Course Syllabus
Introduction
1.1 Environmental problems (water pollution, air pollution, heavy metals)
1.2 Acid rain cycle, bleaching, a natural buffer
Structure of atom
2.1 Subatomic particles (atomic number, atomic mass, isotopes, atomic symbols, ions)
2.2 Quantum numbers
2.3 Electronic configurations (in terms of subshell and orbital diagram, including first transition elements)
Periodic Table
3.1 Periods, groups and blocks, relationship between electronic configuration and periodic table
3.2 Classifications of element
(metal, non metal, metaloid, transition elements)
3.3 Periodic trends
(atomic size, ionization energy, electron affinity, electronegativity)
Chemical Formula & Calculation
4.1 Molecules and compounds (identify, naming, formula)
4.2 Mole concepts (mass to mole conversion and Avogadro's number)
4.3 Empirical and molecular formula
4.4 Balancing non-redox and redox reaction (acid medium)
4.5 Stoichiometry and limiting reactant calculations
Solution
5.1 Standard solution (preparation and dilution)
5.2 Concentration (molarity, normality, ppm, %w/w, %w/v, %v/v)
Chemical Bonding
6.1 Lewis dot structure
6.2 Ionic and covalent bond (Dative bond, exception of the octet rules)
6.3 Characteristics of ionic and covalent compounds
6.4 Intermolecular forces (Hydrogen bond and Van der Waals forces)
Acid and Bases
7.1 Theory of acids and bases (Arrhenius theory and Bronsted-Lowry theory)
7.2 Strength of acids and bases
7.3 pH and pOH calculations
7.4 Acid/base titrations (volumetric analysis, type, curve and indicators)
Chemical Equilibrium
8.1 Acid-base equilibria
8.2 Buffer solution
8.3 Common ion effect
1.1 Environmental problems (water pollution, air pollution, heavy metals)
1.2 Acid rain cycle, bleaching, a natural buffer
Structure of atom
2.1 Subatomic particles (atomic number, atomic mass, isotopes, atomic symbols, ions)
2.2 Quantum numbers
2.3 Electronic configurations (in terms of subshell and orbital diagram, including first transition elements)
Periodic Table
3.1 Periods, groups and blocks, relationship between electronic configuration and periodic table
3.2 Classifications of element
(metal, non metal, metaloid, transition elements)
3.3 Periodic trends
(atomic size, ionization energy, electron affinity, electronegativity)
Chemical Formula & Calculation
4.1 Molecules and compounds (identify, naming, formula)
4.2 Mole concepts (mass to mole conversion and Avogadro's number)
4.3 Empirical and molecular formula
4.4 Balancing non-redox and redox reaction (acid medium)
4.5 Stoichiometry and limiting reactant calculations
Solution
5.1 Standard solution (preparation and dilution)
5.2 Concentration (molarity, normality, ppm, %w/w, %w/v, %v/v)
Chemical Bonding
6.1 Lewis dot structure
6.2 Ionic and covalent bond (Dative bond, exception of the octet rules)
6.3 Characteristics of ionic and covalent compounds
6.4 Intermolecular forces (Hydrogen bond and Van der Waals forces)
Acid and Bases
7.1 Theory of acids and bases (Arrhenius theory and Bronsted-Lowry theory)
7.2 Strength of acids and bases
7.3 pH and pOH calculations
7.4 Acid/base titrations (volumetric analysis, type, curve and indicators)
Chemical Equilibrium
8.1 Acid-base equilibria
8.2 Buffer solution
8.3 Common ion effect
Frequently Asked Questions
Q1 : Any other courses in UiTM that equivalent to ENV 112?
A1 : No, this course was developed for environmental health science students in order to make them understand the use of chemistry concepts relevant to environmental health.
A1 : No, this course was developed for environmental health science students in order to make them understand the use of chemistry concepts relevant to environmental health.