Chapter 2:
Subatomic particles: Proton, Electron , Neutron
Type of particles: Atom, Ion, Molecule
Why substance X has high melting point?
- because it has strong attraction forces between its particles
- therefore required more heat energy to over come the forces.
Why substance P has low boiling point?
- because it has weak attraction forces between its particles
- therefore required less heat energy to over come the forces.
Please also master the following definition or meaning.......
Chapter 2: The Structure of the Atom
A. Knowledge (Definition, meaning and facts)
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Check
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1)
State the kinetic theory of matter.
State one example to support the kinetic theory of matter
2)
What are atom, molecule and ion?
3)
What is melting point?
4)
Define proton number and nucleon number.
5)
State the meaning of isotopes.
6)
State the uses of isotopes such as carbon-14
and cobalt-60.
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B. Understanding / Application / Analysis
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7)
Explain why the temperature remains unchanged
during the melting process.
8)
Explain why the temperature remains unchanged
during the freezing process.
9)
A solid compound is heated until it converts
into gas. Explain the changes in
energy content, forces of attraction between the particles, and arrangement
of particles.
10)
State the main subatomic particles of an atom.
Compare and contrast the relative atomic mass and the relative charge of the subatomic particles of the atom.
11) 23 Al is the symbol of aluminium.
17 (a) Determine the number of neutron of aluminium. (b) Draw the electron arrangement of aluminium. |
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C. Synthesis (Experiment)
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12)
Solid Z has a melting point of 65oC.
Describe a laboratory experiment to determine the melting point of Z. Your
answer should show how the melting point of Z is determined.
13)
Compound W has a freezing point of 82oC.
Describe a laboratory experiment to determine the freezing point of W.
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Chapter 3: Chemical Formulae and Equations
A. Knowledge (Definition, meaning and facts)
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Check
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1) State
the meaning of relative atomic mass based on carbon-12 scale.
2)
Define a mole.
3)
State the meaning of molar mass
4)
State the meaning of molar volume of gas.
5)
State the meaning of empirical formula.
6)
State the meaning of molecular formula.
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B. Understanding / Application / Analysis
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7)
Explain why we couldn’t determine the
empirical formula of copper(II) oxide by heating copper powder in a crucible.
8)
Compare and contrast empirical formula with
molecular formula using ethane as an example.
9)
Vinegar is a dilute ethanoic acid with a
molecular formula of CH3COOH.
(a) Find the empirical formula of ethanoic acid. (b) Find the percentage composition by mass of carbon in ethanoic acid.
10)
3.6 g of carbon reacted with 0.8 g of hydrogen
to form a compound.
(a) Determine the empirical formula of the compound formed. (b) Given that the relative molecular mass of the compound is 88 g, find its molecular formula.
[Relative
atomic mass: C ,12; H, 1]
11)
Hydrogen Gas is reacted with 20 g of hot
copper(II) oxide powders to produce solid copper and water.
(a) Write the chemical equation for the reaction. (b) Calculate the maximum mass of solid copper formed. [Relative atomic mass: Cu, 64; O,16; H,1] |
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C. Synthesis (Experiment)
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12)
Describe a laboratory experiment to determine
the empirical formula of magnesium oxide.
Your answer should include all the precautions and calculations involved. [Relative atomic mass: Mg, 24; O,16] |
Check
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1) State
the basic principle of arranging the elements in the Periodic Table from its
proton number.
2)
State the physical properties of Group 1.
3)
State the physical properties of Group 17.
4)
State the changes in the atomic size and
electronegativity of elements across Period 3.
5)
State three special properties of transition
elements?
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B. Understanding / Application / Analysis
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6)
State the position of element 39 X in Periodic Table.
Explain your answer.
20
7)
When across Period 3 from sodium to argon, the
atomic size decreases. Explain why.
8)
When across Period 3 from sodium to argon, the
electronegativity increases. Explain why.
9)
The reactivity of Group 1 increases when going
down the group. Explain why.
10)
The reactivity of Group 17 decreases when
going down the group. Explain why.
11)
Why helium gas is not reactive?
12)
X is an element from Group 1. X in burnt in
oxygen and the product is dissolved in water. What is the property of the solution
formed? Explain Why.
13)
Chlorine gas is dissolved in water.
What can
you observe if a piece of blue litmus paper is immersed into the solution
formed? Explain why.
14)
W is an element from Group 1. Predict the
chemical reaction of W with:
a) water,
b) Oxygen,
State the observation and write the chemical equation involve. |
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C. Synthesis (Experiment)
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15)
Describe a laboratory experiment to compare
the reactivity of elements in Group 1: lithium, sodium and potassium.
16)
Describe a laboratory experiment to compare
the reactivity of chlorine, bromine and iodine in the reaction with iron
wool. State the observation and write the chemical equations involve in reactions.
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Chapter 5: Chemical Bonds
A. Knowledge (Definition, meaning and facts)
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Check
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1) What
is anion?
2)
What is cation?
3)
State two physical properties of ionic
compounds.
4)
State two physical properties of covalent compounds.
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B. Understanding / Application / Analysis
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5)
Explain why sodium chloride can conduct
electricity in aqueous state but cannot conduct electricity in solid state.
6)
Magnesium chloride and hydrogen chloride are
two compounds of chlorine. At room condition,
magnesium chloride exists as a solid but hydrogen chloride exists as a gas.
Explain why.
7)
Describe the formation of ionic bond in sodium
chloride, NaCl.
8)
By using example, describe the formation of covalent
bond between element from Group 14 and element from Group 17.
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C. Synthesis
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9)
Draw electron arrangement of the compound
formed from the following elements.
a) Nitrogen
and hydrogen,
b) Carbon
and oxygen,
c) Magnesium
and chlorine,
d) Carbon
and hydrogen,
e) Hydrogen
and chlorine,
f) Sodium
and oxygen.
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Chapter 6: Electrochemistry
A. Knowledge (Definition, meaning and facts)
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Check
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1) State
the meaning of electrolyte.
2) State
the meaning of electrolysis.
3) State
three factors affecting electrolysis of an aqueous solution.
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B. Understanding / Application / Analysis
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4) Explain
why solution of hydrogen chloride in water can conduct electricity but
solution of hydrogen chloride in methylbenzene cannot conduct electricity?
5) By
using example, explain how the following factors can determine the selective
discharge of ions at the electrodes.
a) Types
of electrodes,
b) Concentration
of the ions.
6)
Describe the electrolysis of molten lead(II)
bromide.
7)
Describe the extraction of aluminium by
electrolysis.
8)
Draw the structure of Daniell cell and explain
how it can produce electricity.
9)
Draw the structure of a dry cell and explain
how it can produce electricity.
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C. Synthesis
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10)
Describe a laboratory experiment to extract lead
from lead(II) oxide by using electrolysis.
11)
Describe a laboratory experiment to show that
types of electrodes affecting the selective discharge of ions in electrolysis
of copper(II) sulphate solution.
12)
You are given magnesium ribbon, copper plate, magnesium
nitrate solution, copper(II) sulphate solution, connecting wires with
crocodile clips, 250 cm3 beaker, voltmeter and porous pot.
Construct a voltaic cell by using the above materials. Explain how the voltaic cell can produce electricity. Your answer must include observation and half equations for reaction at anode and cathode.
13)
Describe a laboratory experiment to construct
the electrochemical series of magnesium, copper, zinc and lead.
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Chapter 7: Acids and Bases and Chapter 8: Salts
A. Knowledge (Definition, meaning and facts)
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Check
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1) State
the meaning of acid and alkali.
2) What
is the meaning of strong acid and weak alkali?
3) What
is neutralisation?
4)
What is salt?
5)
What is precipitate reaction?
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B. Understanding / Application / Analysis
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6)
The pH value of solution ammonia in water is 9
but the pH value of solution of ammonia in trichlomethane is 7. Explain why
the pH values of the two solutions are different.
7)
80 cm3 of distilled water is added
to 20 cm3 of 2.0 moldm-3 solution of HCl. Find the
molarity of the dilute solution.
8)
In a titration, 40 cm3 of 0.25
moldm-3 potassium hydroxide, KOH solution is needed to neutralise
20 cm3 of nitric acid, HNO3. Calculate the molarity of
the nitric acid, HNO3.
9)
Given dilute nitric acid and dilute sulphuric
acid have the same concentration of 0.5 moldm-3. In a
neutralisation experiment, 20 cm3 of nitric acid is required to
neutralise 20 cm3 of sodium hydroxide solution but only 10 cm3
of sulphuric acid is required to neutralise 20 cm3 of sodium
hydroxide solution. Explain why.
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C. Synthesis
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10)
Describe a chemical test to determine a given
solution is an acid solution.
11)
Describe a laboratory experiment to determine
the concentration of sodium hydroxide by using titration process. You are
given 0.2 moldm-3 of dilute sulphuric acid, phenolphthalein,
burette, pipette and conical flask.
12)
You are given solid sodium chloride. Describe
how to prepare sodium chloride solution of 0.2 moldm-3 in
laboratory by using 250 cm3 volumetric flask.
13)
Describe the preparation of zinc sulphate .
14)
Describe the preparation of lead(II) chloride.
15)
Describe the preparation of potassium nitrate.
16)
Solid W is a salt. Describe the tests you
would carry out to confirm the presence of zinc ions and nitrate ions in the
salt?
17)
Solid X is a metal carbonate. Describe the
tests you would carry out to confirm that X consists of carbonate ions besides
heating.
.
18)
You are given four test tubes filled with
solution consist of zinc ions, lead(II) ions, aluminium ions and magnesium ions
respectively. Describe the tests you would carry out to confirm the ion that
present in each test tube.
19)
You are given potassium chloride solution,
lead(II) oxide powder and dilute nitric acid.
Describe how you would prepare lead(II) chloride salt from the given materials.
20)
You are given dilute sulphuric acid,
copper(II) nitrate solution and sodium carbonate solution. Describe how you
would prepare copper(II) sulphate salt from the given materials.
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Chapter 9: Manufactured
Substance in Industry
A. Knowledge (Definition, meaning and facts)
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Check
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1) What
is the meaning of alloy?
State the aims of making alloys.
2)
What is the meaning of composite materials?
State the components of the following composite materials:
a) Reinforced
concrete,
b) Superconductor,
c) Fibre
optic,
d) Fibre
glass,
e) Photochromic
glass.
3)
State the catalyst, temperature and pressure of
the following process:
a) (a)
Contact process
b) (b)
Haber process
4)
What is the meaning of polymers?
Name the monomer of polythene and polyvinyl chloride.
5)
State four types of glass and their
compositions. List the uses of each glass.
6)
What is ceramics? State the properties
and list the uses of ceramics.
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B. Understanding / Application / Analysis
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7)
Bronze is an alloy consists of copper and tin.
Explain why bronze is harder than copper.
8)
Explain how acid rain is formed.
Describe how acid rain causes environmental pollution.
9)
Explain
the industrial process involved in the manufacture of sulphuric acid.
Write all the chemical equations involve.
10)
Explain the industrial process involved in the
manufacture of ammonia gas.
Write all the chemical equations involve. |
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C. Synthesis
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11)
Describe a laboratory experiment to prepare
ammonium sulphate (ammonium fertiliser)
12)
Describe a laboratory experiment to compare
the hardness of brass and copper.
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Chapter 10: Rate of Reaction
A. Knowledge (Definition, meaning and facts)
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Check
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1) What
is rate of reaction?
2)
What is stated in the collision theory?
3)
What is activation energy?
4)
What is effective collision?
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B. Understanding / Application / Analysis
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5)
Explain how surface area (size of reactant)
can increase the rate of reaction based on collision theory.
6)
Explain how temperature can increase the rate
of reaction based on collision theory.
7)
Explain how catalyst can increase the rate of
reaction based on collision theory.
8)
Explain why hydrochloric acid of 2.0 moldm-3
is reacted faster with zinc compare to hydrochloric acid of 0.5 moldm-3
.
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C. Synthesis
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9)
Hypothesis: The smaller the size of reactant,
the higher the rate of reaction.
Describe a laboratory experiment to confirm the hypothesis by using the reaction between calcium carbonate and hydrochloric acid.
10)
Describe a laboratory experiment to show that
the presence of catalyst will increase the rate of decomposition of hydrogen
peroxide.
11)
Describe a laboratory experiment to show that
an increase in temperature will increase the rate of reaction between sodium
thiosulphate solution and sulphuric acid.
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Chapter 11: Carbon compounds
A. Knowledge (Definition, meaning and facts)
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Check
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1) What
is homologous series?
2) What
is saturated hydrocarbon and unsaturated hydrocarbon? State an example of
each of them.
3) Explain
what is isomers and isomerism by using butane as an example.
4) What
is polimer? State an example of polymer and its monomer.
5) What
are saturated and unsaturated fats?
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B. Understanding / Application / Analysis
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6)
Explain what is isomers and isomerism by using
butane.
7)
Explain why ethene gas can decolourises the acidified
potassium mangante(II) solution but ethane can not decolourises acidified
potassium mangante(II) solution.
8)
Explain why both hexane and hexane have six
carbon atoms but hexene burns with a more sooty flame.
9)
Pentane and propane are members from alkane
family. Explain why the melting point
of pentane is higher than propane.
10)
Propanol and propanoic acid are dissolved in
water. It is found that propanol solution is a neutral but propanoic acid is
an acid solution.
11)
Explain the coagulation process of latex.
12)
Explain how to prevent coagulation of latex.
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C. Synthesis
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13)
Describe a test to differential hexene and
hexane.
14)
Describe a laboratory experiment to prepare
ethane gas from ethanol.
15)
Describe a laboratory experiment to prepare
ethanoic acid gas from ethanol.
16)
Ethylpropanoat is a product from reaction
between alcohol and carboxylic acid.
(a) State two physical properties of ethylpropanoat. (b) Describe a laboratory experiment to prepare Ethylpropanoat. Your answer must include the drawing of the setup-apparatus and the chemical equation involve.
17)
Explain how to prepare propanoic acid from
propene.
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