1 modul tft 2014 (1)

CHEMISTRY 2 SPM 2014
TRAINING FOR TRAINERS YAYASANTERENGGANU
CHAPTER 2 : THE STRUCTURE OF THE ATOM
1 (a) Table 1.1 shows four substances and their chemical formula.
Substance Chemical Formula
Magnesium chloride MgCl2
Chlorine Cl2
Neon Ne
Naphthalene C10H8
Table 1.1
Based on Table 1.1;
(i) State one substance which exists as a molecule.
.......................................................................................................................................................
[1 mark]
(ii) Which substance has the highest melting point?
.......................................................................................................................................................
[1 mark]
(iii) Molten naphthalene cannot conduct electricity, but molten magnesium chloride can conduct
electricity. Explain why.
........................................................................................................................................................
........................................................................................................................................................
........................................................................................................................................................
[2 marks]
(b) Why neon is an unreactive element?
..................................................................................................................................................................
[1 mark]

(c) Diagram 1.2 shows the graph of temperature against time when solid naphthalene is heated.
Diagram 1.2
(i) What is represented by 80 o
C?
.......................................................................................................................................................
[1 mark]
(ii) Draw the arrangement of particles in naphthalene from A to B?
[1 mark]
(iii) Why there is no change in temperature from B to C?
........................................................................................................................................................
........................................................................................................................................................
........................................................................................................................................................
[2 marks]
Time / s
Temperature / o
C
80
D
CB
A
t1 t2

2 Diagram 2 shows the chemical symbols which represent three elements P,Q and R.
The letters used are not the actual symbol of the elements.
9
P
4
32
Q
15
31
R
15
Diagram 2
(a) (i) What is meant by nucleon number?
………………………………………………………………………………………………..
[1 mark]
(ii) State the proton number of atom P.
………………………………………………………………………………………………..
[1 mark]
(b) What is represented by the number 32 for the element Q?
……….……………………………………………………………………………………………..
[1 mark]
(c) (i) Atom Q and R are isotopes. State the difference between the two atoms.
..…………………………………………………………………………………………………
[1 mark]
(ii) State one use of any isotopes in daily life.
……………….…………………………………………………………………………………
[1 mark]
(d) (i) Write the electron arrangement of atom Q.
………………………………………………………………………………………………..
[1 mark]
(ii) Determine the number of valence electron for atom Q.
………………………………………………………………………………………………..
[1 mark]
(iii) Draw the diagram of atomic structure for atom R.
[2 marks]

CHAPTER 3 : CHEMICAL FORMULAE & EQUATIONS
3 (a) Diagram 3.1 shows the molecular formula of glucose.
C6H12O6
Diagram 3.1
(i) What is the meaning of molecular formula?
…………………………………………………………………….…………………........................
…………………………………………………………………….…………………........................
[1 mark]
(ii) Write the empirical formula of glucose.
…………………………………………………………………….…………………........................
[1 mark]
(iii) Compare and contrast between molecular formula and empirical formula of glucose.
…………………………………………………………………….…………………........................
…………………………………………………………………….…………………........................
[2 marks]
(b) Diagram 3.2 shows a balance chemical equation.
2KI(aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbI2(s)
Diagram 3.2
Based on the equation, answer the following questions;
(i) What is the type of the reaction?
…………………………………………………………………….…………………........................
[1 mark]
(ii) State the name of the reactants and the products.
Reactants:…………………………………………………………………….…………………......
Reactants:…………………………………………………………………….…………………......
[2 marks]

(iii) State the physical state of PbI2
…………………………………………………………………….…………………........................
[1 mark]
(iv) In a reaction 20 cm3
of 0.5 mol dm-3
Pb(NO3)2 has reacted, calculate the mass of PbI2 formed.
[Relative atomic mass : I = 127 ; Pb = 207]
[3 marks]

4 Diagram 4 shows the apparatus set-up used in an experiment to determine the empirical formula of an oxide
of copper.
Diagram 4
The following data is obtained :
Mass of combustion tube + porcelain dish = 25.30 g
Mass of combustion tube + porcelain dish + copper oxide = 53.30 g
Mass of combustion tube + porcelain dish + copper = 47.70 g
(a) What is meant by empirical formula?
………………………………………………………………………………………………………….
………………………………………………………………………………………………………….
[1 mark]
(b) How to ensure that all the copper oxide is completely reacted?
………………………………………………………………………………………………………….
………………………………………………………………………………………………………….
[1 mark]
(c) Based on the data given, determine the empirical formula of the copper oxide.
[Relative atomic mass: O = 16 ; Cu = 64]
[3 marks]
Copper oxide
Dry hydrogen gas
Bunsen burner
Porcelain dish

(d) Write the chemical equation for the reaction between hydrogen and the copper oxide.
……………….........................................................................................................................................
[1 mark]
(e) After the reaction is completed, hydrogen gas is allowed to flow continuously until the copper is
cooled to room temperature. Explain why.
……………….........................................................................................................................................
[1 mark]
(f) The empirical formula for magnesium oxide can be determined by direct heating of magnesium.
Draw a labelled diagram to show apparatus set-up to carry out this experiment.
[2 marks]

CHAPTER 4 & 5 : PERIODIC TABLE OF ELEMENTS + CHEMICAL BONDS
5 Table 5.1 shows the electron arrangement of elements U, V and W.
Element Electron arrangement
U 2.6
V 2.1
W 2.8.1
(a) Based on the Table 5.1,
(i) Identify one metal element and one non-metal element. [2 marks]
(ii) State the group and period of element W in the Periodic Table of Elements. [2 marks]
(iii) The reaction between element U and W produces a compound.
 State one physical property of the compound.
 Draw the electron arrangement for the compound formed. [3 marks]
(b) Table 5.2 shows the observations of element V and element W when react with water.
Element Observation
V
Element V
Water
Element V, moves slowly at random on the water surface with a little ‘hissing’
sound.
The solution formed turns the colour of red litmus paper to blue.
W
Element W
Water
Element W, moves rapidly at random on the surface of the water with a louder
‘hissing’ sound.
The solution formed turns the colour of red litmus paper to blue.
Table 5.1
Table 5.2

(i) Write the chemical equation when element V reacts with water. [3 marks]
(ii) Compare the reactivity of elements V and W when react with water.
Explain your answer. [4 marks]
(c) Diagram 5.3 show the set up apparatus used to compare the electrical conductivity of solution P
and solution Q.
Based on the observations in Diagram 5.3,
(i) Identify the type of compound of solution P and solution Q. [2 marks]
(ii) Explain why there is a difference in the observations. [4 marks]
Solution Q
Carbon electrode
Solution P
Bulb lights up Bulb does not light up
Diagram 5.3

6 (a) Magnesium atom and chlorine atom are unstable. Both atoms react to form an ionic compound which
is more stable. Diagram 6.1 shows the electron arrangement of ionic compound that is produced by
the formation of an ionic bond between magnesium ion, Mg2+
, and chloride ion, Cl-
.
Diagram 6.1
(i) How are magnesium ion and chloride ion formed from their respective atoms?
Magnesium ion : …………………………………………………………….…………………
Chloride ion : …………………………………………………………….…………………
[2 marks]
(ii) Write the formula for the compound formed.
……………………………………………………………………………………………………..
[1 mark]
(iii) Name the force that exists between these ions in the compound.
……………………………………………………………………………………………………..
[1 mark]
(iv) The melting point of ionic compound in Diagram 10.1 is 851 o
C and its boiling point is 1423 o
C.
What will happen to the ions in this compound at 950 o
C?
……………………………………………………………………………………………………..
[1 mark]
(v) Give a reason for your answer in 6 (a) (iv).
……………………………………………………………………………………………………..
[1 mark]
Cl
-
Cl
-
Mg
2+

(b) Diagram 6.2 shows the standard symbol for an atom of two elements K and L.
The letters used do not represent the actual symbols of the elements.
16
K
8
12
L
6
Diagram 6.2
(i) Draw the diagram of electron arrangement to show the compound formed between element K
and element L.
[2 marks]
(ii) Compound formed in 6 (b) (i) has a low melting point. Explain why.
……………………………………………………………………………………………………..
……………………………………………………………………………………………………..
[2 marks]

CHAPTER 6 : ELECTROCHEMISTRY
7 A student is carried out the electrolysis of dilute silver nitrate solution by using carbon electrodes.
Table 7 below shows the result of the experiment.
Experiment Description Observation
Electrolysis of dilute silver nitrate solution
 Shiny-silvery solid is deposited at cathode.
 Gas bubbles are released at anode.
Table 7
(a) What is the energy change occurs in this electrolysis process?
......................………………………………………………………………..…......................................
[1 mark]
(b) (i) Write the formula of all ions present in silver nitrate solution.
......................………………………………………………………………..…...........................
[1 mark]
(ii) In the table below, state the ions which moved to the anode and cathode in the electrolysis.
Anode Cathode
[2 marks]
(iii) State the name of the ion selected to be discharged at cathode. Explain why.
……………...................................................................................................................................
……………...................................................................................................................................
[2 marks]
(c) (i) Write the half equation at anode.
……………...................................................................................................................................
[1 mark]
(ii) Describe briefly how you would verify the gas released at the anode.
……………...................................................................................................................................
……………...................................................................................................................................
[2 marks]

(d) Draw the diagram of apparatus set up to carry out this electrolysis.
In your diagram, show how the gas is collected.
[3 marks]

8 Diagram 8 shows the set-up of apparatus of electrolysis of 0.001 mol dm-3
copper(II) sulphate solution
using carbon electrodes; P and Q.
(a) Write the formula of all the ions present in copper(II) sulphate solution.
……………………………………………………………………………………………......................
[1 mark]
(b) (i) State the observation obtained at carbon electrode P.
………………………………………………………………………………………....................
[1 mark]
(ii) Write the half equation for the reaction that takes place at electrode P.
………………………………………………………………………………………....................
[1 mark]
(c) State the name of the gas released at electrode Q. Describe a test to identify the gas.
……………………………………………………………………………………………......................
……………………………………………………………………………………………......................
……………………………………………………………………………………………......................
[3 marks]
(d) After 30 minutes, the colour of the copper(II) sulphate solution change from dark blue to light blue.
Why?
……………………………………………………………………………………………......................
[1 mark]
P Q
Carbon electrodes0.001 mol dm-3
of
copper(II) sulphate
solution
Diagram 8

(e) If the experiment is repeated using copper electrodes,different product is formed at the anode.
(i) State the name of the product.
………………………………………………………………………………………....................
[1 mark]
(ii) Write the half equation occurred at the anode.
………………………………………………………………………………………....................
[1 mark]
(f) If the experiment is repeated using 2.0 mol dm-3
of copper(II) chloride solution, different product is
formed at the anode. Explain the difference.
………………………………………………………………………………………..............................
………………………………………………………………………………………..............................
………………………………………………………………………………………..............................
[3 marks]

CHAPTER 7 : ACIDS AND BASES
9 Diagram 9 shows the apparatus set-up for the neutralisation reaction between nitric acid and potassium
hydroxide solution for preparation of salt S.
Diagram 9
(a) State the colour change of the solution in the conical flask at the end point.
.................................................................................................................................................................
[1 mark]
(b) (i) State the name of salt S.
.......................................................................................................................................................
[1 mark]
(ii) Write a chemical equation for the above reaction.
.......................................................................................................................................................
[1 mark]
(iii) Calculate the maximum mass of the salt S formed.
[Given that molar mass of salt S = 101 g mol-1
]
[3 marks]
20.0 cm3
of 0.5 mol dm-3
potassium hydroxide
solution
+ phenolphthalein
20.0 cm3
of 0.5 mol dm-3
nitric acid

(c) (i) The experiment is repeated with 0.5 mol dm-3
sulphuric acid to replace nitric acid.
Predict the volume of sulphuric acid needed to neutralise the potassium hydroxide solution
completely.
........................................................................................................................................................
[1 mark]
(ii) Explain your answer in (c) (i).
........................................................................................................................................................
........................................................................................................................................................
........................................................................................................................................................
[2 marks]
10 Table 10 shows three solutions with their molarity and pH value respectively.
Solution Molarity pH value
P 1.0 mol dm-3
1
Q 1.0 mol dm-3
13
ammonia 1.0 mol dm-3
9
Table 10
(a) Suggest one name for solution P and solution Q. [2 marks]
(b) Solution P reacts with magnesium to form solution R and gas S.
Based on your suggestion in 17 (a), state the solution R and gas S.
Write the chemical equation involved. [4 marks]
(c) Based on Table 10, explain the different of pH value between solution Q and ammonia solution.
[4 marks]
(d) By using suitable apparatus,solution P and solution Q that you named in 17 (a),describe a laboratory
experiment to obtain the molarity of solution P.
In your description, include the chemical equation and the calculation steps involved. [10 marks]

CHAPTER 8 : SALTS
11 Diagram 11.1 shows a series of reaction for salt S which is a green colour compound.
Salt S is heated strongly to produce black residue of compound T and gas U.
Compound T reacts with sulphuric acid to form blue solution of compound W.
Diagram 11.1
Based on Diagram 11.1,
(a) (i) Suggest one formula of the anion in salt S. [1 mark]
(ii) Identify salt S, compound T, gas U and compound W. [4 marks]
(b) Write a chemical equation for the reaction between compound T and sulphuric acid. [1 mark]
(c) Compound W is a soluble salt. Describe chemical test to verify the cation and anion in compound W.
[4 marks]
(d) Diagram 11.2 shows the chemical equation for the reaction between blue solution of compound W
and barium nitrate solution.
Based on diagram 11.2;
(i) State the name of salt X and salt Y. [2 marks]
(ii) State one observation and name the type of reaction occurred. [2 marks]
(iii) Compound W reacts with 50 cm3
of 0.1 mol dm-3
barium nitrate solution.
Write the ionic equation for the reaction and calculate the mass of salt X produced.
[Molar mass of salt X = 233 g mol-1
] [4 marks]
Diagram 11.2
Compound W(aq) + Ba(NO3)2(aq) → Salt X(s) + Salt Y(aq)
Salt S Compound T Gas U
Compound W
+ H2SO4
Heat
+
Lime water turns cloudy
Pass through
lime water

12 (a) Zinc sulphate can be prepared through the reaction between sulphuric acid and zinc carbonate.
Write the chemical equation for the reaction occurred and calculate the mass of the salt formed if
0.1 mol of zinc carbonate used.
[Given that molar mass of zinc sulphate = 161 g mol-1
] [4 marks]
(b)
Suggest zinc W salt, salt X, salt Y and substance Z.
Write the chemical equation for the Reaction II. [6 marks]
(c) Describe an experiment to prepare zinc carbonate salt in laboratory.
Write the chemical equation for the reaction to prepare the salt. [10 marks]
 Zinc carbonate can be prepared through Reaction I:
between the solution of zinc W salt and solution of X salt
 Zink W salt can be prepared through Reaction II:
between substance Z and zinc carbonate
Solution of zinc W salt Solution of X salt Zinc carbonate Solution of Y salt
+
Reaction I
Substance Z
+
+
Reaction II

CHAPTER 9 : MANUFACTURED SUBSTANCES IN INDUSTRY
13 (a) Diagram 13.1 shows the production of ammonium sulphate from the reaction between substance X
and substance Y. Substance X is produced from Contact process whereas substance Y from Haber
process.
Diagram 13.1
(i) State the name of substance X and substance Y.
X : …………………………………………………………………………
Y : ………………………………………………………………………… [2 marks]
(ii) State one use of ammonium sulphate in agriculture field.
……………………………………………………………………………….......................
[1 mark]
(iii) Write the chemical equation for the reaction between substance Xand substance Y.
……………………………………………………………………………….......................
[2 marks]
(b) Diagram 13.2 shows the structural formula of ethene.
Ethene is the monomer used to produce a synthetic polymer called polyethene.
Diagram 21.2
(i) What is polymer?
……………………………………………………………………………………………..
……………………………………………………………………………………………..
[1 mark]
Contact process
Haber process
X
Y
Ammonium sulphate
HH
H HC C

(ii) Name the process for the formation of polyethene.
……………………………………………………………………………………………..
[1 mark]
(iii) Draw the structural formula of polyethene.
[1 mark]
(iv) Disposal of the polymer by burning is not suitable. Give a reason.
……………………………………………………………………………………………..
[1 mark]
(v) Suggest two ways how to solve the problems in (b) (iii) and (b) (iv).
……………………………………………………………………………………………..
……………………………………………………………………………………………..
[2 marks]

14 (a) Diagram 14.1 shows railway tracks and the arrangement of atom in alloy that made the railway tracks.
The alloy is made-up by mixing iron with element M.
(i) State the name of the alloy X
……………………………………………………………………………………………………
[1 mark]
(ii) State the name of atom M.
……………………………………………………………………………………………………
[1 mark]
(iii) Draw the arrangement of atoms in pure iron.
[1 mark]
(iv) Explain the difference in terms of hardness of alloy X and pure iron.
……………………………………………………………………………………………………
……………………………………………………………………………………………………
……………………………………………………………………………………………………
[3 marks]
Alloy X
Atom iron
Atom M
Diagram 14.1

(b) Table 14.2 shows three manufactured substances in industry; X, Y and Z and their uses.
Substances Use
A To make glass cookware
B To make water storage tanks
C To make the aeroplanes body
Table 14.2
(i) State the name of the following substances:
A : …………………………………………………………………………………....................
B: …………………………………………………………………………………....................
C: …………………………………………………………………………………....................
[3 marks]
(ii) Explain how substance B can cause environmental pollution.
………………………………………………………………………………………..................
………………………………………………………………………………………..................
[2 marks]

CHAPTER 10 : RATE OF REACTION
15 (a) Ahmad dissolve a spoon of salt X in 20 cm3
of water at different temperature.
Table 15.1 shows the temperature and the time taken for the salt X dissolved completely.
Beaker Temperature (o
C) Time taken (s)
A 30 30
B 50 10
Table 15.1
Compare the time taken for the salt X to dissolve in water in both beakers.
Give a reason for your answer. [2 marks]
(b) A group of student carried out and experiment to determine the rate of reaction between excess zinc
and 20 cm3
of 0.2 mol dm-3
nitric acid.
(i) Write a chemical equation for the reaction between zinc and nitric acid.
Name the gas released.
Calculate the maximum volume of the gas released.
[Given; 1 mol of any gas occupied 24 dm3
at room condition] [6 marks]
(ii) Draw a suitable diagram of apparatus set-up used in this experiment. [2 marks]
(iii) Table 15.2 shows the results obtained from the experiment.
Time / s 0 30 60 90 120 150 180 210 240 270 300
Volume ofgas / cm3 0 13 22 32 38 41 44 45 45 45 45
Table 15.2
Based on Table 15.2;
 Plot the graph of the volume of gas released against time for the experiment on the
graph paper provided.
[4 marks]
 Based on the graph, calculate the:
 Average rate of reaction for the whole reaction
 Average rate of reaction between 60 s to 120 s
 Rate of reaction at 120 s
[6 marks]

16 Experiments I and II are carried out to investigate the effect of different sizes of solid Y on the rate of
reaction. Table 16 shows the reactants and time taken to collect 30 cm3
of colourless gas.
Experiment Reactants
Time taken to collect
30 cm3
of gas
/s
I
2 g of solid Y
+ 40 cm3
of 0.1 mol dm-3
hydrochloric acid
120
II
2 g of solid Y
+ 40 cm3
of 0.1 mol dm-3
hydrochloric acid
90
Table 16
Based on the information in Table 16,
(a) (i) Suggest the size of solid Y in Experiment I and Experiment II. [2 marks]
(ii) Suggest the name of solid Y.
By using the suggested chemical substance of solid Y, write the chemical equation for the
reaction between the solid Y and hydrochloric acid.
[3 marks]
(iii) Calculate the maximum volume of gas released in the experiment.
[Molar volume of gas at room conditions = 24 dm3
mol-1
]
Based on the volume of gas obtained in (a) (iii), sketch the graph volume of gas liberated
against time for both experiments on the same axes.
[5 marks]
(iv) Draw the apparatus set-up for the experiment. [3 marks]
(b) (i) Calculate the average rate of reaction for Experiment I and Experiment II. [3 marks]
(ii) By using the name of solid Y in (a) (ii) and the calculation in (b) (i), compare the rate of
reaction between Experiment I and Experiment II. Explain the different in rate of reaction with
reference to the collision theory.
[5 marks]

CHAPTER 11 : CARBON COMPOUNDS
17 Table 17 shows molecular formulae of four carbon compounds.
Compound Molecular Formula
A C4H8
B C4H10
C C4H9OH
D C2H5COOH
Table 17
(a) Write the general formula of the homologous series of compound B.
……..………………………………………………………………………………………....................
[1 mark]
(b) State the functional group of compound A and compound D
Compound A : ………………………………………………………………………….....................
Compound D : ………………………………………………………………………….....................
[2 marks]
(c) Compound B shows isomerism. Draw the structural formula of all isomers of compound B.
[2 marks]
(d) Compound C and compound D are reacted with the presence of the concentrated sulphuric acid.
(i) Name the product formed from the reaction.
……………………………………………………….………………………………..................
[1 mark]
(ii) State one special characteristic of the product formed.
……………………………………………………….………………………………..................
[1 mark]

(e) Compound A burns in excess oxygen to produce carbon dioxide and water.
(i) Write a balanced chemical equation for the reaction.
........................................................................................................................................................
[2 marks]
(ii) Calculate the number of carbon dioxide molecules formed when 11.2 g of compound A is
burnt in excess oxygen.
[Relative atomic mass C = 12, O = 16 and Avogadro constant = 6.02 × 1023
]
[3 marks]

18 Table 18.1 shows the information of two compounds; P and Q.
Compound
General
formula
Molar mass
(g mol-1
)
Reaction with bromine water without
the presence of ultra violet light
P CnH2n 84 Brown colour is decolourised
Q CnH2n+2 86 Brown colour remains
Table 18.1
[Given that, relative atomic mass of H = 1 ; C = 12]
(a) Based on Table 18.1;
(i) Identify the homologous series for compound P and compound Q. [2 marks]
(ii) Determine the molecular formula and state the name of compound Q. [3 marks]
(b) (i) Explain the differences in observation between P and Q when they react with bromine water.
[4 marks]
(ii) Write the chemical equation for the reaction between compound P with bromine water.
Draw the structural formula and state the name of the product formed in this reaction.
[3 marks]
(c) Compare the sootiness of flame when compound P and Q are burnt in excess oxygen. Explain why.
[4 marks]
(d) Diagram 18.2 shows a series of changes occurred to compound P.
Based on the Diagram 18.2, compare the compound R and S in terms of:
 general formula
 functional group [4 marks]
END OF MODULE
P
Diagram 18.2
+ H2O
R
+ Acidified KMnO4
+ KMnO4 berasid
S

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