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1. A list of symbols and formulae is shown: $\text{Br}_2$, $\text{CH}_4$, $\text{C}_2\text{H}_4$, $\text{Cl}^-$, $\text{CO}_2$, $\text{Cr}^{3+}$, $\text{Cu}^{2+}$, $\text{H}_2$, $\text{K}^+$, $\text{N}_2$, $\text{N}_3^-$, $\text{O}_2$, $\text{SO}_4^{2-}$. Answer the following questions about these symbols and formulae. Each symbol or formula may be used once, more than once or not at all.
(a) State which symbol or formula represents a molecule containing only five atoms. [1]
(b) A diatomic molecule of an element in Group VII of the Periodic Table. [1]
(c) An ion formed when an atom gains one electron. [1]
(d) An ion which forms a green precipitate when a few drops of aqueous sodium hydroxide are added to it. [1]
(e) A compound produced by the thermal decomposition of calcium carbonate. [1]
(f) A product of photosynthesis. [1]
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2. (a) A sample of soil is shaken with distilled water. Draw a diagram to show the filtration apparatus used to separate the soil from the solution obtained by shaking the soil with distilled water. On your diagram, label: the filtrate, the residue. [3]
(b) Table 2.1 shows the masses of some of the ions in 1000 cm$^3$ of the solution obtained by filtering a sample of soil with distilled water.
[Table_1]
Answer these questions using the information in Table 2.1.
(i) Name the negative ion that has the lowest concentration. [1]
(ii) State the name of the $\text{SO}_4^{2-}$ ion. [1]
(iii) Calculate the mass of phosphate ions in 200 cm$^3$ of the solution. [1]
(c) Complete Fig. 2.1 to show: the electronic configuration of a sodium ion, the charge on the ion.
[2]
(d) Water from natural sources contains dissolved gases. Choose from the list the gas which is essential for aquatic life. Draw a circle around your chosen answer. [1]
(e) Polluted water may contain sewage or nitrates. State one harmful effect of each of these water pollutants. [2]
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3. This question is about compounds of nitrogen.
(a) Complete the dot-and-cross diagram in Fig. 3.1 of a molecule of ammonia. Show outer shell electrons only.
[2]
(b) Oxides of nitrogen are air pollutants.
(i) State one source of oxides of nitrogen in the air. [1]
(ii) State one adverse effect of oxides of nitrogen. [1]
(c) State whether nitrogen dioxide is an acidic or basic oxide. Give a reason for your answer. [1]
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4. This question is about metals and compounds of metals.
(a) Table 4.1 shows some properties of five metals, A, B, C, D and E. [Table_2]
State which two of these metals, A, B, C, D and E, are transition elements. Give two reasons for your answer using only the information in Table 4.1. [3]
(b) Choose the metal chloride that is insoluble in water. Tick (✓) one box. [1]
(c) Magnesium chloride is produced when magnesium burns in chlorine.
$\text{Mg} + \text{Cl}_2 → \text{MgCl}_2$
Fig. 4.1 shows an incomplete reaction pathway diagram for this reaction.
(i) Complete Fig. 4.1 by writing these formulae on the diagram: $\text{Mg} + \text{Cl}_2$, $\text{MgCl}_2$. [1]
(ii) Explain how Fig. 4.1 shows that the reaction is exothermic. [1]
(d) Table 4.2 shows the reactions of four different metals with steam. [Table_3]
Put the four metals in order of their reactivity. Put the least reactive metal first. [2]
(e) A compound of nickel has the molecular formula $\text{NiP}_4\text{F}_{12}$. Complete Table 4.3 to calculate the relative molecular mass of $\text{NiP}_4\text{F}_{12}$. [2]
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5. Potassium iodide is an ionic compound.
(a) State two properties of an ionic compound. [2]
(b) Molten potassium iodide is electrolysed using graphite electrodes.
(i) Name the products formed at the positive and negative electrodes. [2]
(ii) State the name of the positive electrode in an electrolysis experiment. [1]
(c) Deduce the number of protons and neutrons in the iodide ion shown. $^{127}\text{I}^-$ $^{53}$ [2]
(d) Aqueous chlorine reacts with aqueous potassium iodide.
(i) Complete the symbol equation for this reaction. $\text{Cl}_2 + 2\text{KI} →$ ...... + ....$\text{KCl}$ [2]
(ii) Choose from the list the name of this type of reaction. Draw a circle around your chosen answer. [1]
(iii) State the colour of chlorine gas at room temperature and pressure. [1]
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6. (a) Fig. 6.1 shows the displayed formula of a molecule of crotyl alcohol.
(i) On Fig. 6.1 draw a circle around the alcohol functional group. [1]
(ii) Describe the feature of crotyl alcohol that shows it is an unsaturated compound. [1]
(iii) Deduce the molecular formula of crotyl alcohol. [1]
(iv) Crotyl alcohol is soluble in water. The boiling point of crotyl alcohol is 121 °C. The boiling point of water is 100 °C. Suggest how fractional distillation can be used to separate a mixture of crotyl alcohol and water. [2]
(b) Ethanol is also an alcohol. Describe two conditions for the manufacture of ethanol by the fermentation of aqueous glucose. [2]
(c) Ethanol can be converted to ethene. Choose from the list the general formula for the homologous series to which ethene belongs. Draw a circle around your chosen answer. [1]
(d) Ethene can be converted to ethane.
(i) Ethane is an alkane. Name the type of bonding in alkanes. [1]
(ii) Draw the displayed formula of a molecule of ethane. [1]
(iii) Complete this sentence. Alkanes are unreactive except in terms of combustion and substitution by ......... . [1]
(iv) Complete the symbol equation for the complete combustion of methane. $\text{CH}_4 +$ .....$\text{O}_2 \rightarrow$ ...... + $2\text{H}_2\text{O}$ [2]
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7. This question is about iron.
(a) Iron is extracted from iron ore in a blast furnace.
(i) Name the main ore of iron. [1]
(ii) The main ore of iron contains iron(III) oxide. Describe the extraction of iron from iron ore in the blast furnace. In your answer, describe:
- the production of carbon monoxide [4]
- the role of carbon monoxide
- the role of calcium carbonate, added to the blast furnace.
(iii) Iron collects at the base of the blast furnace as a liquid. Describe the arrangement and motion of the particles in a liquid. [2]
(b) The equation for the reaction of iron with steam is shown. $3\text{Fe} + 4\text{H}_2\text{O} \rightarrow \text{Fe}_3\text{O}_4 + 4\text{H}_2$
Describe how this equation shows that iron is oxidised. [1]
(c) Rust is hydrated iron(III) oxide.
(i) Define the term hydrated. [1]
(ii) Name the two substances needed for iron to rust. [2]
(d) Crystals of iron(II) chloride can be prepared by adding excess iron to dilute hydrochloric acid.
(i) Suggest how the unreacted iron is removed from the reaction mixture. [1]
(ii) Describe how dry crystals of iron(II) chloride are made from a dilute solution of iron(II) chloride. [2]
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8. A student investigates the reaction of iron powder with dilute hydrochloric acid at 20 °C. The hydrochloric acid is in excess.
(a) Fig. 8.1 shows the volume of hydrogen gas released as the reaction proceeds.
(i) Deduce the volume of hydrogen gas released after 2 minutes. [1]
(ii) The student repeats the experiment using dilute hydrochloric acid of a higher concentration. All other conditions stay the same. Draw a line on the grid in Fig. 8.1 to predict how the volume of hydrogen gas changes when dilute hydrochloric acid of a higher concentration is used. [2]
(b) (i) The student repeats the experiment with large pieces of iron. All other conditions stay the same. Describe how the rate of reaction differs when large pieces of iron are used. [1]
(ii) The student repeats the experiment with iron powder at a temperature of 15 °C. All other conditions stay the same. Describe how the rate of reaction differs when a temperature of 15 °C is used. [1]
(c) Hydrochloric acid also reacts with aqueous sodium hydroxide.
(i) Complete the word equation for this reaction. hydrochloric acid + sodium hydroxide → .... + .... [2]
(ii) Write the formula of the ion present in all acids. [1]
(iii) Choose from the list a possible pH value of aqueous sodium hydroxide. Draw a circle around your chosen answer. [1]
(iv) State the colour of methyl orange in aqueous sodium hydroxide. [1]
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