Download CD Roms - 香港道教聯合會圓玄學院第一中學

HONG KONG TAOIST ASSOCIATION THE YUEN YUEN INSTITUTE NO.1 SECONDARY SCHOOL
香港道教聯合會圓玄學院第一中學
Scheme of Work For Teaching 教 學 進 度 表 (2006-2007)
Subject
Teacher
科目：
Form 年級：
Chemistry
任教老師：
1.
Mr/Miss/Ms
2.
Class
( 12
)
Mr/Miss/Ms
(
3.
Mr/Miss/Ms
4.
F.6B
Stream(s)
組別
Biology
每循環週節數
：
10
：
26
：
260
a.
No. of periods per cycle
)
b.
No. of teaching cycles in the year
(
)
c.
Total no. of periods available
Mr/Miss/Ms
(
)
d.
5.
Mr/Miss/Ms
(
)
% of time allocated for extensive learning activities in English 全年用
於英文增潤學習的時間百分比
：
50%
6.
Mr/Miss/Ms
(
)
% of lessons incorporated with cooperative learning activities in the year
全年有合作學習活動課節的百分比
：
20%
Text Books
Ho Pui Yan
班別
F.6
e.
全年教學週數
全年教學節數
教科書：
Title
書名
Author
作者
Publisher
出版
1.
New Way Chemistry for Hong Kong A-Level Vol.1 (3rd Edition)
Y.C. Wong & C.T. Wong
Manhattan
2.
New Way Chemistry for Hong Kong A-Level Vol.2 (3rd Edition)
Y.C. Wong & C.T. Wong
Manhattan
3.
Remark
1.
2.
3.
備註：
在學習目標欄目內，註明公民/德育教育或價值/態度教育(堅毅、尊重他人、責任感、國民身分認同和承擔精神)，以﹝CM﹞代表公民/德育教育，﹝VA﹞代表價值/態度教育。
Please use [CM] to denote ‘moral and civic education’ and [VA] to denote ‘value/attitude education’ in the Column of Learning Objective Column.
在活動/實驗/教具欄目內，註明合作學習、透過閱讀進行學習、英文增潤學習（例如教授英文詞彙等），以﹝CO﹞代表合作學習，﹝RL﹞代表透過閱讀進行學習，﹝EL﹞代表英文增潤學習。
Please use [CO] to denote ‘cooperative learning’, [RL] to denote ‘reading to learn’ and [EL] to denote ‘extensive learning activities in English’ in the Column of Activities/Experiment/Teaching Aids.
可採用一項或以上習作評估的方法：(i) 老師批改(分數/等級)；(ii) 學生互評；(iii) 學生自我評估；(iv) 家長評估；(v) 比賽；(vi) 其他。
Please make use of various assessment methods: (i) marking/grading by teacher; (ii) peer assessment; (iii) self-assessment by students; (iv) assessment by parents; (v) competition; (vi)others.
S/E/1
HONG KONG TAOIST ASSOCIATION THE YUEN YUEN INSTITUTE NO.1 SECONDARY SCHOOL
香港道教聯合會圓玄學院第一中學
Scheme Of Work For Teaching 教 學 進 度 表 (2006 - 2007)
日期 單元
Date Unit
4/9/06
︱
11/9/06
Cycle
1
學習目標 (註 1)
Learning Objective
教學內容
Content
Students should be able to

recognize the importance of
laboratory safety, understand
various types of hazard
warning labels and classify
chemical wastes. (CM)
Introduction : Laboratory Safety or
Regulation

laboratory safety and regulations; fire
drill path

hazard warning labels and classification
of chemical wastes.
Atoms, molecules and stiochiometry
1.1
- The atomic structure.
Unit 1
12/9/06
︱
19/9/06
Cycle
2
20/9/06
︱
27/9/06
Cycle
3
1. to recognize that protons,
neutrons and electrons are
constituents of the atom.
2. to balance nuclear reaction
equations.
3. to recognize that the relative
isotopic, atomic and molecular
masses can be determined by
mass spectrometer.
4. to understand the mole concept.
1.2
- Introduce mass spectrometer.
- Deduce isotopic, atomic and molecular
masses from the mass spectrum.
1.3
- The mole concept.
(i)
The mole and the Avogadro
constant.
(ii)
Molar volume of gases.
(iii)
Ideal gas and ideal gas
equation.
(iv)
Dalton’s law of partial
pressures
5. to find empirical and molecular 1.4
formulae.
- calculation of the empirical and molecular
6. to understand the stoichiometric formulae
relationship between reactants
and products.
活動 / 實驗 / 教具 (註 2)
Activities / Experiment / Teaching Aids
多媒體教學
Use of IT
習作及評估方法 (註 3)
Assignment / Evaluation
備註
Remarks
Laboratory safety
http://www.cityu.ed
u.hk/secondary_sch
ool_safety
Class discussion
Assignment (EL)
CD Roms
New Way
Chemistry for H.K.
power presentation
CD Roms
Ex 1
New Way
Evaluation (i)
Chemistry for H.K.
power presentation
Acid –base titration
(EMB)
Class discussion
Experiment 1 (CO)(RL) (EL)
Standardization of Sodium Hydroxide by using
ethanedioic acid-2-water as the primary standard in
volumetric analysis
Assignment (EL)
CD Roms
Mass Spectrometer
(EMB)
New Way
Chemistry for H.K.
power presentation
Experiment 1
Evaluation (i)
Ex 2
Evaluation (i)
YY1 Website
(Chemistry)
教學進度表（2006-2007）
1
28/9/06 Unit 2 1. to state and interpret the
︱
characteristics of atomic H
6/10/06
spectrum by Bohr’s model.
The Electronic Structure of Atoms and the
Periodic Table
2.1
2. to predict electronic structure
- State and explain characteristics of atomic
from ionization enthalpy
emission of H spectrum. By Bohr’s model
Cycle
3. to plot the graphs of successive
and use the concept E=hνto introduce the
4
I.E. for a particular element or 1st idea of discrete energy level.
I.E. against atomic numbers.
2.2
- Prediction of electronic structure from I.E
- Graphical relationship between 1st I.E and
atomic no.
9/10/06 Unit2 4. to understand the meaning of
2.3
︱
atomic orbital.
- Limitation of Bohr’s model.
16/10/06
- Atomic orbitals.
- the designation, shape and the relative
energies of s, p and d orbitals.
Cycle
5
Class discussion
Experiment 2 (CO)(RL) (EL)
Determination of the Concentration of Potassium
Peroxodisulphate(VI)
Test 1 (EL)
CD Roms
Experiment 2
New Way
Evaluation (i)
Chemistry for H.K.
power presentation
Ex 3
YY1 Website
Evaluation (i)
(Chemistry)
Assignment (EL)
Class discussion
Watching Video tape (EL)
ILPAC series : Atomic H emission spectrum
Display atomic orbital models.
CD Roms
Experiment 3
New Way
Evaluation (i)
Chemistry for H.K.
power presentation
YY1 Website
(Chemistry)
Experiment 3 (CO)(RL)
To determine the calcium carbonate in Eggshell
17/10/06
︱
25/10/06
Cycle
6
5. to build up of electronic
configurations using
s, p and d orbitals.
6. to state and interpret the trends
of I.E. and atomic radii of the
elements in the Periodic Table.
2.4
- Building up of electronic configurations by s,
p and d orbitals based on three principles
2.5
- Interpretation of I.E. and atomic radii of the
elements in the Periodic Table.
Class discussion
Experiment 4 (CO)(RL) (EL)
Analysis of aspirin tablets.
Test 2 (EL)
CD Roms

New Way
Chemistry for
H.K. power
presentation

G.C.E. AL.
chemistry
Experiment 4
Evaluation (i)
Ex 4
Evaluation (i)
Assignment (EL)
26/10/06 Unit 3 1. to understand the meaning of
︱
energetics.
3/11/06
2. relate the enthalpy changes to
Cycle
7
bond breaking and formation.
3. to understand some standard
enthalpy changes.
4. to determine the enthalpy
changes by calorimetric
experiment.
Energetics
3.1
- Energy changes in chemical reactions.
3.2
- Introduce some standard enthalpy changes
(includes formation, combustion,
neutralization, solution)
- Experiment determination of enthalpy
changes
Class discussion
CD Roms
Experiment 5
New Way
Evaluation (i)
Experiment 5 (CO)(RL) (EL)
Chemistry for H.K.
A. To standardize sodium thiosulphate by sodium power presentation
iodate(V).
B. To investigate the amount of ascorbic acid in a
commercial vitamin C tablet.
教學進度表（2006-2007）
2
6/11/06
︱
13/11/06
Cycle
8
5. state and understand Hess’s law. 3.3
6. calculate the enthalpy changes of - Introduce Hess’s law
reactions.
- Use Hess’s law to determine the enthalpy
7. understand spontaneity of
change of reactions which cannot be
changes and relationship
determined directly
ΔG = ΔH - TΔS
3.4
- Introduce and explain the concept of entropy
changeΔS and free energy changeΔG
- The relationship betweenΔG andΔS :
ΔG = ΔH - TΔS
14/11/06 Unit 4
︱
Students should be able to
21/11/06
1. define ionic bond
Cycle
9
2. to define metallic bond
3. to understand various
kinds of metallic crystals
Bonding and structure
4.1
- Different types of bonding
4.2
- Explain the term of metallic bond.
- Metallic structures.(close-packed and open
structures)
Class discussion
Experiment 6 (CO)(RL) (EL)
Qualitative analysis (Test of Cation)
CD Roms
Experiment 6
New Way
Evaluation (i)
Chemistry for H.K.
power presentation Ex 5
Evaluation (i)
Test 3 (EL)
Assignment (EL)
Class discussion
Experiment 7 (CO)(RL) (EL)
Qualitative analysis (Test of Anion)
CD Roms
Experiment 7
New Way
Evaluation (i)
Chemistry for H.K.
power presentation
YY1 Website
(Chemistry)
- Alloys : Properties of alloys and their uses
22/11/06
︱
30/11/06
Cycle
10
4. to define ionic bond
5. to construct the Born- Haber
cycles for the formation of ionic
compounds in terms of some
enthalpy changes
4.3
- Formation of ions and ionic bond.
- Energetics of formation of ionic
compounds and hence introduce
Born-Haber cycle.
- Compare the size of ions with
4.4
- Formation of covalent bond.
Class discussion
4.5
Class discussion
- Bonding intermediate between ionic and
covalent.
- incomplete transfer in ionic compounds.
- polarity of covalent bond.
Experiment 9 (CO)(RL) (EL)
Build up models : molecules (CO)
Experiment 8 (CO)(RL) (EL)
Qualitative analysis (Test of Unknown)
Test 4 (EL)
- Bond enthalpies, bond length and covalent radii.
- Formation of  and  bonds in multiple bond. Assignment (EL)
1/12/06
︱
8/12/06
Cycle
11
6. to define covalent bond and
dative covalent bond.
7. to recognize that multiple bond
contains  and  bonds.
8. draw dot and cross diagrams for
simple molecules; the shapes of
molecules and polyatomic ions.
9. recognize that multiple bond
contains  and  bonds.
To determine the heat of hydration of magnesium
sulphate indirectly by application of Hess’s Law..
Display models : hcp, ccp and bcp.
CD Roms
Ex 6
New Way
Evaluation (i)
Chemistry for H.K.
power presentation
Experiment 8
Evaluation (i)
YY1 Website
(Chemistry)
CD Roms
Experiment 9
New Way
Evaluation (i)
Chemistry for H.K.
power presentation Ex 7
Evaluation (i)
YY1 Website
(Chemistry)
Assignment (EL)
教學進度表（2006-2007）
3
11/12/06
︱
18/12/06
4.6
10. to define and understand
various of intermolecular forces - Intermolecular forces
(i) dipole-dipole interactions
(ii) van der Waals’ force.
(iii) H-bond and importance of H-bonds in ice
and DNA.
Cycle
12
19/12/06
︱
3/1/07
Cycle
13
4/1/07
︱
11/1/07
Cycle
14
Class discussion
- Molecular structures.
- Exemplied by I2, CO2 and buckminsterfullerence
C60.
- Introduce the P-T diagram and explain the
properties of ice and dry ice with the aid of P-T
diagram
11. to acknowledge the relationship 4.7
- Difference in physical properties between
between structures and
properties of materials
(VA)
ionic solids, giant covalent network
substances, molecular solids and metal
solids.
CD Roms
Experiment 10

New
Way Evaluation (i)
Display models : NaCl, CsCl, diamond, graphite and quartz
Chemistry for
H.K. power
Experiment 10 (CO)(RL)(EL)
presentation.
To determine the enthalpy of formation of calcium

Chemistry Set
carbonate indirectly by application of Hess’s Law.
2000
Class discussion
CD Roms

New Way
Chemistry for
H.K. power
presentation

Chemistry Set
2000
Revision
and
Mid-year Examination
12/1/07
︱
22/1/07
Mid-year Examination
Cycle
15
教學進度表（2006-2007）
4
23/1/07 Unit1.5 1. to explain the meaning of
︱
reaction rate.
30/1/07
2. to describe the various kinds of
Cycle
16
31/1/07
︱
7/2/07
Cycle
17
8/2/07
︱
26/2/07
Cycle
18
27/2/07
︱
6/3/07
method to follow the reaction
rate.
3. to describe and understand
factors affecting reaction rate.
Chemical kinetics
5.1
- Definition of reaction rate.
- Method to follow the reaction rate.
5.2
- Effects of concentration, temperature,
pressure, surface area, catalyst and light on
reaction rate
4. to understand and deduce rate
equation from experimental
results.
5. to explain the terms: order of
reaction, rate constant and
half-order.
6. to explain the effect of
temperature on reaction rate.
7. to calculate the activation energy
by Arrhenius equation.
5.3
- determined from experimental results.
- rate constant and half-life.
8. to interpret rates of gaseous
reactions at molecular level.
9. draw energy profiles for a
multi-steps reaction and
determine the rate determining
step from the energy diagram.
5.5
- Distribution of molecular speeds in a gas.
- Graphical representation of the
Maxwell-Boltzmann distribution and its
variation with temperature
- Energy profile for multi-step reactions
- Determination of the rate determining step
from the energy diagram.
Class discussion
Experiment 11 (CO)(RL)(EL)
CD Roms
Gateway
controlling
reactions
Experiment 11
Evaluation (i)
To investigate the existence and strength of hydrogen
New Way
bonding.
Chemistry for H.K.
power presentation
Class discussion
Experiment 12 (CO)(RL)(EL)
Acidity of CuSO4 solution and solubility product of
copper(II) hydroxide
5.4
- explain the effect of temperature on reaction
rate.
Assignment (EL)
- calculate the activation energy by Arrhenius
equation
Class discussion
YY1 Website
(Chemistry)
YY1 Website
(Chemistry)
Experiment 12
Evaluation (i)
New Way
Ex 8
Chemistry for H.K. Evaluation (i)
power presentation
YY1 Website
(Chemistry)
Experiment 13
Evaluation (i)
Experiment 13 (CO)(RL) (EL)
To determine the order of reaction between iodine and
propanone
New Way
Chemistry for H.K.
power presentation
Test 5 (EL)
10. to explain the effect of catalyse 5.6
Class discussion
on reaction rate.
- explain the effect of catalyst on reaction rate.
11. to describe the use of catalyst in - homogeneous and heterogeneous catalyst.
our daily life. (VA)
- Application of catalyst on our daily life.
Experiment 14 (CO)(RL) (EL)
To determine the activation energy of the reaction
Cycle
between bromide and bromate(V) in acidic medium.
19
Chemical Equilibrium
Unit 6
Assignment (EL)
1. recognize that equilibrium is
6.1
dynamic.
- definition and characteristics of dynamic
2. describe the characteristics of
equilibrium.
equilibrium
CD Roms

Gateway
understanding
chemical
equilibrium
Experiment 14
Evaluation (i)
Ex 9
Evaluation (i)
教學進度表（2006-2007）
5
7/3/07
︱
14/3/07
3.
4.
Cycle
20
15/3/07
︱
22/3/07
Cycle
21
23/3/07
︱
30/3/07
Cycle
22
write the equilibrium equation
and calculate equilibrium
constant.
explain the effect changes in
concentration, pressure and
temperature on equilibria by
Le Chatelier’s principle.
- definition of equilibrium law and equilibrium
constant.
- calculation of equilibrium constant.
- Introduce Le Chatelier’s principle.
- The effect of changes in concentration,
pressure and temperature on equilibrium.
Class discussion
Experiment 15 (CO)(RL) (EL)
Determination of the equilibrium constant of
esterification between ethanoic acid and propan-1-ol.
CD Roms
Experiment 15
New Way
Evaluation (i)
Chemistry for H.K.
power presentation
Test 6 (EL)
5. to define acid and base
6. to explain the meaning of ionic
product of water.
7. to define pH value and describe
the method to measure pH value.
8. to define dissociation constant
and use the dissociation constant
to compare the acid strength.
9. to calculate the dissociation
constant of weak acid.
6.2
- Definition of acid and base.
- Dissociation of water and definition of ionic
product of water.
- Definition of pH value
- Methods of measuring pH value
- Calculation of pH value
- Definition, use and calculation of
dissociation of weak acid and weak base.
Class discussion
CD Roms
Experiment 16
New Way
Evaluation (i)
Experiment 16 (CO)(RL) (EL)
Chemistry for H.K.
Ionization Constants of an Indicator and Weak Acids. power presentation
10.to define and prepare buffer
solution.
11.to calculate the pH value of a
buffer solution.
12.to state the types of indicator
and describe the effect of the pH
value on the color of indicator.
- Definition and preparation of buffer solution. Class discussion
- Calculation of pH value of a buffer solution.
Test 7 (EL)
- Definition of indicator.
- Choice of indicator on acid-base titration.
- Effect of pH value on the color of indicator.
- pH titration curve.
Assignment (EL)
Ex 10
Evaluation (i)
CD Roms
New Way
Chemistry for H.K.
power presentation
教學進度表（2006-2007）
6
16/4/07
︱
23/4/07
Cycle
23
24/4/07
︱
2/5/07
Cycle
24
3/5/07 Unit
11
︱
10/5/07
Cycle
25
13. define solubility product Ksp
14. calculate Ksp from solubility and
vice versa.
15. explain the equilibrium shift by
common effect.
16.to define oxidation and
reduction.
17. to balance redox reaction
18. to define standard H
electrode and electrode potential
of a half-cell.
19. to calculate the e.m.f of a
chemical cell formed by two
half-cells.
20. to write ca cell diagram
solubility product of a sparingly soluble
electrolyte
Class discussion
6.3
- Definition of oxidation and reduction in
terms of electron transfer and oxidation
number.
- Balancing redox reactions.
- Emf measurement of electrochemical cells
- Standard H electrode and measurement of e Class discussion
21. to predict the feasibility of
electrode potential of a M/Mx+.system.
redox reactions from the
- Calculation of e.m.f. / electrode potential of a Assignment (EL)
electrode potentials.
chemical cell formed by two half-cells.
22. to understand how lead- Construction of cell diagrams using IUPAC
acid cell and fuel-cell generate
convention.
current (CM)
- Nernst equation
- Prediction of feasibility of cell redox
reactions.
- Lead-acid cell and fuel cell.
Class discussion
1. to explain the shape and the
11.1
bonding of the hydrocarbons
- Explain the tetrahedral arrangement,
2. to identify the functional groups formation of the double/triple bond of the
and homologous series
hydrocarbons in terms of electron repulsion
3. to explain the shape and the
and hybridized orbitals
Test 8 (EL)
bonding of the hydrocarbons
- Explain the delocalization of -electrons in
benzene
11.2
- Study of the functional groups
- Effects of functional groups and the length of
carbon chains on physical properties
CD Roms made by
EMB

To draw pH
titration
curves of
various kinds
of acid-base
titration
CD Roms
New Way
Ex 11
Chemistry for H.K. Evaluation (i)
power presentation
CD Roms
New Way
Chemistry for H.K.
power presentation
教學進度表（2006-2007）
7
11/5/07
︱
18/5/07
4. to study the systematic
nonmenclature
11.3
- Systematic nonmenclature
Class discussion
revision
Class discussion
Assignment (EL)
Cycle
26
21/5/07
︱
29/5/07
CD Roms
New Way
Chemistry for H.K.
power presentation
Cycle
27
30/5/07
︱
6/6/07
Ex 12
CD Roms
Evaluation (i)
New Way
Chemistry for H.K.
power presentation
Final Examination
Cycle
28
教學進度表（2006-2007）
8