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The diagram shows part of the Periodic Table. Only some of the elements are shown.
(a) Answer the following questions using only the elements shown in the diagram.
Each element may be used once, more than once or not at all.
(i) Which element has a giant covalent structure? .............................. [1]
(ii) Which element has the highest relative atomic mass? ................... [1]
(iii) Which two elements are formed when molten aluminium oxide is electrolysed?
........................... and ........................... [1]
(iv) Which element in Group I reacts most rapidly with water? ................... [1]
(v) Which element oxidises in the presence of water to form rust? ...................[1]
(vi) Which element burns in oxygen to form water? .................... [1]
(b) Rubidium reacts with oxygen to form rubidium oxide, $\text{Rb}_2\text{O}$.
Complete the symbol equation for this reaction.
....Rb + ...... $\rightarrow$ 2$\text{Rb}_2\text{O}$ [2]
(c) Lead compounds are atmospheric pollutants.
State one adverse effect of lead compounds on health.
................................. [1]
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Carbon dioxide can be prepared in the laboratory using the apparatus shown below.
(a) State the names of the pieces of apparatus labelled A and B.
A ............................................................................................................
B ............................................................................................................ [2]
(b) Complete the word equation for this reaction.
calcium carbonate + hydrochloric acid $\rightarrow$ ...................... + carbon dioxide + ......................
........................ [2]
(c) Carbon dioxide is slightly soluble in water. What effect will this have on the volume of carbon dioxide collected? Tick one box.
The volume is lower than expected. □
The volume is higher than expected. □
The volume is the same as expected. □
No carbon dioxide is collected. □ [1]
(d) A burning candle is lowered into a beaker of carbon dioxide.
(i) The flame goes out. Explain why the flame goes out.
.................................................................................................... [1]
(ii) After 20 seconds, the candle is removed and relit. It is then lowered into the same beaker again. The flame goes out again.
What does this tell you about the density of carbon dioxide compared to air?
.................................................................................................... [1]
(iii) After 40 minutes, the candle is removed and relit. It is then lowered into the same beaker again. The candle stays alight.
Explain why the candle stays alight.
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529
598
River water contains a variety of ions and gases, and insoluble materials such as soil particles.
(a) Describe how you could remove the insoluble materials from a sample of river water. Include a labelled diagram.
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(b) The table shows the ions present in a sample of river water.
[Table_1]
name of ion | formula of ion | concentration in mg/dm³
calcium | Ca^{2+} | 0.6
chloride | Cl^{-} | 14.0
hydrogen carbonate | HCO_3^{-} | 1.5
iron(III) | Fe^{3+} | 0.5
magnesium | Mg^{2+} | 1.0
potassium | K^{+} | 3.0
sodium | Na^{+} | 11.0
| SO_4^{2-} | 0.4
(i) Which ion with a charge of 2+ is present in the highest concentration?
..................................................................................................................................... [1]
(ii) State the name of the ion with the formula $SO_4^{2-}$.
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(iii) Calculate the total mass of ions present in 1 dm³ of river water.
.................. mg [1]
(iv) Use your answer to part (iii) to calculate the total mass of ions in 50 cm³ of river water.
.................. mg [1]
(v) A student evaporated the sample of river water to leave a solid containing a number of different compounds. Use the information in the table to suggest the name of the compound present in the greatest amount.
..................................................................................................................................... [1]
(c) The table shows the solubility of oxygen in river water at different temperatures.
[Table_2]
temperature /°C | solubility in mg/dm³
0 | 11.0
10 | 8.8
20 | 7.2
30 | 6.0
40 | 4.9
50 | 4.2
60 | 3.6
(i) On the axes below, plot a graph to show how the solubility of oxygen changes with temperature. Draw a curve of best fit through the points.
[Graph_1]
[3]
(ii) Deduce the solubility of oxygen in river water at 25°C.
..................................................................................................................................... [1]
(iii) State the approximate percentage of oxygen in the air.
..................................................................................................................................... [1]
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The alkanes are a homologous series of hydrocarbons.
(a) Name another homologous series of hydrocarbons. [1]
(b) The graph below shows how the melting points of the first eight alkanes vary with the number of carbon atoms.
(i) Describe how the melting points of these alkanes vary with the number of carbon atoms. [2]
(ii) On the graph above, continue the line to show the melting points of the hydrocarbons having 9 and 10 carbon atoms. [2]
(c) The first member of the alkane homologous series is methane.
(i) State one source of the methane in the atmosphere. [1]
(ii) State one adverse effect of methane in the atmosphere. [1]
(d) Complete the symbol equation to show the complete combustion of methane.
$\text{CH}_4 + ....\text{O}_2 \rightarrow ....... + 2\text{H}_2\text{O}$ [2]
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Iron from a blast furnace contains carbon, sulfur, silicon and phosphorus as impurities.
(a) Iron is converted into steel in a basic oxygen converter. The impurities undergo oxidation. What is meant by the term oxidation?
........................................................................................................................... [1]
(b) Carbon is oxidised to carbon dioxide. Sulfur is oxidised to sulfur dioxide. Explain why these oxides are easily removed from the molten iron.
........................................................................................................................... [1]
(c) Phosphorus is converted to phosphorus(V) oxide.
(i) Complete the symbol equation for this reaction.
.....P + 5O$_2$ → 2P$_2$O$_5$ [1]
(ii) Is phosphorus(V) oxide an acidic or basic oxide? Give a reason for your answer.
........................................................................................................................... [1]
(d) Phosphorus(V) oxide is a solid. Explain how this oxide is removed from the molten iron.
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(e) Steel is an alloy.
(i) State one use of:
mild steel, .........................................................................................................
stainless steel. ................................................................................................ [2]
(ii) Which diagram, A, B, C or D, best represents an alloy? Put a ring around the correct answer. [1]
(f) The table shows the composition of some different brasses.
[Table_1]
How does the composition of brass affect its strength?
........................................................................................................................... [1]
(g) A student dissolved a sample of brass in concentrated nitric acid. Nitrogen dioxide, NO$_2$, was released.
Cu + 4HNO$_3$ → Cu(NO$_3$)$_2$ + 2NO$_2$ + 2H$_2$O
(i) Write a word equation for this reaction.
........................................................................................................................... [2]
(ii) The student added aqueous ammonia to the solution formed until the ammonia was in excess. Describe what the student would observe.
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(iii) State one source of the nitrogen dioxide in the atmosphere.
........................................................................................................................... [1]
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In the 1860s, John Newlands listed the elements in order of increasing atomic mass. Part of his table is shown.
[Table_1]
(a) (i) Describe the differences between Newlands’ table and the Periodic Table we use today.
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(ii) What evidence is there, from Newlands’ table, that some elements with similar properties are grouped together?
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(b) The table below shows some properties of some of the halogens.
[Table_2]
Deduce:
the colour of astatine, ...............................................................
the boiling point of bromine, ...............................................................
the state of iodine at 190°C. ..................................................... [3]
(c) Aqueous chlorine reacts with aqueous potassium bromide.
$Cl_2 + 2KBr \rightarrow Br_2 + 2KCl$
(i) Describe the colour change you would observe in this reaction.
.................................................................................................................... [1]
(ii) State the name of the salt formed in this reaction.
.................................................................................................................... [1]
(iii) Explain why aqueous bromine does not react with aqueous potassium chloride.
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(iv) The halogens exist as diatomic molecules.
What is meant by the term *diatomic*?
.................................................................................................................... [1]
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Ethanol is an alcohol.
(a) Complete the structure of ethanol showing all atoms and bonds.
[1]
(b) State the name of the products formed when ethanol undergoes incomplete combustion.
........................................................ and ...............................................................
[2]
(c) Ethanol can be manufactured by fermentation or by the hydration of ethene.
(i) Complete the word equation for the manufacture of ethanol from ethene.
ethene + ......................... → ethanol
[1]
(ii) What conditions are needed for the manufacture of ethanol from ethene?
Tick two boxes.
[ ] temperature above 100°C
[ ] room temperature
[ ] presence of inorganic catalyst
[ ] presence of yeast
[ ] presence of hydrogen
[2]
(iii) When ethanol is prepared by fermentation, the fermentation mixture produced contains ethanol and water.
The boiling point of ethanol is 78°C.
Describe how fractional distillation can be used to separate ethanol from water.
In your answer, refer to:
• the apparatus used,
• changes in state,
• differences in boiling points.
You may use a diagram.
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[5]
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510
