Cambridge IGCSE Chemistry - 0620 - Core Paper 3 2022 Winter Zone 2

The structures of seven compounds or elements, A, B, C, D, E, F and G, are shown.



(a) 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 atoms of a Group VII element
.............................................................................................................................................. [1]
(ii) an element with a giant covalent structure
.............................................................................................................................................. [1]
(iii) a compound that turns anhydrous copper(II) sulfate blue
.............................................................................................................................................. [1]
(iv) an element that conducts electricity
.............................................................................................................................................. [1]
(v) an unsaturated hydrocarbon.
.............................................................................................................................................. [1]

(b) Describe a test for an unsaturated hydrocarbon.
test .................................................................................................................................................
observations ...............................................................................................................................
[2]

(c) Name the two products formed when compound A undergoes complete combustion.
1 ....................................................................................................................................................
2 ....................................................................................................................................................
[2]

(a) The table compares the percentage by mass of the elements in the Earth’s crust and in the Moon’s crust.

[Table_1]

Answer these questions using only the information in the table.

(i) Deduce the percentage by mass of the other elements in the Moon’s crust. ................................................................................................................................................................................. [1]

(ii) State which element is present in the Earth’s crust in the greatest percentage by mass. .................................................................................................................................................................................... [1]

(iii) Give two major differences in the composition of the Earth’s crust and in the Moon’s crust.
1 ..................................................................................................................................................................................
.....................................................................................................................................................................................
2 ..................................................................................................................................................................................
..................................................................................................................................................................................... [2]

(b) Complete the diagram to show the electron arrangement in a silicon atom. [2]

(c) Iron reacts with oxygen to form an oxide of iron with the formula $\text{Fe}_3\text{O}_4$.

(i) Complete the chemical equation for this reaction.
.....Fe + .....O$_2$ → Fe$_3$O$_4$ [2]

(ii) Complete these sentences about the extraction of iron from iron ore in a blast furnace using words from the list.

air decomposed dioxide hydrogen iron
monoxide oxidised reduced slag

The raw materials put into the blast furnace are iron ore, limestone and .................................. . Carbon monoxide reacts with iron(III) oxide to produce iron. In this reaction iron(III) oxide is .................................. .

Limestone decomposes to produce calcium oxide and carbon .................................. . Calcium oxide reacts with impurities in the iron ore to form .................................. . [4]

(d) Iron is converted to steel using oxygen and one other type of compound.

(i) Explain how the oxygen removes the carbon. .................................................................................................................................................................................... [1]

(ii) Choose from the list the name of the other type of compound used to convert iron into steel.

acidic oxide
alcohol
basic oxide
hydrocarbon

................................................................................................................................................................................. [1]

(iii) Steel is an alloy. Choose the diagram, J, K, L or M, which best represents an alloy. ................................................................................................................................................................................. [1]

This question is about fuels and energy production.

(a) Chemical reactions can be endothermic or exothermic.

State the meaning of the term endothermic.

.......................................................................................................................

....................................................................................................................... [1]

(b) The diagram shows the apparatus used to compare the energy released when 100 cm³ of water is heated by burning different liquid fuels, P, Q, R and S.



All conditions are kept the same, apart from the type of fuel and mass of fuel burned.

The results are shown.

[Table_1]

Deduce which fuel, P, Q, R or S, releases the least energy per gram.

....................................................................................................................... [1]

(c) Name a gas that is used as a fuel.

....................................................................................................................... [1]

(d) An energy level diagram for the burning of a fuel is shown.



Complete the diagram using these words:
• products
• reactants.
[1]

(e) The radioactive isotope $^{235}$U is used as a source of energy.

State one other use of radioactive isotopes.

....................................................................................................................... [1]

(a) The table shows some properties of four halogens.


(i) Complete the table by predicting:
● the density of iodine at room temperature and pressure
● the boiling point of astatine.

(ii) Predict the physical state of bromine at 20°C.
Give a reason for your answer.

(b) Bromine reacts with sulfur dioxide and water.

(i) Complete the chemical equation for this reaction.
$$\text{Br}_2 + \text{SO}_2 + \text{......}\text{H}_2\text{O} \to \text{H}_2\text{SO}_4 + \text{......}\text{HBr}$$ [2]

(ii) In this reaction both oxidation and reduction take place.

State the meaning of the term reduction.

(c) Concentrated aqueous hydrobromic acid releases fumes of acidic hydrogen bromide gas.

A long glass tube is set up as shown.



At first the blue litmus paper does not turn red.
After a short time the blue litmus paper turns red.

Explain these observations using the kinetic particle model.


 

This question is about air and fertilisers.

(a) Air contains nitrogen, oxygen, noble gases and carbon dioxide.
State the percentage of nitrogen in clean, dry air.
............................................................................................................................. [1]

(b) Polluted air contains oxides of nitrogen.
(i) Give one source of oxides of nitrogen in the air.
.................................................................................................................. [1]

(ii) State one adverse effect of oxides of nitrogen on health.
.................................................................................................................. [1]

(c) Many fertilisers contain nitrogen and potassium.
(i) Name one other element found in most fertilisers.
.................................................................................................................. [1]

(ii) Explain why farmers use fertilisers on fields where crops are to be grown.
.................................................................................................................. [1]

(iii) Describe a test for potassium ions.
test ...........................................................................................................
observations ............................................................................................ [2]

(a) Describe the reaction of excess dilute sulfuric acid with magnesium carbonate and with magnesium oxide. Give the names of the products and any observations.   [4]

• reaction with magnesium carbonate
• reaction with magnesium oxide

(b) State the colour change when excess aqueous sodium hydroxide is added to a solution of litmus in dilute sulfuric acid.   [2]

(c) (i) Describe how universal indicator can be used to find the pH of an acidic solution.   [2]

(ii) Choose the pH value that is acidic.

Draw a circle around your answer.

pH 2 pH 7 pH 10 pH 14 [1]

(d) The salt zinc chloride can be prepared by reacting hydrochloric acid with zinc oxide.

(i) Choose the type of reaction that occurs.

Draw a circle around your answer.

addition neutralisation polymerisation reduction [1]

(ii) The method for preparing pure dry crystals of zinc chloride is given.

Complete the missing steps 3 and 6.

1. Add excess zinc oxide to dilute hydrochloric acid.
2. Warm the mixture to complete the reaction.
3. .......................................................................................................................................................................
4. Evaporate the filtrate until the point of crystallisation and leave for crystals to form.
5. Remove the crystals.
6.  ....................................................................................................................................................................... [2]

(e) (i) Small pieces of zinc react with excess dilute hydrochloric acid at different temperatures. The time taken for each reaction to finish is recorded.

The temperatures are:
• 20°C
• 40°C
• 60°C

All other conditions stay the same.

Complete the table by writing the temperatures in the first column.  [1]

(ii) Describe the effect on the time taken for the reaction to finish when it is carried out with dilute hydrochloric acid of a higher concentration.

All other conditions stay the same.   [1]

(a) The structure of compound T is shown.

(i) Choose from the list the word that describes compound T.
alcohol
alkane
alkene
carboxylic acid
............................................................................................................................... [1]
(ii) Deduce the formula of compound T to show the number of carbon, hydrogen and oxygen atoms.
............................................................................................................................... [1]
(b) Compound T reacts with ethanol in the presence of a catalyst.
(i) State the meaning of the term catalyst.
............................................................................................................................... [1]
(ii) Complete the sentence about ethanol using a word from the list.
combustion cracking electrolysis fermentation
Ethanol is manufactured from ethene or by .............................................. . [1]
(c) Ethene can be produced from ethanol.
(i) Draw the structure of ethene to show all of the atoms and all of the bonds.
............................................................................................................................... [1]
(ii) Ethene is a gas at room temperature.
Use the kinetic particle model to describe the separation of the particles in a gas.
............................................................................................................................... [1]
(iii) Ethene can be produced by cracking long-chain hydrocarbons to form short-chain hydrocarbons.
Explain why long-chain hydrocarbons are cracked to form short-chain hydrocarbons.
...............................................................................................................................
............................................................................................................................... [1]
(iv) Ethene can be polymerised.
State the name of the polymer formed.
............................................................................................................................... [1]
(d) Terylene is a polymer.
Give one use of Terylene.
............................................................................................................................... [1]
(e) Name a polymer that is a constituent of food.
............................................................................................................................... [1]

This question is about metals.

(a) Chromium is a transition element. Potassium is an element in Group I of the Periodic Table. Chromium has a higher density than potassium.
Give two other ways in which the physical properties of chromium differ from the physical properties of potassium.
1 ...............................................................
2 ............................................................... [2]

(b) The apparatus used to electroplate a nickel rod with chromium is shown.

(i) Choose a word from the list which describes the nickel rod.
Draw a circle around your answer.

anode, cathode, cation, electrolyte, mixture [1]

(ii) One use of electroplating is to make objects attractive.
Describe one other reason for electroplating an object.
....................................................................... [1]

(c) Deduce the number of electrons and neutrons in one atom of the isotope of chromium shown.
$$^{54}_{24}\text{Cr}$$

number of electrons ...................................................
number of neutrons ................................................... [2]

(d) A compound of chromium has the formula CrH₂O₆.
Complete the table to calculate the relative molecular mass of CrH₂O₆.

[Table_1]
| atom | number of atoms | relative atomic mass | |
|---------|-----------------|----------------------|-----------------| | chromium | 1 | 52 | 1 × 52 = 52 | | hydrogen | 1 | | | | oxygen | 16 | | | relative molecular mass = ........................................ [2]

(e) The table shows the rates of reaction of four metals with air.

[Table_2]
| metal | rate of reaction |
|----------|----------------------------------------------------------|
| chromium | reacts very slowly only when heated strongly |
| silver | does not react at room temperature or when heated strongly |
| sodium | reacts quickly at room temperature |
| uranium | reacts slowly at room temperature |

Put the four metals in order of their reactivity.
Put the least reactive metal first.

least reactive ................................................ most reactive [2]