Kimia Module 1-5 Diagnostik f4

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CHEMISTRY

FORM 4

MODULE 1


INTRODUCTION TO CHEMISTRY, THE STRUCTURE OF THE ATOM,

CHEMICAL FORMULAE AND EQUATIONS

MINISTRY OF EDUCATION MALAYSIA

1. You are given this formula:

What is X ? A Molar mass B Molar volume C Number of moles 2. You are given the molecular formula of glucose: C6H12O6

The molecular formula of glucose shows the

A actual mass of glucose B formula of a glucose molecule that exists in solid state C actual number of each atom of the elements in a glucose molecule D ratio for the number of atoms of each type of element in a glucose

molecule 3. Molar mass of a substance is the mass

A of one mole of the substance B of one atom of the substance C of 6.023 x 10 24 particles of the substance

4. The diagram shows the symbol of an atom.

The isotopes of hydrogen are , and . What is isotopes?

A Different atoms with the same number of electron, protons and neutrons. B Different atoms with the same number of electrons but different number

of protons. C Different atoms with the same number of neutrons but different number

of protons. D Different atoms with the same number of protons but different number of

neutrons.

X = tConsAvogadro

ParticlesofNumbertan

XAZNucleon number

Proton number

H11 H21 H31

2

5.

What is Avogadro constant? A The number of neutrons in an atom. B The mass in one mole of a substance C The number of protons and electrons of an atom. D The number of particles in one mole of a substance

6. ‘ 1 mole of any gas occupies 24 dm3 at room conditions’ is the definition of

A molarity B molar mass C molar volume

7. ‘An amount of substance that contains as many particles as the number of

atoms in exactly 12 g of carbon-12’ Which of the following terms explains the above statement?

A mole B molar mass C relative atomic mass D relative molecular mass

8. The equation below shows the reaction between magnesium and oxygen

2 Mg (s) + O2 (g) 2 MgO(s) Number 2 represents

A mass B volume C number of moles D number of particles

9. Which of the following statements is true about matter?

A Matter has mass only. B Matter has mass and occupies space. C Matter is the smallest particle of an element.

The value of Avogadro constant is 6.023 x 1023 mol-1

3

10. Which of the following is not true about molar mass?

A the mass of 6.02 x 10 23 particles B the mass of NA number of particles C the mass of one mole of the substances D the mass of one gram of the substances

11. An atom is a neutral particle. It contains the same number of

A protons and neutrons. B protons and electrons. C neutrons and electrons.

12. The diagram shows the heating curve of solid naphthalene.

Which of the following points shows the melting process of naphthalene?

A At point P B From point P to point Q C From point Q to point R D From point R to point S

13.

What is (are) the reactant (s) for the above chemical equation?

A CaCO3 only B CO2 and H2O C CaCO3 and HCl D CaCI2, H2O and CO2

time/minP

Q R

S

temperature/oC

CaCO3 (s) + HCI (aq) CaCI2(aq) + CO2 (g) + H2O(l)

4

14. The diagram shows the electron arrangement of atom X

How many valence electrons are there in the atom X?

A 2 B 5 C 7

15. The table shows the relative masses of the three subatomic particles.

Subatomic Relative mass

Proton 1 Electron

18401

Neutron 1 Which of the subatomic particles has the least mass?

A Proton B Neutron C Electron

16. The table shows the simplest ratio of elements P and Q

Element P Q Simplest ratio 1 3

What is the empirical formula of this substance?

A PQ B P3Q C PQ3 D P2Q3

X

5

17. The diagram shows the changes in the state of a substance from P to Q under pro

What is process X ?

A Melting B Freezing C Sublimation D Condensation

18. What is the number of molecules in one mole of carbon dioxide gas, CO2?

[NA = 6.02 x 1023 ]

A 2

1002.6 23×

B 1 x 6.02 x 1023 C 2 x 6.02 x 1023 D 3 x 6.02 x 1023

19. The number of electrons and the number of neutrons of atom X are 4 and 5

respectively. What is the proton number and nucleon number of atom X?

Proton

number Nucleon number

A 4 9 B 4 5 C 9 4 D 1 9

P Q

Process X

6

20. The table shows the relative atomic masses of copper and oxygen.

Elements Copper Oxygen

Relative atomic mass 64 16

How many times is copper atom heavier than oxygen atom?

A 0.25 B 4 C 48 D 80

21. The symbol of sodium atom can be written as Na23

11 The nucleus of this sodium atom contains

A. 11 protons and 12 neutrons B. 11 neutrons and 12 protons C. 11 protons and 12 electrons D. 12 neutrons and 11 electrons

22. The table below shows the proton number and the number of electrons of four

different particles.

Particle Proton number Number of electrons

P 8 8

Q 12 10

R 17 17

S 17 18

Which of the particles are ions? A P and Q B P and R C Q and R D Q and S

7

23. The table below shows the number of protons of four atoms W, X, Y and Z.

Atom Number of protons

W 3

X 16

Y 17

Z 19

Which of the atoms have the same number of valence electrons?

A W and Z B X and Z C X and Y D Y and Z

24. Calculate the number of moles of 16 g of Copper.

[ Relative atomic mass : Cu , 64 ]

A 0.25 B 0.75 C 2.50 D 7.50

25. An experiment is carried out to determine the empirical formula of oxide of metal

X . The data below shows the result of the experiment.

What is the empirical formula of oxide of metal X? [ Relative atomic mass: O,16 ; X, 65 ]

A XO B XO2 C X2O D X2O3

Mass of crucible and lid = 139.50g Mass of crucible, lid and metal X = 148.31g Mass of crucible, lid and oxide of metal X = 150.48g

8

26 What is the relative formula mass of hydrated copper(II) sulphate , CuSO4.5H2O?

[ Relative atomic mass : H , 1 ; O , 16 ; S , 32 ; Cu,64 ]

A 160 B 186 C 250 D 818

27. An oxide of metal X contains 6.9 g of metal X and 4.6 g of oxygen.

What is the empirical formula of oxide of metal X ?

[ Relative atomic mass: O, 16 ; X, 24 ]

A XO B XO2 C X2O D X2O3

28. The equation shows the reaction between calcium carbonate and nitric acid.

What is the volume of carbon dioxide gas released when 5 g of calcium carbonate

reacts completely?

[ Relative atomic mass: Ca,40 ; C,12 ; O,16 ; H ,1 ; one mole of any gas occupies

24 dm3 at room conditions]

A 1.2 dm3 B 2.4 dm3 C 12 dm3 D 24 dm3

29. What is the number of moles of 560 cm3 of carbon dioxide gas at STP?

[Given that number of mole of gas = volume ÷ molar volume ;

molar volume : 22.4 dm3 mol -1 at STP ]

A 0.025 mol B 0.25 mol C 2.5 mol D 25 mol

CaCO3(s) + 2HNO3 (aq ) Ca(NO3) 2(aq ) + H2O(l) + O2(g)

9

30. The diagram shows the set-up of apparatus used to investigate diffusion in a solid

gel.

After a few days, the entire solid gel turned purple.

What can we deduce from the above investigation?

A Potassium manganate(VII) dissolves in the gel.

B Potassium manganate(VII) is less dense than the gel.

C Potassium manganate(VII) reacts with the gel to produce purple

colour

D Potassium manganate(VII) particles diffuse through spaces

between the gel particles.

31. The equation shows the reaction between carbon and oxygen gas.

What is the mass of carbon dioxide gas released when 12 g of carbon reacts

completely in the reaction?

[ Relative atomic mass: C, 12 : O, 16 ]

A 12 g

B 28 g

C 32 g

D 44 g

Gel

Potassium manganate(VII) cystal

C (s) + O2 ( g) CO2 (g)

10

32. The diagram shows two balloons P and Q.

Balloon P is filled with 1.5 moles of carbon dioxide gas whereas balloon Q is

filled with 2.5 moles of oxygen gas.

What is the mass of carbon dioxide and oxygen ?

[ Relative atomic mass: C,12: O,16 ]

carbon dioxide oxygen

A 22 g 16 g

B 42 g 40 g

C 44 g 32 g

D 66 g 80 g

P Q

1.5 mol of carbon dioxide

2.5 mol of oxygen

11

33. You are given a chemical equation:

2 Mg (s) + O2 (g) 2MgO(s) Write three information based on the chemical equation.

i) ………………………………………………………………………………………..…

ii) ……………………………………………………………………………………….….

iii) ………………………………………………………………………………………….

34. The figure shows the relationship between the number of particles, the number of

moles and the mass of a substance. ÷ NA x Molar mass x NA ÷ Molar mass Based on the above figure write the formulae to determine : i) number of moles = ii) mass of a substance = iii) Number of particles =

Number of particles

Number of moles

Mass

12

35. A crystal of copper(II) sulphate is placed at the bottom of a beaker filled with water. The

beaker is left aside until the water turns blue.

Name the process occurred. Explain your answer.

Name of process : …………………………………………………………………………….

Explanation : …………………………………………………………………………….

..……………………………………………………………………………………………………..

……………………………………………………………………………………………………….

……………………………………………………………………………………………………….

Blue solution of copper (II) sulphate, CuSO4

Copper (II) sulphate crystal

Water After 1 day

13

36. The figure shows the heating curve of solid naphthalene.

Describe the changes in term of the movement and the forces of attraction of

naphthalene particles from point

(a) P to Q: 1. Movement: ………………………………………………………………..…

………………………………………………………………………………..

2. Forces of attraction:…………………………………………………..…...

……………………………………………………………………………………...

(b) R to S:

1. Movement: ……………………………………………………………..…

……………………………………………………………………….……..

2. Forces of attraction:……………………………………………………...

…………………………………………………………………..………….

time/minP

Q R

S

temperature/oC

14

Listen carefully to the text read by the teacher. Answer questions 37 and 38. 37. The smallest particle of an element that can participate in a chemical reaction is

called A ion B atom C element D molecule 38. A negatively-charged and positively-charged particles are called A ions B atoms C elements D molecules Listen carefully to the text read by the teacher. Answer questions 39 and 40 39. Which of the following is not true about chemical equation? A It can be written in words only. B It shows the state of substances. C It can be written in words or symbols. D It is a shorthand description of a chemical reaction. 40. What are the states of matter that involved in a chemical reaction?

i) ………………………………………………………………………...

ii) ……………………………………………………………………….

iii) …………………………………………………….………………….


CHEMISTRY

FORM 4

MODULE 2


PERIODIC TABLE OF ELEMENTS,

CHEMICAL BONDS


3

1 In the Periodic Table, the horizontal row of elements is known as the

A group B family C period D series

2 The term ampotheric means

A alkali in nature. B basic in nature. C acidic in nature. D both acidic and alkali in nature.

A measurement of the strength of an atom in its molecule to attract electrons towards its nucleus.

3 Which of the following referred to the statement above?

A Electropositivity B Electronegativity C Electrical conductivity D Electropositivity

4 What is an anion?

A A neutral particle. B A positively-charged particle. C A negatively-charged particle.

5 What is the type of chemical bond in sodium chloride, NaCl?

A Ionic bond. B Single bond. C Double bond. D Covalent bond.

4

6 One hydrogen atom combines with another hydrogen atom to form a covalent

molecule by

A sharing electrons. B accepting electron. C donating electron. D exchanging electrons.

7 Group 18 elements are known as

A halogens. B noble gases. C alkali metals. D alkali earth metals

8 All the following elements are in group 17 except

A iodine. B fluorine. C chlorine. D caesium

9 Elements in the Modern Periodic Table are arranged according to their

A boiling point. B atomic mass. C proton number. D nucleon number.

10 Which of the following is true?

Noble gases Uses

A Neon To detect pipes leakage. B Argon To fill photographic flash lamps. C Helium To fill up balloons and airships. D Krypton To fill light bulbs.

11 Which of the following scientists proposed the Law of Octaves ?

A Lothar Meyer B John Newlands C Dmitri Mendeleev D Johann W. Dobereiner

5

12 Which of the following is true about the special properties of transition elements ?

I low density. II act as catalysts. III form complex ions. IV form coloured compounds.

A I and II B I and III C I , III , and IV D II , III , and IV

13 Which of the following is the property of ionic compounds?

A High melting point. B Does not dissolve in water. C Can conduct electricity. D Dissolve in organic solvents.

14 An atom that receives an electron forms

A a cation. B an anion. C an ionic bond. D a covalent bond.

15 Where is X23

11 located in the Periodic Table?

Group Period A 1 3 B 2 3 C 1 4 D 2 4

16 The type of chemical bond in an oxygen molecule is

A single covalent bond. B double covalent bond. C triple covalent bond.

6

17 Which of the following chemical formulae represents an ionic compound?

A CO2 B H2O C K2O D SO2

18 Which of the following pairs of elements will form a compound by sharing

electrons?

A Sodium and chlorine. B Hydrogen and chlorine. C Potassium and oxygen. D Magnesium and oxygen.

19 Which of the following has the same number of electrons as neon?

[ Proton number : F, 9 ; Na , 11 ; Cl, 17 ; O , 8 ; Ne , 10 ]

A F B O2- C Cl- D Na

20 Which of the following substances when dissolves in water, has the highest

electrical conductivity?

A Vinegar B Ammonia C Carbon dioxide D Potassium oxide

21 Element Y with proton number 19 reacts with water to form gas X.

What is gas X ?

A Oxygen B Hydrogen C Carbon dioxide D Nitrogen dioxide

7

22 Element A has proton number 20.

What is the position element A in the Periodic Table?

Group Period A 1 3 B 2 3 C 1 4 D 2 4

23 Which of the following statements is true about element chlorine?

A Chlorine is more reactive than fluorine. B Chlorine is more reactive than bromine. C Chlorine is more electronegative than fluorine. D Atomic size for chlorine is larger than bromine.

24 Which of the following statements is not true about sodium metal?

A Sodium is more reactive than lithium. B Atomic size of sodium is larger than lithium. C Sodium reacts with oxygen to form white solid. D Tendency of sodium atom to release electron is higher than

potassium atom. 25 The electron arrangement of atom P is 2.8.8.1.

Which of the following is true about P?

I P reacts vigorously with water. II P is more electropositive than sodium. III P burns in air to produce white P oxides. IV P reacts with chlorine gas to form yellow P chlorides.

A I , II, and III B I, III, and IV C II , III, and IV D I, II, III, and IV

8

26 Which of the following substances has high melting point?

I II III IV

Ethanol Sodium chloride Lead(II) bromide Tetrachloromethane

A I and II only B I and III only C II and III only D III and IV only

27 The proton number of element M is 8.

Which of the following is true about element M?

A M atom forms M2+ ion. B M2+ ion achieves octet electron arrangement. C Carbon atom combines with atom M to form a compound with chemical

formula CM2. D Sodium atom combines with atom M to form a compound with chemical

formula NaM. 28 An element M reacts with oxygen to form a covalent compound, MO2. What is the

electron arrangement of atom M?

A 2.4 B 2.6 C 2.8.2 D 2.8.8.1

29 Which of the following compounds contain only covalent bonds?

A K2O B CO2 C CO2 D K2O

9

30 Table shows the proton number of four atoms, P, Q, R and S.

Atom P Q R S Proton number 17 8 11 6

Which of the following chemical formulae is correct?

A PQ B SP C RP2 D R2Q

31 Element P has an electron arrangement of 2.8.1.

Element R has an electron arrangement of 2.6. Which of the following is true about the compound formed between elements P and R?

Type of compound Chemical formula

A Ionic compound PR B Ionic compound P2R C Covalent compound PR D Covalent compound P2R

10

Question 32 to 34. Write the answers in the spaces provided. 32 Based on the information given below, describe the formation of ionic bond in

sodium chloride, NaCl.

1. Sodium atom with ……….. 2.8.1 …………. .electron to achieve ……….. electron …………… 2. Chlorine atom with …………… 2.8.7 ……………. electron to achieve ……………. electron ………... 3. Sodium ion and ……………. ion formed are …………. to one another by ………….. force.

The formation of sodium chloride, 1. ……………………………………………………………………………

……………………………………………………………………………

2. .…………………………………………………………………………..

…………………………………………………………………………… 3. …………………………………………………………………………… ….……………………………………………………………………………

11

33 Diagram shows the electron arrangements of hydrogen atom and chlorine atom.

Based on the information given below, describe the formation of covalent bond in hydrogen chloride. ……………………………………………………………………………………………… ……………………………………………………………………………………………… ……………………………………………………………………………………………… ……………………………………………………………………………………………… ……………………………………………………………………………………………… ………………………………………………………………………………………………

Hydrogen atom - 1 valence electron - needs one more electron to achieve duplet electron arrangement

Chlorine atom - 7 valence electrons - needs one more electron to achieve octet electron arrangement

Hydrogen chloride - share electrons - covalent bond

12

34 The table below shows the properties of ionic compounds and covalent

compounds.

Properties Ionic compound

Covalent compound

Melting point High Low Conduct electricity in molten and aqueous

Yes No

Solubility in water Yes No

Based on the table describe three differences between ionic compounds and covalent compounds.

………............................................................................................................... ………………………………………………………………………………………… ………………………………………………………………………………………… ………………………………………………………………………………………… ………………………………………………………………………………………… ………………………………………………………………………………………… ………………………………………………………………………………………… …………………………………………………………………………………………

Listen carefully to the text read by the teacher. Answer the questions 35 and 36 that follows.

35 Why do the ionic compounds have high melting and boiling points?

………...............................................................................................................

13

36 What is another property for the ionic compounds?

………...............................................................................................................

Listen carefully to the text read by the teacher. Answer the questions 37, 38, 39 and 40 that follows.

37 What happen when a piece of sodium is placed in the water?

………...............................................................................................................

38 State the changes of universal indicator when added to the solution.

………...............................................................................................................

39 Name the gas released during the reaction.

………...............................................................................................................

40 Name the product formed.

………...............................................................................................................


CHEMISTRY

FORM 4

MODULE 3


ELECTROCHEMISTRY


3

1 The diagram shows a type of cell that consists of batteries, electrolyte and two

electrodes.

Name the cell.

A Electrode cell B Electrolyte cell C Electrolytic cell D Electrolysis cell

2 An electrode which is connected to the positive terminal of the source of electricity in an electrolytic cell is called

A anion B cation C anode D cathode

Carbon electrodes

Electrolyte

Battery

4

3 The diagram shows the decomposition of molten lead(II) bromide into its

constituent elements when an electric current passes through it.

What is the process called?

A Extraction B Purification C Electrolysis D Electroplating

Molten lead(II) bromide

Heat

Carbon electrodes

5

4 The diagram shows an experiment to prevent the iron ring from rusting.

Name the process involved.

A Extraction B Purification C Electroplating D Neutralization

5 What is meant by electrolytes?

A Substances that can conduct electricity in any state but are not chemically changed.

B Substances that can conduct electricity in solid or molten but are not chemically changed.

C Substances that can conduct electricity in aqueous solution only and undergo chemical changes.

D Substances that can conduct electricity either in molten state or in aqueous solution and undergo chemical changes.

6 Ion that is attracted to the positive terminal during electrolysis is known as

A anion B proton C cation D electron

Copper strip CuSO4 solution

Iron ring

Iron coated with copper

6

7 Which of the following substances undergoes electrolysis?

A Molten sulphur B Glucose solution C Molten lead metal D Sodium chloride solution

8 Which of the following is not a factor that affects the electrolysis of an aqueous solution?

A Position of ions in electrochemical series B Types of electrodes C Presence of catalyst D Concentration of ions

9 What is the change of energy that occurs in a voltaic cell?

A Electrical energy to potential energy. B Potential energy to chemical energy. C Electrical energy to chemical energy. D Chemical energy to electrical energy.

10 Which of the following pairs of electrodes are inert?

A Copper and carbon. B Carbon and platinum. C Copper and magnesium. D Platinum and magnesium.

11 What are the ions that present in copper(II) sulphate solution?

A Copper(II) ion and sulphate ion. B Copper(II) ion and hydrogen ion. C Copper(II) ion, hydrogen ion, sulphate ion and oxide ion. D Copper(II) ion, hydrogen ion, sulphate ion and hydroxide ion.

7

12 What are the ions that present in the molten lead(II) bromide?

A Lead(II) ion and bromide ion only. B Lead(II) ion, hydrogen ion and bromide ion only. C Lead(II) ion, hydroxide ion and bromide ion only. D Lead(II) ion, hydrogen ion, hydroxide ion and bromide ion.

13 The electrochemical series can be constructed based on

A the ability of a metal to displace another metal from its salt solution. B the availability of an element in many organic substances. C the ability of an element to exist in more than one oxidation number.

14 The table shows the differences between electrolytic cell and voltaic cell.

Choose the false statement.

Characteristic Electrolytic cell Voltaic cell A Energy changes Electrical energy→ chemical

energy Chemical energy → electrical energy

B Flow of electrons From negative to positive electrodes.

From positive to negative electrodes.

C Types of electrodes

Same or different types of metals or graphite electrodes.

Two different types of metals.

8

15 Diagram shows the electrolysis of molten lead(II) bromide.

What are the observations at the anode and cathode?

Anode Cathode

A Colourless gas is given off

Grey solid is deposited

B Brown gas is given off Colourless gas is given off C Brown gas is given off Grey solid is deposited D Grey solid is deposited Bromine gas is given off

16 The diagram shows the set-up of apparatus for the electrolysis of concentrated

iron(III) chloride solution using carbon electrodes.

What are the products formed at test tubes X and Y during the electrolysis?

X Y

A Chlorine gas Hydrogen gas B Hydrogen gas Oxygen gas C Chlorine gas Iron metal D Hydrogen gas Chlorine gas

heat


Carbon electrodes

Concentrated iron(III) chloride solution Carbon electrodes

X Y

9

17 Which of the following voltaic cells shows the correct direction of electron flow?

18 The diagram shows a part of the electrochemical series.

Based on the electrochemical series, which of the following pairs of the terminals is correct?

Negative terminal Positive terminal

A Aluminium Iron B Zinc Magnesium C Aluminium Magnesium D Iron Zinc

Magnesium

Tin

Dilute hydrochloric acid

Copper Aluminium

Lead Zinc


Iron Zinc

A C

B D

Electropositivity decreases

Ca Al Mg Fe Zn

10

heat


Carbon electrodes

19 Which of the following pairs of metals that gives the highest voltage in a voltaic

cell?

A Zinc and iron. B Tin and lead. C Copper and tin. D Silver and magnesium.

20 The diagram shows an experiment of the electrolysis of molten lead(II) bromide.

Which of the statements is true?

A Solid lead(II) bromide is a

molecule. B Molten lead(II) bromide is a molecule. C Solid lead(II) bromide contains freely moving ions. D Molten lead(II) bromide contains freely moving

ions.

11

+ −

Carbon electrodes

Sodium chloride solution

21 The diagram shows an electrolysis of sodium chloride solution.

What are the ions that are attracted to the cathode?

A Sodium ion , Na+ and chloride

ion, Cl- B Sodium ion, Na+ and hydrogen

ion, H+ C Chloride ion, Cl- and hydroxide

ion, OH- D Hydrogen ion, H+ and hydroxide

ion, OH- 22 Q is a metal that can displace lead from lead(II) nitrate solution.

Which of the following metals cannot displace Q from its salt solution?

A Iron. B Silver. C Aluminium. D Magnesium.

23 Which of the following compounds could be used as an electrolyte in

electroplating of iron spoon with silver?

A Silver nitrate solution. B Iron(II) chloride solution. C Copper(II) sulphate solution. D Dilute hydrochloric acid.

12

24 Sodium chloride does not conduct electricity in solid state because

A it has a high density. B it has a high melting point. C the sodium ions and the chloride ions are only present in molten state. D the sodium ions and the chloride ions are held in a fixed position in the crystal

lattice. 25 In the diagram below, the electrons flow from the zinc electrode to the copper

electrode because

A copper is more reactive than zinc. B sulphuric acid contains free electrons. C zinc is more electropositive than copper. D there is more electrons at the zinc electrode.

Copper Zinc

Dilute sulphuric acid

e e

13

26 The diagram shows a Daniell cell using magnesium and lead as electrodes.

Which of the following represents the half-equation at lead electrode? A 2H+ + 2e H2 B Pb Pb2+ + 2e C Pb2+ + 2e Pb D Mg2+ + 2e Mg

27 The diagram below shows the set-up of apparatus to coat an iron spoon with

copper.

What can be observed at the anode and cathode after 30 minutes?

Anode Cathode A Copper strip becomes thinner Gas bubbles are released B Copper strip becomes thicker Brown solid is formed C Copper strip becomes thinner Brown solid is formed D Copper strip becomes thicker Gas bubbles are released

Iron spoon

Copper strip

Aqueous copper(II) sulphate solution

Magnesium electrode

Magnesium sulphate solution

Lead electrode

Porous pot

Lead(II) nitrate solution

14

28 A solution of sodium nitrate is electrolysed by using carbon electrodes.

Which of the following statements shows the reaction that occur at the beginning of the electrolysis?

A Nitrate ions are discharged at the anode. B Sodium ions are discharged at the cathode. C Hydrogen ions receive electrons at the

anode. D Hydrogen ions receive electrons at the

cathode. 29 The diagram shows four simple voltaic cells.

Which of the cells shows the highest potential difference?

Copper


Aluminium Copper

Zinc Copper


Lead Copper

A C

B D

15

30 The table shows pairs of metals and the results obtained when they are used as

electrodes in chemical cells.

Pair of Metal

Voltage/V Negative terminal

P / Q 0.78 P R / Q 2.72 R S / R 0.72 R S / P 1.22 S

The electrochemical series formed in descending order is

A P, Q, R, S B S, R, P, Q C R, P, Q, S D R, S, P, Q

31 The tables show the ions present in aqueous silver nitrate, AgNO3 and the ions

that are attracted to the cathode and the anode during the electrolysis.

Electrolyte Silver nitrate solution

Ions present Ag+, NO3−, H+, OH−

Electrode Cathode Anode

Ions attracted Ag+, H+ NO3−, OH−

Based on the tables,

(a) explain the electrolysis of aqueous silver nitrate, AgNO3, using carbon electrodes.

…………….…………………………………………………………………………… ………………………………………………………………………………………… …………………………………………………………………………………………

(b) name the products at the cathode and anode.

…………………………………………………………………………………………

16

32 The diagram shows a simple voltaic cell.

Based on the diagram, describe the structure of the simple voltaic cell. …………………………………………………………………………………………………. …………………………………………………………………………………………………. …………………………………………………………………………………………………. ………………………………………………………………………………………………….

Listen carefully to the text read by the teacher. Answer questions 33 and 34.

33 Name the ore that contains aluminium oxide.

A Galena B Bauxite C Hematite D Casiterite

34 What is the function of adding cryolite to aluminium oxide?

A To melt the ore. B To act as the anode. C To act as the cathode. D To lower the melting point of aluminium oxide.

Metal X Metal Y

Electrolyte

17

Listen carefully to the text read by the teacher. Answer questions 35 and 36. 35 What is electrochemical series?

A An arrangement of metals based on its reactivity with oxygen. B An arrangement of metals based on its reactivity with hydrogen. C An arrangement of metals based on the tendency of each metal atom to

accept electrons. D An arrangement of metals based on the tendency of each metal atom to

donate electrons. 36 Which of the following is true about the electrochemical series?

A It can be used to determine the standard cell voltage. B It is based on the tendency of a metal atom to accept electron. C The metal which is situated at a higher position in the series will be the negative

terminal. D The greater the tendency of a metal atom to accept electron the higher it is in the

series.


CHEMISTRY

FORM 4

MODULE 4


ACIDS AND BASES

& SALTS


3

1 What is meant by ‘strong acid’?

A Acid that partially ionized to produce low concentration of hydrogen ions B Acid that partially ionized to produce high concentration of hydrogen ions C Acid that completely ionized to produce low concentration of hydrogen ions D Acid that completely ionized to produce high concentration of hydrogen

ions.

2 The equation below represents a reaction between acid and alkali.

Acid + alkali salt + water

What is the name of this reaction?

A Titration. B Precipitation. C Fermentation. D Neutralisation.

3 The diagram shows a flow chart to identify substance P. What is the type of analysis used to identify substance P?

A Qualitative analysis B Quantitative analysis C Psychometric analysis D Spectrometry analysis

Substance P

Test for anions

Test for gases

Test for cations

4

4 What is salt?

A A mixture formed when an acid is added to a metal or an ammonium compound. B A mixture formed when an alkali is added to a metal or an ammonium compound. C A compound formed when the hydrogen ion of an acid is replaced by a metal ion or

an ammonium ion. D A compound formed when the hydroxide ion of an alkali is replaced by a metal ion or

an ammonium ion.

5 An indicator is added to an alkali and acid solution respectively. Which of the following is correct?

Indicator Colour in alkali Colour in acid A Phenolphthalein colourless pink B Phenolphthalein pink colourless C Methyl orange red yellow D Methyl orange red orange

6 Which of the following is not a monoprotic acid?

A Nitric acid B Sulphuric acid C Hydrochloric acid D Methanoic acid

5

7 The diagram below shows changes that occur before and after water is added to

a chemical substance.

Name the substance.

A Acid. B Salt C Base. D Alkali.

8 Which of the following is an insoluble salt?

A Silver nitrate B Lead(II) sulphate C Sodium carbonate D Copper(II) chloride

9 Neutralisation process is used in various fields in our daily life.

Which of the following statements is false?

A Vinegar is used to prevent coagulation of latex B An antacid is used to neutralise excess acid in the stomach. C Acidic soil is treated with powdered lime, lime stone or ashes of burnt wood D Toothpaste is used to neutralise the acid produced by bacteria in our mouth.

10 Which of the following is the physical characteristic of crystals?

A Crystals of the same substance have same size. B Crystals of the same substance have different shapes. C Crystals have same angles between two neighbouring surfaces. D Crystals have flat surfaces, straight edges and sharp angles.

Before adding water After adding water

CH3COOH

CH3COOH

CH3COOH

H+

H+ H+

H+

CH3COO-

CH3COO-

CH3COOH

6

11 The diagram shows the pH values of five different solutions.

Which of the solutions has the highest concentration of hydrogen ions?

A V B W C X D Y

12 The diagram shows types of particles in a solution. The solution is a

A weak acid

B strong acid C weak alkali D strong alkali

V W X Y

pH = 1 pH = 4 pH = 8 pH = 12

NH4+

OH-

NH4+

OH-

NH3

NH3

NH4+

OH-

7

13 The table shows the concentration and pH value of sodium hydroxide solution,

NaOH in test tube P, Q, R and S.

Test tube

Concentration of NaOH solution (mol dm-3)

pH value

P 0.0001 10 Q 0.001 11 R 0.01 12 S 0.1 13

Which of the following statements is true?

A When the concentration of sodium hydroxide solution increases, the concentration

of hydrogen ions decreases. B When the concentration of sodium hydroxide solution increases, the concentration

of hydroxide ions decreases. C When the concentration of sodium hydroxide solution increases, the concentration

of hydrogen ions also increases. D When the concentration of sodium hydroxide solution increases, the concentration

of hydroxide ions also increases.

14 The diagram shows the titration of sodium hydroxide solution with dilute hydrochloric acid. What is the function of phenolphthalein?

A To determine the amount of the product. B To determine the degree of ionization of an acid. C To determine the degree of ionization of an alkali. D To determine the end point of neutralisation reaction.

Burette


NaOH solution + phenolphthalein

8

15 The diagram shows the results when electricity is passed through two solutions

R and S. Based on the observations, solution R and solution S are

Solution R Solution S A Sodium hydroxide in water. Sodium hydroxide in methyl benzene. B Ammonia in propanon. Ammonia in methyl benzene. C Hydrochloric acid in water. Hydrochloric acid in propanon. D Ethanoic acid in methyl benzene. Ethanoic acid in water.

16 Which of the following ions forms a white precipitate which will dissolve in excess sodium hydroxide solution and ammonia solution?

A Zn2+ B Ca2+ C Al3+ D Pb2+

17 Which of the following is used to prepare lead (II) sulphate?

A Add lead metal to sodium sulphate. B Add lead(II) nitrate to potassium sulphate. C Add lead(II) chloride to sodium sulphate D Add lead(II) carbonate to potassium sulphate.

Carbon electrodSolution R Solution S

Bulb does not light up Bulb lights up

9

18 The equations below show the reaction used to prepare insoluble salt.

AgNO3 + KCl AgCl + KNO3 CaCl2 + Na2CO3 CaCO3 + 2NaCl Which of the following pairs is insoluble salt?

A AgCl and NaCl B AgCl and CaCO3 C KNO3 and NaCl D KNO3 and CaCO3

19 Which of the following salts is prepared by titration method?

A Copper(II) nitrate B Lead(I) nitrate C Magnesium nitrate D Potassium nitrate

20 The equation below shows the neutralisation reaction between hydrochloric acid and sodium hydroxide solution.

HCl + NaOH NaCl + H2O

What is the concentration of 50 cm3 hydrochloric acid, HCl needed to neutralise 50 cm3 of 0.5 mol dm-3 sodium hydroxide, NaOH solution?

A 0.25 mol dm

B 0.50 mol dm

C 0.75 mol dm

D 1.00 mol dm

10

21 The equation below shows the reaction between sodium and oxygen.

4Na + O2 2Na2O

What is the mass of sodium oxide formed when 2.3g of sodium reacts completely with oxygen? [Relative atomic mass : Na, 23 ; O, 16]

A 1.55g B 3.10g C 4.65g D 6.20g

22 What is the volume of 0.1 mol dm-3 nitric acid required to neutralise completely 25.0 cm3 of 0.1 mol dm-3 sodium hydroxide solution?

A 10.0 cm3 B 25.0 cm3 C 30.0 cm3 D 45.0 cm3

23 What is the concentration of hydrogen ion in 0.10 mol dm-3 nitric acid?

A 0.05 mol dm-3

B 0.10 mol dm-3

C 0.15 mol dm-3

D 0.20 mol dm-3

11

24 The table below shows the information in a qualitative analysis.

Reagent Observation Result

Sodium hydroxide solution until excess

• White precipitate

• Dissolve in excess

Zn2+ Al3+ Pb2+

Aqueous ammonia until excess

• White precipitate

• Does not dissolve in excess

Al3+ Pb2+

Potassium iodide solution

• Yellow precipitate

Pb2+

A solution may contain Pb2+ ions, Zn2+ ions or Al3+ ions. Explain the chemical test to confirm the presence of ions Pb2+ , Zn2+ and Al3+ .

Answer: ………………………………………………………………………………………………………

………………………………………………………………………………………………………

………………………………………………………………………………………………………

……………………………………………………………………………………………………...

……………………………………………………………………………………………………...

……………………………………………………………………………………………………...

12

25 The equation below shows the reaction when zinc nitrate is heated strongly.

2Zn(NO3)2 2ZnO + 4NO2 + O2 State three observations when zinc nitrate is heated strongly.

Answer: ………………………………………………………………………………………………………

………………………………………………………………………………………………………

………………………………………………………………………………………………………

26 The diagram shows the heating process of zinc carbonate. State two observations for the heating of zinc carbonate.

Answer: ………………………………………………………………………………………………………

………………………………………………………………………………………………………

Zinc carbonate

Lime water

Heat

13

27 The diagram below shows the flow chart for the chemical test of Fe2+ ions and

Fe3+ ions. Based on the flow chart, explain how to differentiate Fe2+ ions and Fe3+ ions.

Answer:

………………………………………………………………………………………………………

………………………………………………………………………………………………………

………………………………………………………………………………………………………

………………………………………………………………………………………………………

Solution contains Fe2+ ions or Fe3+ ions.

Light blue precipitate

Dark blue precipitate

Fe2+ ions

Fe3+ ions

K4Fe(CN)6

Potassium hexacyanoferrate(II)

Test II

Solution contains Fe2+ ions or Fe3+ ions.

No change

Blood red solution

Fe2+ ions

Fe3+

Potassium thiocyanate

KSCN

Test I

14

Listen carefully to the text read by the teacher. Answer questions 28 and 29.

28 State one common use of salt.

……………………………………………………………………………………………………

29 State one effect when we take excess salt in our food?

……………………………………………………………………………………………………

Listen carefully to the text read by the teacher. Answer questions 30, 31, and 32.

30 Name a substance that can be used to overcome the gastric problem.

……………………………………………………………………………………………………

31 What can be used to reduce pain caused by bee sting?

……………………………………………………………………………………………………

32 State the other use of neutralisation.

……………………………………………………………………………………………………


CHEMISTRY

FORM 4

MODULE 5


MANUFACTURED SUBSTANCES IN

INDUSTRY


3

1. The diagram shows the formation of a large molecule by joining together all the sub-

units in process X.

What is proses X?

A Freezing B Refraction C Polymerisation D Depolymerisation

2. What is Contact Process?

A An industrial process for the manufacture of ammonia

B An industrial process for the manufacture of nitric acid

C An industrial process for the manufacture of sulphuric acid

D An industrial process for the manufacture of hydrochloric acid

3. What is a composite material?

A A mixture of elements and has metallic properties

B A long chain molecule formed by joining together many small repeating units

C A material with more superior properties that formed by combining two or

more different substances

Sub-units

X

Large molecule

4

4. What is an alloy?

A An alloy is a mixture of two or more ions with a certain fixed composition.

B An alloy is a mixture of two or more atoms with a certain fixed composition.

C An alloy is a mixture of two or more elements with a certain fixed

composition.

D An alloy is a mixture of two or more molecules with a certain fixed

composition

5. Name the industrial process that produce ammonia?

A Haber process

B Contact process

C Ostwald process

6. Which of the following is not the property of ammonia?

A Colourless gas

B Soluble in water

C Changes moist blue litmus paper to red

D Changes moist red litmus paper to blue

7. Which of the following are the uses of ammonia in daily life?

I To manufacture nitric acid

II To manufacture explosives

III To manufacture sulphuric acid

IV To manufacture nitrogenous fertilizers

A III and IV

B I, II and III

C I, II and IV

D I, II, III and IV

5

8. Polymer X is used to make safety glass, lens and reflectors. Its monomer is

methylmethacrylate.

What is the name of polimer X?

A Nylon

B Perspex

C Polythene

D Polypropene

9. The chemical equation below shows the reaction of the manufacture of sulphuric acid

in stage II. SO2(g) + O2(g) SO3(g) What is the optimum conditions for the reaction in stage II

Temperature/°C Catalyst Pressure/ atm A 450 Iron 1 B 450 Iron 10 C 450 Vanadium(V) oxide 1 D 450 Vanadium(V) oxide 10

10. The diagram shows the arrangement of atoms in alloy X. Alloy X What is the name of alloy X?

A Steel B Brass C Bronze D Duralumin

Tin

Copper

6

11.Which of the following is not true about the uses of sulphuric acid?

A Leather tanning

B Manufacture of paint

C Production of margerine

D Manufacture of detergents

12. Which of the following is not the aim of making alloy?

A To prevent rusting

B To minimize corrosion

C To improve physical appearance

D To lower the melting of the metal

13. Which of the following pairs is not true?

Process Catalyst A Manufacture of sulphuric acid Vanadium(V) oxide B Manufacture of ammonia Copper(II) sulphate C Manufacture of nitric acid Platinum D Manufacture of margerine Nickel

14. Which of the following information is true?

Type of glass Properties

A Lead crystal glass • Low melting point • High density

B Soda lime glass • High melting point • Reflects light rays

C Borosilicate glass • Low melting point • High refractive index

D Fused silicate glass • Low melting point • More resistant to

chemical

7

15. The diagram shows an experiment to investigate the rate of corrosion of iron nail,

steel nail and stainless steel nail.

The manipulated variable in the experiment is

A type of nails

B rate of corrosion

C condition of experiment

Jelly solution + potassium hexacyanoferrate(III)

Iron nail Steel nail Stainless steel nail

8

16. The diagram shows the structure of polymer P Which of the following is the monomer of polymer P?

A C B D 17. Which of the following statements explains the reason of why steel is harder and stronger than iron?

A The orderly arrangement of atoms in steel enables the layer of atoms to slide on

one another

B The defects in the arrangement of atom in steel allows the layer of atoms to

slide on one another

C The presence of foreign atoms disturbs the orderly arrangement of atom in

steel thus reduces the layer of atoms from sliding on one another

C C

H H

Cl H

C C

H H

Cl H

H H C C

H

Cl H

H

C

H

H

C C

H

Cl H

H

C

H

H

C C

H H

Cl H

C C

H H

Cl H

C C

H H

Cl H

C C

H H

Cl H

9

18. What is the percentage of nitrogen by mass in ammonium sulphate, (NH4)2SO4?

[Relative Atomic Mass : H,1; N,14; O, 16; S, 32]

A 4.71 %

B 10.60 % C 21.21 % D 28.00 %

19. Fertilizer ammonium sulphate can be prepared by reacting ammonia with sulhuric

acid.

Which of the following balanced chemical equation is correct?

A NH3 + HSO4 → NH4SO4

B 2NH3 + H2SO4 → (NH4)2SO4

C NH3 + H2SO4 → (NH4)2SO4

D 2NH3 + HSO4 → (NH4)2SO4

10

20. The following shows the composition, properties and uses of alloy X.

• 96% tin • 3% copper • 1% antimony

What is alloy X?

A Steel

B Brass

C Pewter

D Stainless steel

Alloy X

Composition Properties Uses

• luster • shiny • strong

• Making of souvenirs •

11

21. The diagram shows the environmental pollution caused by sulphur dioxide.

(a) State two types of pollution.

1 : ………………………………………………………………………..…………………

2 : ………………………………………………………………………………..…………

(b) State one effect caused by each pollution in (a)

1: …………………………………………………………………………...………………

2: …………………………………………………………………………………...………

SO2

SO2

SO2 O2 O2

Acid rain Acid rain

SO2

12

(c) Explain the formation of acid rain. You may used the keywords below.

………………………………………………………………………………………………

……………………………………………………………………………...………………

………………………………………………………………………………………………

22. The diagram shows the manufacturing of ammonia in an industry.

Based on the diagram in the manufacturing of ammonia, NH3 , answer the following

questions.

(a) What are the raw materials used?

…..…………………………………………………………………………………………

SO2 – factories. Burning petrol – SO2. SO2 – water and oxygen – acid rain.

N2 gas

H2 gas

Mixture: N2 + H2 Temperature: 450 OC Pressure: 200 atm Catalyst: Iron

Reactor

NH3

13

(b) Describe the manufacturing of ammonia and state the conditions involved. ……………………….………………..………………………..…………………………

…….……………………………..……………………….……………………...…………

………………………………………………………………………………………………

………………………………………………………………………………………………

………………………………………………………………………………………...……

………………………………………………………………………………………………

(c) Write the chemical equation involved.

…………………………………………………………………………………...…………

14

23. The table below shows three stages involved in the manufacturing of sulphuric acid.

Explain the manufacturing of sulphuric acid. Your explanation should start with stage

I until you finally get the sulphuric acid.

………………………………………………………………………………………..………… ………………………………………………………………………………………..………… ………………………………………………………………………………………..………… ……………………………………………………………………………..…………………… ……………………………………………………………………………………..…………… Listen carefully to the text read by the teacher. Answer questions 24, 25 and 26. 24. What is the pH of natural rain water and the pH of acid rain?

………………………………………………………………………………………………

25. Name the gas that caused acid rain …….…………………………………………………………………..………………………

26. How is acid rain formed? ….………………………………………………………………………………..…………… ….…………………………………………………………………………………..…………

Stage Reactant Product

I Sulphur and oxygen Sulphur dioxide

II Sulphur dioxide and oxygen Sulphur trioxide

Sulphur trioxide and concentrated sulphuric acid Oleum II

Oleum and water Sulphuric acid

15

Listen carefully to the text read by the teacher. Answer questions 27, 28 and 29. 27. Polymer is made up of

………………………………………………………………………………..………………

28. State two examples of natural polymer

………………………. ……………………………………………..……………………....

29. Man-made polymers are known as

…………………………………………………………………………………………...…..

Listen carefully to the text read by the teacher. Answer questions 30, 31 and 32. 30. State three examples of ceramic.

………………………………………………………………………………………………

.………………………………………………………………………………………..……

………………………………………………………………………………………………

31. Ceramics are made of ……………………………………………………………………………………………….. 32. State two properties of ceramic. ………………………………...……………………………………………..………………

…………………………………………..…………………………………………...………

Kimia Module 1-5 Diagnostik f4

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