June 2015
The Hong Kong Polytechnic University
Hong Kong Community College
Subject Description Form
Subject Code
CCN1110
Subject Title
General Chemistry I
Level
1
Credit Value
3
Medium of
Instruction
English
Pre-requisite /
Co-requisite/
Exclusion
Nil
Objectives
This subject introduces a molecular perspective for understanding the
natural world and helps students to identify the fundamental concepts on
physical and chemical changes of matters. Throughout the course,
students will visualise the physical and chemical changes through the
understanding of molecular behaviour. Studying this subject also helps
develop students’ analytical thinking for their lifelong learning.
Intended Learning
Outcomes
Upon completion of the subject, students will be able to:
(a) understand the macroscopic properties of the states of matters.
(b) understand the basic principles of chemical energetics and
equilibria.
(c) apply and incorporate the chemical principles and knowledge
learned to solve chemical problems and to appreciate modern
applications in real life.
(d) demonstrate the abilities in communication skills in problemsolving and analytical thinking.
Subject Synopsis/
Indicative Syllabus
Measurement in Chemistry
Significant figures; SI units; Substances and mixtures; Solution and
concentration; Mole and Avogadro’s number; Chemical reactions and
balanced equations; Temperature scales.
Thermochemistry
Heat and work; The First Law of Thermodynamics; Heat of Reactions
(ΔU and ΔH); Hess’s law.
Chemical Kinetics
Reaction rates and measurements; The rate law and rate constant;
Molecularity and mechanism of a reaction; Collision theory; Activated
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June 2015
complexes; Transition state theory; Chain reaction; Catalysis; Enzymatic
reactions.
Physical Properties of Solutions
Solution concentration; Intermolecular forces and the solution process;
Solubilities of gases; Vapor pressures of solutions; Osmotic pressure;
Freezing point depression and boiling point elevation; Solutions of
electrolytes; Colloidal properties.
Principle of Chemical Equilibria
Law of chemical equilibrium and equilibrium constant; Le Chatelier’s
Principle.
Acid-base Equilibria in Aqueous Solutions
Ionisation of water; pH, pOH and pKw; Acids and bases; Polyprotic
acids; Buffers; Solubility equilibria.
Solubility and Complex-Ion Equilibria
Solubility constants and solubility; common ion effects; precipitation;
equilibria involving complex ions.
Structures and Reactions of Organic Compounds
Isomerisms; Functional groups of organic compounds; Nucleophilic
substitution reactions; Elimination reactions; Addition reactions of
alkenes; Electrophilic aromatic substitution; Reactions of alkanes;
Polymers and polymerization reactions.
Teaching/Learning
Methodology
Lectures will provide theory-based teaching on physical and organic
chemistry. Examples and references will be given to students whenever
appropriate. Tutorials will provide students with opportunities to
broaden, enlighten and reinforce the general knowledge obtained in the
lectures. Students will be involved in problem-based activities,
classroom feedback, and discussions in the tutorials. Laboratory
sessions will allow students to understand, verify, and apply knowledge
developed from the lectures.
Assessment Methods
in Alignment with
Intended Learning
Outcomes
A variety of assessment tools will be used to develop and assess
students’ achievement of the subject intended learning outcomes.
Specific assessment
methods/tasks
%
Intended subject learning
weighting outcomes to be assessed
a
b
c
Continuous Assessment*
50
 Test
25



 Assignment 1
12.5



 Group Assignment
12.5




Final Examination
50
Total
100
2

d

June 2015
*Continuous assessment items and/or weighting may be adjusted by the subject
team subject to the approval of the College Programme Committee.
To pass this subject, students are required to obtain Grade D or above in
both the Continuous Assessment and Final Examination.
Student Study
Effort Expected
Class contact
Hours

Lecture
26

Tutorial
13

Laboratory
3
Other student study effort

Self-study
52

Continuous Assessment
36
Total student study effort
Reading List and
References
130
Recommended Textbook
Petrucci, R.H., Herring, F.G., Madura, J.D. & Bissonnette, C. (2011).
General chemistry: Principle and modern applications. (10thed.),
Pearson.
References
Brady, J.E. (2009). Chemistry: Matter and its changes. (5th ed.), Wiley.
Bauer, R. C. (2009). A conceptual introduction to chemistry. (2nd ed.),
McGraw-Hill.
Chang, R. (2011). General chemistry: The essential concepts. (6th ed.),
McGraw-Hill.
Malone, L.J. & Dolter, T.O. (2010). Basic concepts of chemistry.
(8th ed.), Wiley.
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