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Summer assignment and revision notes / F3 to F4 Chemistry
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Christian Alliance S C Chan Memorial College
F3 to F4 Chemistry
Summer Assignment and Revision Notes
Name : ( ) Grade :
Class : F.4 ( ) Group : 4X / 4Y / 4Z
Welcome! You will be studying Chemistry in the coming three years. Here are some summer
assignments that you need to complete during this summer vacation.
Part 1 References : NSS Chemistry Curriculum (Secondary 4 6)
Part 2 Revision : Fundamental knowledge in Chemistry. ( Ch 1, 5-8 )
A quiz will be held in early September, 2011.
Part 3 Exercises : Q.1 to Q.9 covering Chapters 5 to 8 of Book 1B. You should hand-in this
assignment on 1 September, 2011.
Part 1 Reference : Chemistry Curriculum (Secondary 4 -6)
A. Compulsory Part
Topic Content
1 Planet Earth ( Book 1A)
1.1The atmosphere1.2The ocean1.3Rocks and minerals
F6
2 Microscopic World I ( Book 1B )
2.1 Atomic structure
2.2 Periodic Table
2.3 Metallic bonding
2.4 Structures and properties of metals
2.5 Ionic and covalent bond
2.6 Structures and properties of giant ionic substances
2.7 Structures and properties of simple molecular substances
2.8 Structures and properties of giant covalent structure
2.9 comparison of structures and properties of important types of substances
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and
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3 Metals ( Book 1C )
3.1 Occurrence and extraction of metals
3.2 Reactivity of metals
3.3 Reacting masses
3.4 Corrosion of metals and their protection
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4 Acids and Alkalis ( Book 2)
4.1 Introduction to acids and alkalis
4.2 Indicators and pH
4.3 Strength of acids and alkalis
4.4 Neutralisation and salts
4.5 Concentration of solutions
4.6 Volumetric work involving acids and alkalis
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5 Fossil Fuels and Carbon Compounds ( Book 2 )
5.1 Hydrocarbon from fossil fuels
5.2 Homologous series, structural formulae and naming of carbon compounds
5.3 Alkanes and alkenes
5.4 Addition polymers
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6. Microscopic world II ( Book 3 )
6.1 Bond polarity
6.2 Intermolecular forces
6.3 Structures and properties of molecular crystals
6.4 Simple molecular substances with non-octet structures
6.5 shapes of simple molecules
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7 Redox reactions, chemical Cells and electrolysis ( Book 3 )
7.1 Chemical cells in daily life
7.2 Reactions in simple chemical cells
7.3 Redox reactions
7.4 Redox reaction in chemical cells
7.5 Electrolysis
7.6 Importance of redox reactions in modern way of living
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and
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8. Energy changes in chemical reactions ( Book 3 )
8.1 Energy changes in chemical reactions
8.2 Standard enthalpy change of neutralization, solution, formation and
combustion
8.3 Hesss law
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9. Rate of reaction ( Book 4A )
9.1 Rate of chemical reaction
9.2 Factor affecting rate of reaction9.3 Molar volume of gases at r.t.p.
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10. Chemical equilibrium ( Book 4A )
10.1 Dynamic equilibrium
10.2 Equilibrium constant
10.3 The effect of changes in concentration and temperature on chemical
equilibria
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11. Chemistry of carbon compounds ( Book 4B )
11.1 Introduction to selected homologous series
11.2 Isomerism
11.3 Typical reaction of various functional groups
11.4 Inter-conversion of carbon compounds
11.5 Importance of organic substances
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12. Patterns in the Chemical World ( Book 4B )
12.1 Periodic variation in physical properties of the elements Li to Ar
12.2 Bonding, stoichiometric composition and acid-base properties of the
oxides of elements Na to Cl
12.3 General properties of transition metals
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B. Elective Part
Topic Content
13 Industrial chemistry ( Book 5 )
13.1 Importance of industrial processes
13.2 Rate equation
13.3 Activation energy
13.4 Catalysis and industrial processes
13.5 Industrial processes
13.6 Green Chemistry
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14 Material chemistry ------
15 Analytical chemistry ( Book 7 )
15.1 Detecting the presence of chemical species
15.2 Separation and purification methods
15.3 Quantitative methods if analysis
15.4 Instrumental analytical methods
15.5 Contribution of analytical chemistry to our society
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Part 2. Revision
Pleasestudy wellthe following fundamental knowledge of Chemistry.
You will have a quiz in early September. The quiz will cover chapters 1, 5 to 8.
Chapter 1 Fundamentals of Chemistry
What is chemistry?
The study of substances, about their
- compositions,- structures,- properties ( physical and chemical ) and- the changes among them.
Chemistry is closely related to our daily life, for examples :
- Clothing, Food , Housing , Transport , Medicines , etc.
Classifications of matter:
Element:- a pure substance that cannot be broken down into anything simpler by chemical methods
- a pure substance that is made up of one kind of atoms only
Compound: a pure substance made up of two or more elements chemically combined together
Mixture : consists of two or more pure substances ( elements or compounds ) which haveNOT chemically combined together.
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Observations in experiments include FOUR activities :- Seeing with eyes , i.e. What color change , gas bubbles produce , solid dissolve,
precipitate form / what color flame/ ...
- Feeling with hands, i.e. solution become hot / warm / cold /
- Smelling with nose , i.e. with burning smell , choking / pungent smell,
- Hearing with ears , i.e. hissing sound produce , burn with pop sound,
Physical change : occur without changing into new substances ,usually just involves states change ( solid , liquid , gas )
Chemical change: occur chemical reactions involved, i.e. new substances are formed
Physical and chemical properties of substances
Physical properties of substances are those properties that can be determined without thesubstance changing into another into substance.
ExamplesPhysical
Property Chalk Iron clip Table salt Water
appearance white solid Shiny silver solid White solid
odour --- --- No smell
taste --- --- Salty
hardness hard but brittle hard Hard
Density* Low high ----
Solubility ( in
water )
Insoluble Insoluble Soluble
Malleability &
ductility
non malleable
& non-ductile/
hard but brittle
Malleable &
ductile
non malleable
& non-ductile
Electrical
conductivity
Non-conductor
/ insulator
Good conductor Non- ( solid state)
Cond- ( molten )
Thermal
conductivity
Poor thermal
conductor
Good thermal
conductor
Poor thermal
conductor
Melting points
and boiling point
Low high high
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Chemical properties :- of the substances are chemical reactions take place at the respective conditions.
e.g. rusting of iron
Iron only rusts if presence of water and oxygen.
e.g. burning of a candle
Candle can be burned if there are oxygen and with sufficient of energy supply to start
the reaction.
Hazard warning labels: ( Laboratory Handbook P.3 )Label Hazard Example Safety Precautions
Explosive -Potassium, Sodium,
explosive,
Keep away from heat and flame
Flammable Hydrogen , LPG,
town gas, alcohol,
- Keep away from heat and
flame
- stored in wellventilated place
Toxic Chlorine, carbon
monoxide, hydrogen
sulphide ,
-Handle it in the fume cupboard.
-Wear gloves
Carcinogenic Benzene ,
Tetrachloromethane,
Asbestos
-Handle it in the fume cupboard.
-Wear gloves
Oxidizing Concentrated nitric
acid , potassium
permanganate,
- wear gloves and safety glasses
Corrosive conc. acids ,
conc. alkalis,
- wear gloves and safety glasses
Harmful Lead compounds,
Trichloromethane,
- wear gloves and safety glasses
Irritant Dilute acids and
alkalis,
- wear gloves and safety glasses
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Chapter 5 Atomic structure
Classifications of Elements(i) By Physical states
- Solid ( 104 )
- Liquid ( 2 , Br and Hg )
- Gas ( 12 , H, He, N, O, F, Ne, Cl, Ar, Kr, Xe, Rn, Uuo)
(ii)
Metal and Non-metal
Properties of metals and non-metals:Properties Metals Non-metals
State
at room temp &
pressure ( r.t.p.)
All are solids
except Hg(l)
Most are gases (O2, N2, He, etc.),
Some are solids (C, S, etc),
one liquid (Br2)
Melting pt & boiling pt usually High Low, (except C, Si)
Appearance Shiny, silvery white;
(except Au and Cu ,
golden /shiny brown )
Dull ( except graphite ) and in
various colours
Hardness and strength usually Hard and strong Not uniform
Malleability & ductility Malleable & ductile Brittle
Density High Low
Thermal conductivity
and electrical
conductivity
All are good
conductors
Bad conductors of heat,
non-conductors of electricity,
(except graphite)
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Semi-metals (metalloids): boron and silicon (Si is a semi-conductor which is used in makingcomputers chip )
Subatomic particlesSymbol Relative mass Relative charge Position in atom
Proton p 1 + 1 Inside the nucleus
Neutron n 1 0 Inside the nucleus
Electron e- 0 - 1 Moving around nucleus
Full symbol of an atom: XAZ A: mass number = no. of p + no. of n (different for isotopes)
Z: atomic number = no. of p (fixed for each element)
Isotopes:Isotopes are atoms of the same element with the same number of protons ( atomic number )
but different number of neutrons ( mass number ).
Relative atomic mass ( R.A.M. ) :- is the averaged mass of isotopes of the element.
e.g. chlorine-35 & chlorine-37 have relative abundances 75% & 25% respectively,
the R.A.M. of chlorine = 35 x 75% + 37 x 25% = 35.5
( No unit ! One decimal place !)
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Patterns in the Periodic Table: Across a period, elements change from metals through semi-metals to non-metals
(i.e. more non-metallic)
An interesting rule: an element with group no. > period no. is a non-metal (except H andnoble gases)
Groups : similarities and trends down a group* Elements in the same group have similar chemical properties.
* Reactivity increases / decreases down the group.
Properties ofGroup I elements (alkali metals: Li, Na, K, Rb, Cs, Fr ):-- soft (can be cut by knife)
-- low density (float on water)
-- reactive (more reactive than other groups, stored under paraffin oil), e.g. all react with
water to form hydroxide solution and give off hydrogen; Observation of reaction of alkali
metals with water (p.144)
Reactivity of metals increases down the group
(reactivity: Li < Na < K < Rb < Cs < Fr)
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Properties ofGroup VII elements (halogens, X : F, Cl, Br, I, At ):-- poisonous
-- with pungent choking smell
-- form diatomic molecules, X2
-- m.p. & b.p. increases down the group: F2 : (g), Cl2 : (g), Br2 : (l), I2 : (s);
because van der Waals forces increase with the size of molecules
-- colour intensity increases down the group,
F2(g) : pale yellow
Cl2(g) : greenish yellow
Br2(l) : dark red / reddish brown Br2(aq) : orange / reddish brown, Br2(g): brown
I2(s) : dark purple /black I2(aq) : brown I2(g) : purple
I2(heptane) : purple
-- reactive :
Reactivity of non-metals decreases down the group
( reactivity : F > Cl > Br > I )
Properties ofGroup 0 elements (noble gases: He, Ne, Ar, Kr, Xe, Rn)-- colourless gases
-- density down the gp (He is less dense than air, but Xe is much denser than air)
-- exist as monoatomic molecules
-- m.p. & b.p. down the gp because van der Waals forces increase with molecular size
-- unreactive
(Qhaving stable electronic arrangement, He is duplet, the others are octet)
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Chapter 7 & 8 Chemical bonding : Ionic bonding (Ch.7) and Covalent bonding (Ch.8)
All ionic compounds can conduct electricity when they are in molten or in aqueoussolution
because ofmobile ions produced in molten state or in aqueous solution. (In solid state, theions are not mobile, but in molten or aqueous states, the ions become mobile!)
Ions:Cation: when atom loses e
-
, it becomes a cation and carries +ve charge, (usually metals
form cations)
Anion : when atom gains e-, it becomes an anion and carries ve charge, (usually
non-metals form anions)
Simple ion : a ion derived from a single atom.
Polyatomic ions : a ion derived from a group of atoms.
Examples :
Cl
chloride ion is a simple anion.
Na+
sodium ion is a simple cation.
SO42-
sulphate ion is a polyatomic anion.
NH4+
ammonium ion is a polyatomic cation.
Exercises :
OH
hydroxide ion is a .
Fe3+
is a
Br is a
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Names & formulae of ions: (names & formulae of ionic compounds)Cations Anions
Charge Formula Name Charge Formula Name
1+ Na+
K+
Cu+
Ag+
NH4+
H+
sodium
potassium
copper (I)
silver
ammonium
hydrogen
1- H
F-
Cl-
Br-
I-
OH-
NO3-
NO2-
HCO3-
HSO4-
MnO4-
ClO-
hydride
fluoride
chloride
bromide
iodide
hydroxide
nitrate
nitrite
hydrogencarbonate
hydrogensulphate
permanganate
hypochlorite
2+ Mg2+
Ca2+
Fe2+
Cu2+
Ni2+
Mn2+
Pb2+
Hg2+
Zn2+
magnesium
calcium
iron(II)
copper(II)
nickel(II)
manganese(II)
lead(II)
mercury(II)
zinc
2- O2-
S2-
SO42-
SO32-
CO32-
CrO42-
Cr2O72-
oxide
sulphide
sulphate
sulphite
carbonate
chromate
dichromate
3+ Al3+
Fe3+
Cr3+
aluminium
iron(III)chromium(III)
3- N3-
P3-
PO43-
nitride
phosphidephosphate
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Colours of ions:Fe
2+Fe
3+Cu
2+Ni
2+Cr
3+Cr2O7
2- Mn
2+ MnO4
-
pale green brown Blue/green green green orange Colourless purple
/ Very pale pink
Migration of ions: - Evidence of presence of ions ( in Book 1B, P.144-146 )
Under electric field / during electrolysis, the migration of coloured ions can be observed. For KMnO4, purple colour ( MnO4- ) is observed at the +ve electrode. ( Figure 7.5 ) For CuCr2O7, blue colour ( Cu2+ ) is observed at the ve electrode while orange colour
(Cr2O72-
) is observed at the +ve electrode. ( Figure 7.4 )
Expt.7.2 Migration of potassium and permanganate ions: Observation:
purple colour moves towards the +ve electrode Conclusion:
KMnO4 consists of colourless K+ ions and purple MnO4- ions. In aqueousKMnO4(aq), the ions become mobile. So, the negative, purple MnO4
-ions move
towards the +ve electrode while the positive, colourless K+
ions move towards
the ve electrode (which cannot be seen).
Note: the filter paper should be moistened with sodium sulphate solution to increaseelectrical conductivity (Qit provides more ions to conduct electricity)
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Summary and comparison of ionic and covalent bondings.
Ionic bonding Covalent bonding
Formed between metals & non-metals to
attain noble gas electronic arrangement
Formed between non-metals to
attain noble gas electronic arrangement
By e-transfer,
metal atoms lose e-to form cations (+);
non-metal atoms gain e-to form anions (-)
By e-sharing,
non-metal atoms share e-between nuclei to
form molecules, e.g. Cl2 , CH4, etc.
Strong non-directional electrostatic attraction
between +ve and ve ions.
Strong directional electrostatic attraction
between the shared electrons and the two
nuclei of the bonded atoms.
Electron diagram of MgF2
Ionic formula : ( F-
)(Mg2+
)( F-
) /(Mg
2+)( F
-)2
Empirical formula : MgF2
Electron diagram of NCl3
Structural formula:
Molecular formula : NCl3
* names & formulae names & formulae
of ions of ionic cpds
e.g. magnesium ion and fluoride ion
magnesium fluoride
with water of crystallization as:
n water
e.g. CuSO47H2O
copper (II) sulphate -7-water
* all ionic compounds are in giant ionic
structure, i.e. each Mg2+
ion is surrounded
by 6 F-ions and vice versa.
* molecular formula & structural formula
* single bond (), double bond (=),
triple bond ()
* bond pair electrons & lone pair electrons
* shapes of molecules: linear (CO2),
V-shaped (H2O), trigonal pyramidal
(NH3), tetrahedral (CH4)
* atomicity of molecules ( for elements )
monoatomic (He), diatomic (Cl2),
triatomic (O3)
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Ionic compound
An ionic compound ( or ionic substance ) is a compound which consists ions.
Covalent substance
A covalent substance is a non-ionic substance in which the atoms are held together by covalent
bonds.
Molecule
A molecule is the smallest part of an element or a compound which can exist on its own under
ordinary conditions.
Distinguish between name, symbol & formula of some elements:
Element Atomic / Chemical symbol Molecular formulaHydrogen H H2
Nitrogen N N2
Oxygen O O2
Chlorine Cl Cl2 ( for all halogens )
Helium He He ( for all noble gases )
Sodium Na ---
Sulphur S S8
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Part 3. Exercises
1. a) Complete the following table of particles and their particle composition. The particles
are either atoms or ions.
Number of
Particle Mass number Protons Neutrons Electrons
O
O 2
Cl
W 37 20 17
Y 37 17 18
Z 10 10
Ni
Ni2+
Ca
b) What is the relationship between 35Cl and particle W? Explain your answer.
c) What is the name of
(i) W ? (ii) Y ?
(iii) Z ?
d) Which of the above particles are metals ?e) Which of the above particles are ions ?
18
17
35
64
64
39
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2. The table below shows the colours of solutions of three ionic compounds containing four ions:
W+, X
2+, Y
2and Z
2.
Ionic compound Colour of solution of compound
W2Z Colourless
W2Y Orange
XZ Blue
Deduce and explain the colour of the ions :
W+(aq), X
2+(aq), Y
2(aq), Z
2(aq).
3. Iron occurs naturally as a mixture of four isotopes. The relative abundance of these isotopes is
tabulated below:
Isotope54
Fe56
Fe57
Fe58
Fe
Abundance (%) 5.84 91.68 2.17 0.31
a) What is meant by the term 'isotopes'?
b) Calculate the relative atomic mass of iron.
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4. An element X occurs naturally as a mixture of two isotopes. The relative atomic masses of
the two isotopes are 63.0 and 65.0. The relative atomic mass of X is 63.6. What is the
percentage abundance of the two isotopes?
5. The student places a drop of copper(II) chloride solution at A and a drop of potassium
permanganate solution at B.
microscopicslide
filter papermoistened withsodium sulphatesolution
20 V d.c. power supply+
A B
a) Why is the filter paper moistened with sodium sulphate solution?
b) Write the chemical formula of the ions responsible for the purple colour of potassium
permanganate.
c) What will be observed on the filter paper after an electric current is passed for about 10
minutes? Explain your answer.
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6. The table below gives the group number of four elements.
Element Symbol Group number
Caesium Cs I
Indium In III
Tellurium Te VI
Astatine At VII
a) Would you expect caesium to be a conductor of electricity? Explain your answer.
b) Give the chemical formula of caesium sulphate.
c) Give the chemical formula of indium oxide.
d) Give the chemical formula of tellurium oxide.
e) Caesium and astatine combine to form a compound.
(i) Draw the electron diagram of the compound. (showing the outermost shell electrons only.)
(ii) Would an aqueous solution of the compound conduct electricity? Explain your answer.
f) Astatine and hydrogen combine to form a compound.(i) Draw the electron diagram of the compound (showing the outermost shell electrons only.)
(ii) Give the chemical formula of the compound.
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7. W, X, Y and Z are four different elements. Their atomic numbers and electronic arrangements
of their atoms are as follows.
Element Atomic number Electronic arrangement of atom
W 14 (i)
X 18 (ii)
Y 35 p, q, 18, r
Z 37 p, q, 18, 8, s
a) Calculate the values of p, q, r and s in the above table.
b) In which groups and periods of the periodic table should Y and Z be placed?
c) (i) What is the electronic arrangement of atom
W : X :
(ii) In what way are the electronic arrangements of the atoms of W and X.
(1) similar to one another?
(2) different from one another?
d) Which TWO of the four elements would form
i) an ionic compound?
ii) a covalent compound?
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8. With reference to the part of the periodic table shown below, answer the following questions.
Group
I II III IV V VI VII 0
Period 2 Li Be B C N O F Ne
Period 3 Na Mg Al Si P S Cl Ar
Period 4 K Ca Cr Br
a) Name two elements which are mainly obtained from sea water.
b) Name two elements which are present in the free state ( elemental form ) on land.
c) Explain why argon is monoatomic.
d) Name a metal which can form a coloured anion. Give the chemical formula and colour of
this anion.
e) In what way are the electronic arrangements of the atoms of magnesium and calcium.
i) similar to each other?
ii) different to each other?
f) Point out the gradual change in the reactivity of Group I elements down the group.
g) Suggest TWO gradual changes in the physical properties of the Group VII elements down
the group.
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For Q.9, write your answer in full sentences and in paragraphs
9. "When atoms combine, they tend to achieve the electronic arrangements of atoms of noblegases."
Write an essay to discuss, with reference to suitable examples, how atoms of Group VI elementsachieve the electronic arrangements of atoms of noble gases.
*** The End***