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(a) The structures of seven compounds or elements, A, B, C, D, E, F and G, are shown.
Answer the following questions about these structures. Each structure may be used once, more than once or not at all.
State which structure, A, B, C, D, E, F or G, represents:
(i) a compound that contains an atom of an element in Group V of the Periodic Table [1]
(ii) an element [1]
(iii) a substance that is used for cutting tools [1]
(iv) a compound that is a major contributor to climate change [1]
(v) a saturated hydrocarbon. [1]
(b) Describe how aqueous bromine can be used to distinguish between a saturated hydrocarbon and an unsaturated hydrocarbon. [2]
(c) When a hydrocarbon undergoes incomplete combustion, carbon monoxide is formed.
(i) State the meaning of the term incomplete combustion. [1]
(ii) Give one adverse effect of carbon monoxide on health. [1]
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(a) The table compares the percentage by mass of the elements in the whole Earth and in the oceans.
[Table_1]
Answer these questions using only the information in the table.
(i) Deduce the percentage by mass of the other elements in the oceans.
................................................................................................................................................... [1]
(ii) State which non-metallic element is present in the whole Earth in the greatest percentage by mass.
................................................................................................................................................... [1]
(iii) Give \textbf{two} major differences in the composition of the whole Earth and of the oceans.
1 ...................................................................................................................................................
...................................................................................................................................................
2 ...................................................................................................................................................
................................................................................................................................................... [2]
(b) Complete the diagram to show the electron arrangement in a chlorine atom.
[2]
(c) Iron is extracted from iron(III) oxide in a blast furnace.
(i) Explain why air is blown into the blast furnace.
...................................................................................................................................................
................................................................................................................................................... [1]
(ii) In the blast furnace, carbon dioxide reacts with carbon to produce carbon monoxide.
Complete the chemical equation for this reaction.
\[ \text{CO}_{2} + \text{C} \rightarrow ......\text{CO} \] [1]
(iii) Carbon monoxide reduces iron(III) oxide to iron.
State the meaning of the term \textit{reduction}.
................................................................................................................................................... [1]
(iv) When 80 g of iron(III) oxide reacts with excess carbon monoxide, 56 g of iron is produced.
Calculate the minimum mass of iron(III) oxide needed to produce 14 g of iron.
............................. g [1]
(d) Steel is an alloy of iron.
(i) Choose \textbf{two} substances from the list that are used in the conversion of iron from the blast furnace into steel.
calcium oxide
carbon dioxide
hydrogen
nitrogen
oxygen
silicon(IV) oxide
sulfur dioxide
1 ...................................................................................................................................................
2 ................................................................................................................................................... [2]
(ii) State the meaning of the term \textit{alloy}.
...................................................................................................................................................
................................................................................................................................................... [1]
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(a) The diagram shows the apparatus used to compare the energy released when 100 cm³ of water is heated by burning different liquid fuels, J, K, L and M.
All conditions are kept the same apart from the type of fuel and mass of fuel burned.
The results are shown.
Deduce which fuel, J, K, L or M, releases the most energy per gram. [1]
(b) The fractional distillation of petroleum produces fractions, such as gasoline and diesel, which are used as fuels.
(i) Name one other petroleum fraction that is used as a fuel. [1]
(ii) State the physical property on which the fractional distillation of petroleum depends. [1]
(iii) Bitumen is a fraction of petroleum.
Write an X on the diagram to show where bitumen is obtained. [1]
(c) (i) Name a radioactive element that is used as a source of energy in nuclear power stations. [1]
(ii) State one other industrial use of radioactive isotopes. [1]
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(a) The table shows some properties of four Group I elements.
[Table]
\begin{tabular}{|c|c|c|c|}\hline \text{element} & \begin{array}{c}\text{melting point} \\ (^\circ C) \end{array} & \begin{array}{c}\text{boiling point} \\ (^\circ C) \end{array} & \begin{array}{c}\text{hardness} \\ \text{(MPa)} \end{array} \\ \hline \text{lithium} & 181 & 1342 & 5.00 \\ \hline \text{sodium} & 98 & \cdots & 0.70 \\ \hline \text{potassium} & 63 & 760 & 0.36 \\ \hline \text{rubidium} & 39 & 686 & \cdots \\ \hline \end{tabular}
(i) Complete the table by predicting:
• the boiling point of sodium
• the hardness of rubidium. [2]
(ii) Predict the physical state of potassium at 50°C. Give a reason for your answer.
..............................................................................................................................
.............................................................................................................................. [2]
(b) When a mixture of sodium and sodium hydroxide is heated, sodium oxide and hydrogen are formed.
(i) Complete the chemical equation for this reaction.
......Na + 2NaOH \rightarrow ......Na_2O + H_2 [2]
(ii) Describe a test for hydrogen.
test ........................................................................................................................
observations .............................................................................................. [2]
(c) Sodium hydroxide is used to make the red dye alizarin. Alizarin is soluble in ethanol.
A crystal of alizarin is placed in a beaker of ethanol.
After a few hours, the red colour has spread throughout the beaker.
Explain these observations using the kinetic particle model.
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This question is about compounds of nitrogen and fertilisers.
(a) Ammonium chloride is heated with sodium hydroxide.
$$\text{NH}_4\text{Cl} + \text{NaOH} \rightarrow \text{NH}_3 + \text{NaCl} + \text{H}_2\text{O}$$
Choose from the list the word that describes this reaction.
Draw a circle around your answer.
addition displacement oxidation reduction [1]
(b) Ammonia is manufactured from nitrogen and hydrogen.
$$\text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3$$
(i) Give the meaning of the symbol $\rightleftharpoons$.
...................................................................................................................................... [1]
(ii) The nitrogen for this process is obtained from the air.
State the percentage of nitrogen in clean, dry air.
...................................................................................................................................... [1]
(c) Fertilisers contain nitrogen.
Name two other elements found in most fertilisers that are essential for plant growth.
...................................................... and ........................................................ [2]
(d) Bacteria in the soil can convert ammonium ions into oxides of nitrogen.
Oxides of nitrogen contribute to acid rain.
(i) Name one other pollutant in the air that contributes to acid rain.
...................................................................................................................................... [1]
(ii) State one adverse effect of acid rain on buildings.
...................................................................................................................................... [1]
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(a) Describe the reaction of excess dilute hydrochloric acid with magnesium and with magnesium carbonate. Give the names of the products and any observations.
(i) reaction with magnesium
• products
• observations
(ii)reaction with magnesium carbonate
• products
• observations
(b) (i) Different sized pieces of magnesium react with excess dilute hydrochloric acid. The time taken for each reaction to finish is recorded.
The sizes of the pieces of magnesium are:
• large
• small
• very small.
Equal masses of magnesium are used in each reaction.
All other conditions stay the same.
Complete the table by writing the size of the magnesium pieces in the first column.
(b) (ii) Describe the effect on the time taken for small pieces of magnesium to react with hydrochloric acid of a lower concentration.
All other conditions stay the same.
(c) (i) Sodium hydroxide is an alkali.
State the colour change when excess aqueous sodium hydroxide is added to a solution of methyl orange in acid.
from ..................... to ..................
(c) (ii) Choose the pH value of an alkali.
Draw a circle around your answer.
pH=3 pH=5 pH=7 pH=14
(d) (i) The salt magnesium chloride can be prepared by reacting hydrochloric acid with magnesium oxide.
The method for preparing pure dry crystals of magnesium chloride is given.
Complete the missing steps 4 and 6.
1 Add excess magnesium oxide to dilute hydrochloric acid.
2 Warm the mixture to complete the reaction.
3 Filter off the excess magnesium oxide and collect the filtrate.
4 ....................................................................................................................................
5 Remove the crystals.
6 ....................................................................................................................................
(d) (ii) Magnesium oxide is used as a catalyst in some reactions.
State the purpose of using a catalyst.
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(a) The structure of an organic compound, S, is shown.
(i) On the structure, draw a circle around the carboxylic acid functional group. [1]
(ii) Deduce the formula of compound S to show the number of carbon, hydrogen, and oxygen atoms. [1]
(iii) Compound S is a solid at room temperature.
Use the kinetic particle model to describe the arrangement of the particles in a solid. [1]
(b) Compound S reacts with ethanol.
(i) Draw the structure of ethanol to show all of the atoms and all of the bonds. [1]
(ii) Ethanol can be manufactured by fermentation.
Describe one other method of manufacturing ethanol. [2]
(c) Compound S can be polymerised.
(i) State the general name given to the small units that join together to form a polymer. [1]
(ii) Name one natural polymer. [1]
(iii) Some plastics are non-biodegradable.
Describe one pollution problem caused by non-biodegradable plastics. [1]
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This question is about metals.
(a) (i) Copper is a transition element. Sodium is an element in Group I of the Periodic Table. Copper is harder than sodium.
Give two other ways in which the physical properties of copper differ from the physical properties of sodium.
1 .................................................................................................................................
2 ................................................................................................................................. [2]
(ii) Give one use of copper.
................................................................................................................................. [1]
(b) The apparatus used to electroplate a steel spoon with copper is shown.
(i) Label the diagram to show:
• the anode
• the electrolyte. [2]
(ii) Describe the observations made during this electroplating at the:
steel spoon ....................................................................................................................
.................................................................................................................................
copper rod. ....................................................................................................................
................................................................................................................................. [2]
(c) Deduce the number of electrons and neutrons in one atom of the isotope of copper shown.
$$^{65}_{29}Cu$$
number of electrons ...................................................................................................
number of neutrons ................................................................................................... [2]
(d) A compound of copper has the formula $K_2CuF_4$.
Complete the table to calculate the relative molecular mass of $K_2CuF_4$.
[Table_1]
relative molecular mass = .............................. [2]
(e) The table shows the rates of reaction of four metals with steam.
[Table_2]
Put the four metals in order of their reactivity. Put the least reactive metal first.
least reactive _________________ __________________ __________________ most reactive [2]
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