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The diagram shows the structures of five elements, A, B, C, D and E.
(a) Answer these questions using the letters A, B, C, D or E. Each element can be used once, more than once or not at all.
Which one of these elements
(i) is in Group V of the Periodic Table, .................................................. [1]
(ii) is used to fill weather balloons, .................................................. [1]
(iii) is a diatomic gas at room temperature, .................................................. [1]
(iv) conducts electricity, .................................................. [1]
(v) is a transition element? .................................................. [1]
(b) Which two of the elements A, B, C, D or E are simple molecules? .................................................. and .................................................. [2]
(c) Which two of the words or phrases in the list below describe the structure of element B?
covalent giant ionic
metallic simple atomic simple molecular
.................................................. and .................................................. [2]
(d) What do you understand by the term element? .................................................. [1]
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Ammonia, $\text{NH}_3$, is an alkaline gas.
(a) Describe a test for ammonia.
test ......................................................................................................................
result .................................................................................................................... [2]
(b) What is the pH of an aqueous solution of ammonia?
Put a ring around the correct answer.
pH1 pH3 pH5 pH7 pH9 [1]
(c) Ammonia reacts with hydrochloric acid.
(i) Complete the symbol equation for this reaction.
$\text{NH}_3 + \text{HCl} \rightarrow$ ............. [1]
(ii) Hydrochloric acid can be made by dissolving hydrogen chloride, HCl, in water.
Draw a diagram to show the arrangement of electrons in hydrogen chloride.
Show only the outer electrons.
Show a hydrogen electron as •
Show a chlorine electron as x [2]
(d) Aqueous ammonia reacts with sulfuric acid to form a solution of ammonium sulfate.
$$2\text{NH}_3(\text{aq}) + \text{H}_2\text{SO}_4(\text{aq}) \rightarrow (\text{NH}_4)_2\text{SO}_4(\text{aq})$$
(i) Ammonium sulfate is a colourless salt. Describe how you could use a titration method
to make a colourless solution of ammonium sulfate.
....................................................................................................................
....................................................................................................................
....................................................................................................................
....................................................................................................................
.................................................................................................................... [4]
(ii) How can crystals of ammonium sulfate be obtained from a solution of ammonium sulfate?
....................................................................................................................
.................................................................................................................... [1]
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The table below shows the properties of some halogens.
[Table_1]
(a)
(i) What is the trend in the colour of the halogens down the Group?
............................................................................................................................... [1]
(ii) Predict the state of fluorine at room temperature.
............................................................................................................................... [1]
(iii) Predict the melting point of chlorine.
............................................................................................................................... [1]
(b) The reactivity of three different halogens was compared by reacting them with solutions of sodium halides.
The results are shown in the table below.
[Table_2]
(i) Use the results in the table to suggest the order of reactivity of astatine, bromine, chlorine and iodine.
most reactive ______________________________________ least reactive
[2]
(ii) Predict whether bromine will react with sodium chloride solution. Explain your answer.
...............................................................................................................................
............................................................................................................................... [1]
(c) Chlorine reacts with excess cold dilute sodium hydroxide. The products of the reaction are sodium chloride, sodium chlorate(I) and water.
The formula of sodium chlorate(I) is NaClO.
Complete the equation for this reaction.
$$Cl_2 + ......NaOH \rightarrow NaCl + NaClO + .........$$
[2]
(d)
(i) Explain why chlorine is used in water purification.
............................................................................................................................... [1]
(ii) Impure water contains particles of minerals and remains of dead plants and animals. One stage in water purification is the removal of these particles by filtration.
The diagram below shows a water filter.
Explain how this water filter works.
...............................................................................................................................
...............................................................................................................................
...............................................................................................................................
[2]
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The process of distillation is used in an oil refinery to separate petroleum into different fractions.
(a) What do you understand by the term petroleum fraction?
...............................................................................................................................................
............................................................................................................................................... [2]
(b) Some petroleum fractions are more useful than others. There is a greater demand for these fractions. The diagram shows the demand from customers and the ability of an oil refinery to supply these fractions by fractional distillation alone.
(i) State the name of two fractions for which demand is greater than supply.
............................................................................................................................................... [2]
(ii) State one use for each of the following fractions.
refinery gas ..............................................................................................................................
bitumen .................................................................................................................................... [2]
(c) More gasoline can be made by cracking long-chain hydrocarbons.
State the conditions needed for cracking.
...............................................................................................................................................
............................................................................................................................................... [2]
(d) Dodecane, $C_{12}H_{26}$, can be cracked to form smaller hydrocarbons.
(i) What do you understand by the term hydrocarbon?
............................................................................................................................................... [1]
(ii) Complete the equation for the cracking of dodecane.
$C_{12}H_{26} \rightarrow C_{8}H_{18} +$ ............. [1]
(e) Ethene, $C_{2}H_{4}$, can be formed by cracking.
(i) Draw the full structure of ethene showing all atoms and bonds. [1]
(ii) Poly(ethene) can be made from ethene. Complete the following sentences using words from the list below.
addition atoms condensation dimers monomers polymers subtraction
The small ethene molecules which join together to form poly(ethene) are called ethene .............................. . The process of joining the ethene molecules together is an example of an .............................. reaction. The long-chain molecules which are formed are called .............................. . [3]
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Aluminium is in Group III of the Periodic Table. Iron is a transition element.
(a) Both aluminium and iron have high melting points and boiling points. State two differences in the physical properties of aluminium and iron.
...........................................................................................................................
........................................................................................................................... [2]
(b) State one use of aluminium.
............................................................................................................................. [1]
(c) Sodium hydroxide is used to test for aluminium ions. Describe what happens when you add a solution of sodium hydroxide to a solution of aluminium ions until the sodium hydroxide is in excess.
...........................................................................................................................
...........................................................................................................................
........................................................................................................................... [3]
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The diagram below shows a kiln used for manufacturing lime.
The reaction taking place in the kiln is
$\text{calcium carbonate} \rightarrow \text{calcium oxide} + \text{carbon dioxide (lime)}$
(a) (i) State the name of a rock which is largely calcium carbonate.
............................................................................................................ [1]
(ii) Explain why, at the end of the reaction, there is only lime left in the lime kiln.
............................................................................................................ [1]
(b) (i) Coke is mainly carbon. Combustion of coke provides the heat for the reaction in the lime kiln. Write a symbol equation for the complete combustion of carbon in oxygen.
............................................................................................................ [2]
(ii) Complete these sentences using words from the list below.
air dioxide harmless hydrogenated limited monoxide poisonous water
When carbon burns in a ............................. supply of .........................., carbon .......................... is formed. This is a colourless gas which has no smell and is ........................ . [4]
(c) Calcium carbonate reacts with hydrochloric acid to form carbon dioxide. Complete the word equation for this reaction.
$\text{calcium carbonate} + \text{hydrochloric acid} \rightarrow$
...............................................
............................................... + carbon dioxide [2]
(d) The speed of reaction of calcium carbonate with hydrochloric acid can be found using the apparatus shown below.
(i) Suggest how this apparatus can be used to find the speed of this reaction.
............................................................................................................
............................................................................................................
............................................................................................................ [2]
(ii) State how the speed of this reaction changes when the concentration of acid is increased, ...............................................................
larger pieces of calcium carbonate are used, ...................................................
the temperature is increased. ................................................................. [3]
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The structures of iodine and potassium iodide are shown below.
(a) Iodine is a solid at room temperature. Its melting point is +114°C.
(i) Describe what happens to the arrangement and movement of iodine molecules when iodine is gradually heated from 20°C to 120°C.
...............................................................................................................................................
...............................................................................................................................................
...............................................................................................................................................
...............................................................................................................................................
............................................................................................................................................... [4]
(ii) Calculate the relative molecular mass of iodine.
............................................................................................................................................... [1]
(b) (i) What type of bonding is present in potassium iodide?
............................................................................................................................................... [1]
(ii) Write the simplest formula for potassium iodide.
............................................................................................................................................... [1]
(c) Complete the table below to show the solubility in water and electrical conductivity of solid iodine and solid potassium iodide.
[Table_1]
[4]
(d) Predict the product formed at each electrode when molten potassium iodide is electrolysed.
at the positive electrode ............................................................................................................................
at the negative electrode ............................................................................................................................ [2]
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