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Copper (II)

carbonate

NAMA:............................................................. CLASS:4........

Section B ( 52%)

Answer all questions in this section. Write your answer in the spaces provided.

1 Table 1 shows the proton number and nucleon number of atom for the elements carbon,

oxygen, magnesium and sulphur.

Elements

Unsur

Carbon

Karbon

Oxygen

Oksigen

Magnesium

Magnesium

Sulphur

Sulfur

Proton number

Nombor proton6 8 12 16

Nucleon number

Nombor nukleon12 16 24 32

Table 1

a) What is meant by proton number?

.

( 1 mark)

b) State the type of particles consists in magnesium metal.

...

( 1 mark)

c) (i) Write the electron arrangement for sulphur atom .

..

( 1 mark)

ii) State the valence electron for sulphur atom.

( 1 mark)

d) Carbon-12 and Carbon-14 are the isotopes of carbon.

i) What is meant by isotopes?

.

( 1 mark)

ii) State the use of carbon-14 in archeology field.

.

( 1 mark)

e) Figure 1 shows the set-up of apparatus to study the heating of copper (II) carbonate.

Heat

Fi ure 1

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i) Complete the set-up of apparatus in Figure 1 to test the gas liberated when copper (II) carbonate

is heated.

( 2 marks)

ii) Write the chemical equation for the reaction that takes place.

( 2 marks)

iii) Draw the formation of chemical bond between Magnesium and Oxygen.

( 2 marks)

2. Table 2 shows the results of two tests done to hydrogen chloride in solvent X and solvent Y.

Test Hydrogen chloride in

Solvent X Solvent Y

A small piece of marble chip is

added into hydrogen chloride

No change Effervescence occurs. A

colourless gas is liberated

Reaction with blue litmus paper No change The colour of blue litmus

paper turns red.

Table 2

a) Name the type of particles of hydrogen chloride found in

i) Solvent X:...............................................................

ii) Solvent Y:...............................................................

( 2 marks)

b) Suggest a name for solvent Y.

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

( 1 mark)

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c) Explain why hydrogen chloride in solvent Y produce colourless gas while no change is

observed when hydrogen chloride is in solvent X.

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

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

( 2 marks)

d) Flow chart in diagram 3.2 shows a series of chemical changes of salt Q.

i) Name solid U.

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

( 1 mark)

ii) Write the chemical equation to represent the reaction when salt Q is heated.

....( 2 marks)

e) Solution Z is produced when solid U is reacted with dilute sulphuric acid.

Describe the confirmatory test for the cation presents in solution Z.

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

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

( 2 marks)

3. Diagram below shows the set-up of apparatus for two types of cells.

a) Name the type of cells in cell 1 and cell 2.

Salt Q

Solid U + nitrogen dioxide + oxygen

(Solid U is yellow when hot, white when cold)

Heated

Solution Z

Add dilute sulphuric acid

salt bridgesilver zinc

silver nitrate zinc sulphate

Beaker 2Beaker 1

copper(II) sulphate

carbon

Cell 1 Cell 2

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Cell 1 :. Cell 2 :.

( 2 marks)

b) State the energy change that takes place in cell 2.

.

( 1 mark)

c) (i) State the product formed at the negative terminal of Cell 1.

( 1 mark)

(ii) Write the half equation for the reaction at the negative terminal of cell 1.

( 1 mark)

d) Draw the direction of the flow of electron in Cell 1 in the diagram above.

( 1 mark)

e) State all the ions present in the electrolyte in Cell 2.

.

( 1 mark)

f) The circuit in Cell 2 is completed and the current is allowed to flow for 10 minutes.

(i) State the observation at the cathode of this cell.

.

( 1 mark)

(ii) Explain your answer in f (i) above.

.

( 1 mark)

g) What is the difference between Cell 1 and Cell 2 in terms of their structures?

.

(1 mark)

4. Table 3 shows pH values of different concentration of hydrochloric acid, HCl solution.

Type of solution Solution I Solution II Solution III

Concentration 0.1 mol dm-3 0.01 mol dm-3 0.001 mol dm-3

pH value 1 2 3

Table 4

(a) (i) Which of the solutions in Table 4 has the highest concentration of hydrogen ions?

.

( 1 mark)

(ii) Calculate the number of hydrogen ions in 25 cm3 of solution II.

(Avogadro Constant = 6 x 1023mol)

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(2 marks)

(iii) Name an indicator that can be used to measure the pH values of the solutions I, II and III.

.(1 mark)

(b) Solution I is used to neutralise 25 cm3 a of 0.1 mol dm-3 of sodium hydroxide, NaOH

Solution.

(i) Calculate the number of moles of sodium hvdroxide, NaOH in the solution.

( 1 mark)

(ii) Calculate the volume of solution I used to neutralise sodium hydroxide, NaOH solution in cm3.

(3 marks)

(c) Draw an apparatus set-up for the titration of sodium hydroxide solution with solution I.

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( 2 marks)

5. A student has carried out an experiment to determine the empirical formula of oxide of copper

According to the following steps shown in diagram below.

(a) Record the reading to two decimal places for :

Reading (a) :

(b) :

(c) : ( 3 marks)

(b) Construct a table to record the readings in the experiment.

( 3 marks)

(c) (i) Calculate the mass of

Copper : .

Oxygen :

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(ii) Determine the empirical formula of oxide of copper. (Relative atomic mass: Cu, 64 ; O, 16)

( 3 marks)

(d) State an observation in this experiment.

.

.

.

( 3 marks)

Section C (10%)

Answer one question from this section. Write your answer in the test pads.

1. (a) What is meant by salt?

[1 mark]

(b) The table shows the names for two types of salts.

Lead(II) Iodide Copper (II) sulphate

Which of the salts given is an insolublesalt?

Name the reaction used to prepare

insoluble salt.

[2 marks]

(c) Describe how you would prepare the insoluble salt above in the laboratory. In your answer,

write the ionic equation to represent the reaction.

[7 marks]

OR

2. Table below shows the atomic radii and melting points of part of group 18 elements.

(a) By referring to the table, describe and explain the trend of change in the physical properties

of the Group18 elements as we down the group in the Periodic Table. [6marks]

(b) Give the uses of the Group 18 elements in table 8 in our daily life.

Group 18

Elements

Physical PropertiesAtomic radius/ nm Melting Point / oC

Helium 0.050 -270

Neon 0.070 -248Argon 0.094 -189

Krypton 0.109 -156

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[4marks]

-QUESTIONS END-

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. .

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