Nam Wah Catholic Secondary School_Learning Manual

Subject：Chemistry Class/Form：S6S Year:2010-11 Teacher’s Name：Wong Mei TinName of Panel Head:Wong Mei Tin

Daily grade/Exam marks Ratio：30/70 ★Extended

Cycles /

Main Teaching Points

/ Daily Grade (1+2+3 = 30% of total subject marks)
1. Class Performance
(5 marks) / 2. Homework
(5 marks) / 3. Test s
(20marks) / 4. Exam Marks
(70%)
1 / Lab. safety and experimental techniques
Ch.1 Atoms, Molecules and Stoichiometry
1.1The atomic structure
Relative isotopic, atomic and molecular masses
1.2The mole concepts: The mole and Avogadro Constant.
1.3 Molar Volume of gases. Ideal gas equation and its application to relative molecular mass determination, Partial Pressure of gases. / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Report
  2. Exercise.
/ First
Term
Exam
2-3 / 1.4 Empirical and Molecular formulae
1.5 Chemical equations and stoichiometry
Ch.2 The Electronic structure of Atoms and The Periodic Table.
2.1 Atomic emission spectra and electronic structure
2.2 Electronic structure, ionization enthalpies
2.3 Atomic orbital.
2.4 Electronic Configuration / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Report
  2. Exercise
/ 1 time
Cycles /

Main Teaching Points

/ 1. Class Performance
(5 marks) / 2. Homework
(5 marks) / 3. Test s
(20 marks) / 4. Exam Marks
(70%)
4-5 / 2.5 The Periodic Table and The properties of elements
Ch.3 Energetic
3.1 Energy changes in chemical reactions
3.2 Standard enthalpy changes
3.3 Hess’s Law
Enthalpy level diagram. Calculations
3.4 Spontaneity of changes
△G=△H-T△S / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Report
  2. Exercise
  3. Essay
/ 1 time / First
Term
Exam
6 / Ch.4 Bonding and structure
4.1 The nature of forces holding atoms together
4.2 Metallic bonding, metallic crystals, alloys
4.3 Ionic bonding, Energetic of formation of ionic compounds
Stoichiometry of ionic compounds, ionic crystals ionic radii. / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Report
  2. Exercise
  3. Essay
/ 1 time
Total Marks：1+2+3+4=
Cycles /

Main Teaching Points

/ 1. Class Performance
(5 marks) / 2. Homework
(5 marks) / 3. Test s
(20 marks) / 4. Exam Marks
(70%)
7 / Revision
(10/12-18/12)1st Term Exam
Discuss Exam Paper
4.4 Covalent bonding, Dative bond, bond enthalpies, bond length covalent radii. Shapes of molecules and poly-atomic ions, covalent crystals / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Report
  2. Exercise
  3. Essay

8 / 4.5 Bonding Intermediate between ionic and covalent
Incomplete e–transfer in ionic compounds, polarity of covalent bond.
4.6 Intermolecular forces, H – bonding, Van der Waals’ forces.
4.7 The relationship between structures and properties of substances
Ch. 5 Chemical Kinetics.
5.1 Rate of Rx.
Measurement of chemical Rx. rate, following a Rx. by chemical and physical methods. / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ /
  1. Report
  2. Exercise
3. Essay / 1 time
9 / 5.2 Factors influencing reaction rates (conc., temp., pressure , surface area, catalyst and light.) / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Report
  2. Exercise
  3. Book Report
/ Second
Term
Exam
4. Exam Marks
(70%)
Cycles /

Main Teaching Points

/ 1. Class Performance
(5 marks) / 2. Homework
(5 marks) / 3. Test s
(20marks)
10 / (11/2-20/2)Chinese New Year Holidays
5.3 Rate equation and order of reactions.
5.4 Arrhenius equation
5.5 Interpretation of rates of gaseous reactions at molecular level
5.6 Catalysis
Ch.6 Chemical equilibrium
6.1 Dynamic equilibrium: The equilibrium law, partition coefficient. Effect of changes in concentrations, pressure and temperature on equilibrium / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
1. Report
2Exercise
3.Essay / 1 time / Second
Term
Exam
11 / 6.2 Ionic equilibrium . Concept of acid/ base, Dissociation of water. pH and its measurement. Strong and weak acids/bases
(18/3-29/3) Easter Holidays
Buffer/★. Acid- base titration and the choice of indicator. Solubility product / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
1. Report
2. Exercise.
12 / 6.3 Redox equilibria.
Electrochemical cells. Electrode potential, The Nernst equation
Secondary cells and fuel cells
(30/3-10/4)Easter Holidays / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
1. Report
2. Exercise
3.Proposal
of Project
  1. Essay
/ 1 time
Cycles /

Main Teaching Points

/ 1. Class Performance
(5 marks) / 2. Homework
(5 marks) / 3. Test s
(20marks) / 4. Exam Marks
(70%)
13 / Ch.7 Periodic properties of the elements in the periodic Table.
7.1 Periodic Variation in physical properties of elements: H to Ar / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
1. Report
2.Poster Design / Second
Term
Exam
14 / 7.2 Periodic relationship among oxides of the elements Li to Cl / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Exercise
/ 1 time
15 / 8.1 Characteristic properties of s-block elements
8.2 Variation in properties of the s-block elements / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Report
2. Exercise / 1 time
16 / Ch.13 Chemistry in action: Drugs and
Green Chemistry
Revision
Second Term Exam(11/6-22/6) / O(5) □
Act(4-3) □
F(2) □
Sub(1-0) □ / Types of HW
  1. Project Presentation (after the Second Term Exam)

Total Marks：1+2+3+4 =

Remarks: #O: Outstanding Act: Active F: Fair Sub: Substandard