Kit Sam Lam Bing Yim Secondary School

Subject head：Heung Hau Ling

______________________

Written by：Heung Hau Ling

Remarks：

8. "Law-abidingness" , 9. "Empathy" and 10. "Diligence” (11. “Unity” 12. ‘Filial Piety’)

D. The Constitution, the Basic Law and the National Security Education code : #

Unit 23 Shapes of molecules
23.1 The octet rule
23.2 Molecules not obeying the octet rule
23.3 Shapes of simple molecules containing only single covalent bonds
23.4 Shapes of simple molecules containing multiple covalent bonds
23.5 Relationship between the number of electron pairs in the outermost shells of central atoms and shapes of simple molecules

- Explain the polar nature of molecules (such as HF, H2O, NH3 and CHCl3) and the non-polar nature of molecules (such as CH4 and BF3) with reference to electronegativity, polarity of bonds and molecular shape.

Unit 24 Bond polarity and intermolecular forces
24.1 Sharing of bonding electrons in a covalent bond
24.2 Electronegativity and the Periodic Table
24.3 Covalent bond between two different atoms
24.4 Polarity of molecules
24.5 Testing whether or not a liquid is polar
24.6 Forces of attraction between non-polar molecules
24.7 Forces of attraction between polar molecules
24.8 Factors affecting the strength of van der Waals’ forces

- state the factors affecting the strength of van der Waals’ forces between molecules
- compare the strength of van der Waals’ forces with that of hydrogen bonding
- understand the effect of hydrogen bonding on properties of substances such as water and ethanol

Chapter 25 Fossil fuels #
25.1 Different sources of energy in Hong Kong
25.2 Fossil fuels
25.3 Hydrocarbon
25.4 Why is petroleum important?
25.5 Fractional distillation of petroleum
25.6 Trends in properties of fractions from petroleum
25.7 Uses of fractions from petroleum
25.8 Combustion of fuels
25.9 What is the greenhouse effect?
25.10 Increasing the greenhouse effect of
the atmosphere
25.11 Polluting the atmosphere
25. 12 Air pollution in Hong Kong

– Understand the importance of fossil fuel
– Describe fractional distillation of petroleum and understand the concepts
- Understand the problems by using fossil fuels

- evaluate the impact of using fossil fuels on our quality of life and the environment
-

Unit 36 An introduction to rate of reaction
36.1 Rate of reaction
36.2 Measuring the rate of reaction
36.3 Methods for following the progress of a reaction
36.4 Following the progress of a reaction by measuring the change in volume of a gaseous product
36.5 Following the progress of a reaction by measuring the change in mass of the reaction mixture
36.6 Following the progress of a reaction by measuring the change in pressure
36.7 Following the progress of a reaction by measuring the change in colour intensity
36.8 Studying the reaction
between sodium
thiosulphate solution
and dilute hydrochloric
acid
36.9 Following the progress of a reaction by titrimetric analysis

- recognize that initial rate is equal to instantaneous rate at time t = 0

- determine instantaneous rate and average rate from a suitable graph (e.g. concentration-time graph)
- carry out experiment to follow the progress of reaction between sodium
thiosulphate solution and dilute hydrochloric
- acid,

Chapter 37 Factors affecting rate of reaction
37.1 Changing the rate of a reaction
37.6 Factors affecting the rate of a reaction
37.2 Effect of change in concentration of a reactant on the rate of a reaction
37.3 Effect of change in surface area of a solid reactant on the rate of a reaction.
37.4 Effect of change in temperature on the rate of a reaction
37.5 Effect of using a catalyst on the rate of a reaction
37.11 Catalysts in industry
37.12 Enzymes

- explain qualitatively the effect of changes in concentration, surface area and temperature on the rate of reaction.

- perform experiments to study the effects of different factors on rate of reaction

Unit 38 Gas volume calculations
38.1 Reacting volumes of gases
38.2 Molar volume of a gas
38.3 Calculations involving
gases and solids or solutions
38.4 Calculations using
reacting volumes of gases

- understand what molar volume is.

- perform stoichiometric calculations involving molar volume of gases at r.t.p.

Unit 34 Energy changes in chemical reactions
34.1 What is energy?
34.2 Heat capacity and specific heat capacity
34.3 Conservation of energy
34.4 Enthalpy changes
34.5 Exothermic and endothermic reactions
34.6 Enthalpy level diagrams
34.7 Energy changes and bonding
34.8 Thermochemical equations
34.9 Standard enthalpy changes
34.10 Standard enthalpy change of reaction

- explain the nature of exothermic and endothermic reactions in terms of breaking and forming of chemical bonds.
- explain and use the terms: enthalpy change of reaction and standard conditions, with particular
- reference to combustion

- draw diagrams to explain the nature of exothermic and endothermic reactions in terms of enthalphy change
- calculate enthalpy changes from experimental results, including the use of the relationship:ΔH = mcΔT.
- Carry out experiment to determine the enthalpy change of neutralization

34.11 Standard enthalpy change of formation
34.12 Standard enthalpy change of combustion
34.13 Standard enthalpy change of neutralisation
34.14 Determining an enthalpy change of combustion, ΔHc
34.15 Determining enthalpy changes of reactions

Unit 35 Hess’s law and its applications
35.1 Hess’s law
35.2 Determining the enthalpy change of formation of calcium carbonate
35.3 Enthalpy change of formation from enthalpy changes of combustion
35.4 Enthalpy change of reaction from enthalpy changes of formation

- apply Hess’s Law to construct simple enthalpy change cycles.

- perform calculations involving enthalpy change cycles and relevant energy terms

Unit 18 Chemical cells in daily life
18.1 Chemical cells and you
18.2 Types of chemical cell
18.3 Zinc-carbon cell
18.4 Alkaline manganese cell
18.5 Silver oxide cell
18.6 Lead-acid accumulator
18.7 Nickel metal hydride (NiMH) cell
18.8 Lithium ion cell
18.9 Choosing a chemical cell for a particular purpose
18.10 Environmental
impacts of using chemical cells

- describe the characteristics of common primary and secondary cells

- justify uses of different chemical cells for particular purposes

Unit 19 Simple chemical cells
19.1 Building a simple chemical cell
19.2 Building a chemical cell from two half cells
19.3 The Daniel cell
19.4 Comparing the tendencies of metals to form ions
19.5 The electrochemical series of metals

- describe how a chemical cell work to produce electricity

- write equations involved in simple chemical cells.

Unit 20 Oxidation and reduction in chemical cells
20.1 Oxidation and reduction in terms of gain and loss of oxygen
20.2 Oxidation and reduction in terms of loss and gain of hydrogen
20.3 Oxidation and reduction in terms of loss and gain of electrons
20.4 Oxidation numbers
20.5 Oxidation and reduction in terms of changes in oxidation numbers
20.6 Using oxidation numbers to identify redox reactions

20.7 Naming inorganic compounds
20.8 Half equations of oxidation and reduction
20.9 Common oxidising agents
20.10 Common reducing agents
20.11 Balancing redox
equations by using half equations
20.12 Balancing redox
equations by using changes in oxidation numbers
20.13 Deducing half
equations from the overall redox equation

20.14 How are the relative oxidising and reducing power of chemical species related to their positions in the electrochemical series?
20.15 Chlorine as an
oxidising agent
20.16 Hydrogen halides as reducing agents
20.17 Aqueous sulphur
dioxide as a reducing agent


Unit 21 Oxidation and reduction in chemical cells
21.1 Chemical cells with inert electrodes
21.2 Hydrogen-oxygen fuel cell

- identify oxidation and reduction in a simple chemical cell.

- write half equations for reactions occurring at each half cell and overall ionic equation for the chemical cell

Unit 22 Electrolysis
22.1 What is electrolysis?
22.2 Electrolysis of molten zinc chloride
22.3 Comparing a chemical cell and an electrolytic cell
22.4 Electrolysis of aqueous solutions
22.5 Position of ions in the electrochemical series and the preferential discharge of ions

22.6 Concentration of ions in solution and
preferential discharge of ions
22.7 The nature of
electrodes and the preferential discharge of ions
22.8 Electroplating
22.9 Environmental impact of the electroplating industry

Chapter 26
Homologous series, structural formulae and naming of carbon compounds
26.1 Chemistry of carbon compounds
26.2 Formulae of carbon compounds
26.3 Functional groups and homologous
series
26.4 Homologous series of alkanes
26.5 Naming alkanes
26.6 Writing structural formulae from systematic names
26.7 Naming alkenes
26.8 Naming alkanols
26.9 Naming alkanoic acids

– show a gradation in physical properties and similarity in chemical properties

- write structural formulae of alkanes
- give systematic names of alkanes

Unit 30 Isomerism
30.1 Isomerism
30.2 Structural isomerism
30.3 Cis-trans isomerism
30.4 Enantiomers
30.5 Properties of enantiomers

- recognise the existence of cis-trans isomerism in acyclic carbon compounds resulting from restricted rotation about a C=C bond
- show an understanding of structural and geometrical isomerism by predicting structures of the isomers of some given carbon compounds
- recognise the existence of enantiomerism in compounds with only one chiral carbon

Use structural formulae and molecular models to demonstrate the arrangement of atoms in isomers of carbon compounds

Chapter 27
Alkanes and alkenes
27.1 Important reactions of alkanes
27.2 Demand and supply of petroleum
fractions
27.3 Alkenes
27.4 Physical properties of alkenes
27.5 Important reactions of alkenes
27.6 Renewable energy sources in Hong Kong

- describe the reactions of alkanes and alkenes
- explain the importance of cracking in the petroleum industry

- carry out chemical tests for unsaturated hydrocarbons

Chapter 28 Addition polymers
28.1 Synthetic polymers all around you
28.2 Why are synthetic polymers so useful?
28.3 Addition polymerisation of ethene
28.4 Making other synthetic polymers
28.5 Uses of some common addition
polymers

- Describe addition polymerization using chemical equation
- Describe the structure, properties and uses of some addition polymers.

- Writing chemical equations for the formation of addition polymers based on given
- information.

Unit 29 Naming and physical properties of carbon compounds
29.1 Functional groups and homologous series
29.2 Naming carbon compounds with functional groups
29.3 Trends in physical properties within a homologous series
29.4 Haloalkanes
29.5 Alcohols
29.6 Aldehydes and ketones
29.7 Carboxylic acids
29.8 Esters
29.9 Amides
29.10 Amines
29.11 Common names of carbon compounds

- Give systematic names, formula for organic compounds
- Understand the effects of functional groups and the length of carbon chains on physical properties of carbon compounds

- Draw the structures of the compounds based on their systematic names

Unit 31 Typical reactions of selected functional groups
Unit 29 Naming and physical properties of carbon compounds
Making new carbon compounds
31.1 Making new carbon compounds
31.2 Reaction of alkanes with halogens
31.3 Addition reactions of alkenes
31.4 Substitution reactions of haloalkanes
31.5 Reactions of alcohols

- Describe the reactions and write the chemical equations

- Suggest routes to convert one functional group into another by using the organic reactions.
- state the reagents and conditions to accomplish conversions of carbon compounds using the reactions

- Predict and name the products of the above reactions



- carry out laboratory preparations and purification of simple carbon compounds such as and ester
- calculate the percentage yield of a product obtained from a reaction

Unit 33 Important organic substances
33.1 Aspirin
33.2 Soaps
33.3 Structure of a soap molecule
33.4 Wetting and
emulsifying properties of soap
33.5 The cleansing action of soap
33.6 Soapless detergents
33.7 Polyesters
33.8 Polyamides

- identify the functional groups of the acetylsalicylic acid molecule
- describe the structures of soaps and soapless detergents
- explain the wetting and emulsifying properties of detergents in relation to their structures
- describe the structures and properties of nylon and polyesters

- write equations for the formation of nylon and polyesters

Unit 39 An introduction to chemical equilibrium
39.1 Irreversible and reversible reactions
39.2 The road to equilibrium
39.3 Equilibrium requires a closed system
39.4 Equilibrium attained from either direction of a reaction
39.5 Changing the
conditions of a chemical equilibrium system
39.6 Characteristics of a chemical equilibrium system

- describe characteristic of s system existing in dynamic equilibrium


- express the mathematical relationship between concentrations of reactants and products at
equilibrium and equilibrium constant, Kc

- write equations of irreversible and reversible reactions

- perform calculations related to equation stoichiometry and Kc by either finding Kc from equilibrium concentrations or vice versa

- recognize the fact that the majority of reactions employed in chemical industries are reversible.


- recognize the fact that the majority of reactions employed in chemical industries are reversible

Unit 40 Factors affecting chemical equilibrium systems
40.1 Position of equilibrium
40.2 Shifting the position of equilibrium by changing conditions
40.3 Le Chatelier’s principle
40.4 Effect of concentration changes on chemical equilibrium systems
40.5 The link between Le Chatelier’s principle and the reaction quotient, Qc
40.6 Effect of pressure changes on chemical equilibrium systems
40.7 Effect of temperature changes on chemical equilibrium systems
40.8 Effect of catalysts on chemical equilibrium systems
40.9 Chemical equilibrium systems in industry

- Deduce the effect of change in pressure and temperature on the position of chemical equilibrium.

- Predict the shift in equilibrium position using Le Chatelier’s Principles

Unit 41 Periodic trends in elements and their compounds
41.1 Development of the periodic table
41.2 Categories of elements in the modern periodic table
41.3 Periodic variations in the type of structure and bonding of elements across periods 2 and 3
41.4 Variation in atomic radius of elements across a period
41.5 Trend in melting points of Period 3 elements
41.6 Variation in electrical conductivities of Period 3 elements

- describe the periodic variations of melting point and electrical conductivity of the elements

- interpret the variations in melting point and in electrical conductivity in terms of the bonding and structure of the elements

41.7 Reactions of Period 3 elements with oxygen
41.8 Properties of oxides of Period 3 elements
41.9 Composition of the oxides of Period 3 elements
41.10 Effect of water on oxides of Period 3 elements

Unit 42 The transition metals
42.1 Introduction to transition metals
42.2 Coloured compounds of transition metals
42.3 Variable oxidation states of transition metals

- describe the variation in behaviour of the following oxides in water: Na2O, MgO, Al2O3, SiO2, P4O10, SO2 and Cl2O.

- write down the equation of different oxides with water.

42.4 Variable oxidation states of vanadium
42.5 Variable oxidation states of chromium
42.6 Variable oxidation states of manganese
42.7 Variable oxidation states of iron
42.8 Transition metals and their compounds as catalysts
42.9 Uses of transition metals in medicine

- describe the general properties of transition metals

- deduce the oxidation number of the atom in a compound or ion.