid sodium metal with that of solid sodium chloride. Explain your answer. Comparison...... Explanation......... (d) Explain why sodium metal is malleable (can be hammered into shape)....... (e) Sodium chlorate(v), NaClO 3, contains 21.6% by mass of sodium, 33.3% by mass of chlorine and 45.1% by mass of oxygen. Use the above data to show that the empirical formula of sodium chlorate(v) is NaClO 3 Sodium chlorate(v) may be prepared by passing chlorine into hot aqueous sodium hydroxide. Balance the equation for this reaction below.... Cl 2 +... NaOH... NaCl + NaClO 3 + 3H 2 O (Total 12 marks) Page 10 of 30
Q13. The table below shows the electronegativity values of some elements. H C N O Electronegativity 2.1 2.5 3.0 3.5 (a) State the meaning of the term electronegativity.......... (b) State the strongest type of intermolecular force in the following compounds. Methane (CH 4 )... Ammonia (NH 3 )... (c) Use the values in the table to explain how the strongest type of intermolecular force arises between two molecules of ammonia................ (d) Phosphorus is in the same group of the Periodic Table as nitrogen. A molecule of PH 3 reacts with an H + ion to form a PH 4+ ion. Name the type of bond formed when PH 3 reacts with H + and explain how this bond is formed. Type of bond... Explanation......... Page 11 of 30
(e) Arsenic is in the same group as nitrogen. It forms the compound AsH 3 Draw the shape of an AsH 3 molecule, including any lone pairs of electrons. Name the shape made by its atoms. Shape Name of shape... (f) The boiling point of AsH 3 is 62.5 C and the boiling point of NH 3 is 33.0 C. Suggest why the boiling point of AsH 3 is lower than that of NH 3......... (g) Balance the following equation which shows how AsH 3 can be made.... AsCl 3 +... NaBH 4... AsH 3 +... NaCl +... BCl 3 (Total 14 marks) Q14. (a) Complete the electronic configuration for the sodium ion, Na + ls 2... (b) Write an equation, including state symbols, to represent the process for which the energy change is the second ionisation energy of sodium. Page 12 of 30
Explain why the second ionisation energy of sodium is greater than the second ionisation energy of magnesium. (iii) An element X in Period 3 of the Periodic Table has the following successive ionisation energies. First Second Third Fourth Ionisation energies / kj mol 1 577 1820 2740 11600 Deduce the identity of element X. (c) State and explain the trend in atomic radius of the Period 3 elements from sodium to chlorine. Trend... Explanation......... (d) Explain why sodium has a lower melting point than magnesium............. Page 13 of 30
(e) Sodium reacts with ammonia to form the compound NaNH 2 which contains the NH 2 ion. Draw the shape of the NH 2 ion, including any lone pairs of electrons. Name the shape made by the three atoms in the NH 2 ion. Shape of NH 2 Name of shape... (f) In terms of its electronic configuration, give one reason why neon does not form compounds with sodium.... (Total 16 marks) Q15. Iodine and graphite are both solids. When iodine is heated gently a purple vapour is seen. Graphite will not melt until the temperature reaches 4000 K. Graphite conducts electricity but iodine is a very poor conductor of electricity. (a) State the type of crystal structure for each of iodine and graphite............. Page 14 of 30
(b) Describe the structure of and bonding in graphite and explain why the melting point of graphite is very high......................... (4) (c) Explain why iodine vaporises when heated gently............. (d) State why iodine is a very poor conductor of electricity....... (Total 9 marks) Page 15 of 30
Q16. Water can be found as ice, water and steam. (a) The following diagram shows the arrangement of some of the water molecules in a crystal of ice. With reference to the structure shown above give one reason why ice is less dense than water.......... (b) Water and methane have similar relative molecular masses and both contain the element hydrogen. The table below gives some information about water and methane. H 2 O CH 4 M r 18.0 16.0 Melting point / K 273 91 State the strongest type of intermolecular force holding the water molecules together in the ice crystal. State the strongest type of intermolecular force in methane. Page 16 of 30
(iii) Give one reason why the melting point of ice is higher than the melting point of methane. (c) A molecule of H 2 O can react with an H + ion to form an H 3 O + ion. Draw and name the shape of the H 3 O + ion. Include any lone pairs of electrons. Shape of the H 3 O + ion Name of shape... Suggest a value for the bond angle in the H 3 O + ion. (iii) Identify one molecule with the same number of atoms, the same number of electrons and the same shape as the H 3 O + ion. (d) Water can also form the hydroxide ion. State the number of lone pairs of electrons in the hydroxide ion.... (Total 9 marks) Q17. There are several types of crystal structure and bonding shown by elements and compounds. (a) Name the type of bonding in the element sodium. Page 17 of 30
Use your knowledge of structure and bonding to draw a diagram that shows how the particles are arranged in a crystal of sodium. You should identify the particles and show a minimum of six particles in a twodimensional diagram. (b) Sodium reacts with chlorine to form sodium chloride. Name the type of bonding in sodium chloride. Explain why the melting point of sodium chloride is high. (Extra space)... (c) The table below shows the melting points of some sodium halides. NaCl NaBr NaI Melting point /K 1074 1020 920 Suggest why the melting point of sodium iodide is lower than the melting point of sodium bromide....... (Total 7 marks) Page 18 of 30
Q18. Trends in physical properties occur across all Periods in the Periodic Table. This question is about trends in the Period 2 elements from lithium to nitrogen. (a) Identify, from the Period 2 elements lithium to nitrogen, the element that has the largest atomic radius.... (b) State the general trend in first ionisation energies for the Period 2 elements lithium to nitrogen... Identify the element that deviates from this general trend, from lithium to nitrogen, and explain your answer. Element... Explanation....... (Extra space)..... (c) Identify the Period 2 element that has the following successive ionisation energies. First Second Third Fourth Fifth Sixth Ionisation energy / kj mol 1 1090 2350 4610 6220 37 800 47 000... Page 19 of 30
(d) Draw a cross on the diagram to show the melting point of nitrogen. (e) Explain, in terms of structure and bonding, why the melting point of carbon is high................ (Extra space)......... (Total 10 marks) Page 20 of 30
Q19. Fluorine forms compounds with many other elements. (a) Fluorine reacts with bromine to form liquid bromine trifluoride (BrF 3 ). State the type of bond between Br and F in BrF 3 and state how this bond is formed. Type of bond... How bond is formed...... (b) Two molecules of BrF 3 react to form ions as shown by the following equation. 2BrF 3 BrF 2 + + BrF 4 Draw the shape of BrF 3 and predict its bond angle. Include any lone pairs of electrons that influence the shape. Shape of BrF 3 Bond angle... Draw the shape of BrF 4 and predict its bond angle. Include any lone pairs of electrons that influence the shape. Shape of BrF 4 Bond angle... Page 21 of 30
(c) BrF 4 ions are also formed when potassium fluoride dissolves in liquid BrF 3 to form KBrF 4 Explain, in terms of bonding, why KBrF 4 has a high melting point................ (Extra space)...... (d) Fluorine reacts with hydrogen to form hydrogen fluoride (HF). State the strongest type of intermolecular force between hydrogen fluoride molecules... Draw a diagram to show how two molecules of hydrogen fluoride are attracted to each other by the type of intermolecular force that you stated in part (d). Include all partial charges and all lone pairs of electrons in your diagram. (e) The boiling points of fluorine and hydrogen fluoride are 188 C and 19.5 C respectively. Explain, in terms of bonding, why the boiling point of fluorine is very low.......... (Extra space)...... (Total 15 marks) Page 22 of 30
Q20. (a) Graphene is a new material made from carbon atoms. It is the thinnest and strongest material known. Graphene has a very high melting point and is an excellent conductor of electricity. Part of the structure of graphene is illustrated in the diagram. Deduce the type of crystal structure shown by graphene... Suggest why graphene is an excellent conductor of electricity......... (iii) Explain, in terms of its structure and bonding, why graphene has a high melting point......... (b) Titanium is also a strong material that has a high melting point. It has a structure similar to that of magnesium. State the type of crystal structure shown by titanium... Page 23 of 30
Explain, in terms of its structure and bonding, why titanium has a high melting point......... (c) Titanium can be hammered into objects with different shapes that have similar strengths. Suggest why titanium can be hammered into different shapes..... Suggest why these objects with different shapes have similar strengths..... (d) Magnesium oxide (MgO) has a melting point of 3125 K. Predict the type of crystal structure in magnesium oxide and suggest why its melting point is high. Type of crystal structure... Explanation............ (Total 13 marks) Page 24 of 30
Q21. The following table shows the electronegativity values of the elements from lithium to fluorine. Li Be B C N O F Electronegativity 1.0 1.5 2.0 2.5 3.0 3.5 4.0 (a) State the meaning of the term electronegativity....... (Extra space)..... Suggest why the electronegativity of the elements increases from lithium to fluorine....... (Extra space)..... (b) State the type of bonding in lithium fluoride. Explain why a lot of energy is needed to melt a sample of solid lithium fluoride. Bonding... Explanation......... (Extra space)...... (c) Deduce why the bonding in nitrogen oxide is covalent rather than ionic....... (Extra space)...... Page 25 of 30
(d) Oxygen forms several different compounds with fluorine. Suggest the type of crystal shown by OF 2.. Write an equation to show how OF 2 reacts with steam to form oxygen and hydrogen fluoride... (iii) One of these compounds of oxygen and fluorine has a relative molecular mass of 70.0 and contains 54.3% by mass of fluorine. Calculate the empirical formula and the molecular formula of this compound. Show your working. Empirical formula............. Molecular formula..... (4) (Total 14 marks) Page 26 of 30
Q22. Zinc forms many different salts including zinc sulfate, zinc chloride and zinc fluoride. (a) People who have a zinc deficiency can take hydrated zinc sulfate (ZnSO 4.xH 2 O) as a dietary supplement. A student heated 4.38 g of hydrated zinc sulfate and obtained 2.46 g of anhydrous zinc sulfate. Use these data to calculate the value of the integer x in ZnSO 4.xH 2 O Show your working...................... (b) Zinc chloride can be prepared in the laboratory by the reaction between zinc oxide and hydrochloric acid. The equation for the reaction is ZnO + 2HCl ZnCl 2 + H 2 O A 0.0830 mol sample of pure zinc oxide was added to 100 cm 3 of 1.20 mol dm 3 hydrochloric acid. Calculate the maximum mass of anhydrous zinc chloride that could be obtained from the products of this reaction......................... (4) Page 27 of 30
(c) Zinc chloride can also be prepared in the laboratory by the reaction between zinc and hydrogen chloride gas. Zn + 2HCl ZnCl 2 + H 2 An impure sample of zinc powder with a mass of 5.68 g was reacted with hydrogen chloride gas until the reaction was complete. The zinc chloride produced had a mass of 10.7 g. Calculate the percentage purity of the zinc metal. Give your answer to 3 significant figures......................... (4) (d) Predict the type of crystal structure in solid zinc fluoride and explain why its melting point is high................... (Total 14 marks) Page 28 of 30
Q23. In 2009 a new material called graphane was discovered. The diagram shows part of a model of the structure of graphane. Each carbon atom is bonded to three other carbon atoms and to one hydrogen atom. (a) Deduce the type of crystal structure shown by graphane.... (b) State how two carbon atoms form a carbon carbon bond in graphane....... (c) Suggest why graphane does not conduct electricity....... (d) Deduce the empirical formula of graphane.... (Total 4 marks) Page 29 of 30
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