Syllabus for CHEM1001 (Fundamentals of Chemistry 1A)

The order of topics presented here is essentially the order of presentation in the lecture course, although individual lecturers may make some variations from this. Some topics span more than one week.

Week

Topics covered

Introduction

- admin. matters

- overview of course

Elements and Atoms

- elements, compounds and mixtures

- physical and chemical change

- chemical symbols

- allotropes

Elements and Atoms (continued)

- atomic structure

- protons

- electrons

- neutrons

- atomic number

- isotopes

- radioactivity

- shell structure

Molecules and Ions

- formation of ions

- ionic compounds: formation, formulas, naming

- covalent bonding, valence, bonding/nonbonding pairs

Molecules and Ions (continued)

- double and triple bonds

- naming covalent compounds

- polyatomic ions

- empirical, molecular, and structural formulas

- types of bonding in solids

Chemical Equations

- reaction types: combintaion, precipitation, decomposition, replacement, acid/base

- molecular/ionic equations

- specification of phase

- balancing equations for neutral and charged species

- reactions involving acids

Stoichiometry

- atomic, formula and molecular weights

- the Avogadro constant, the mole and molar mass

- % composition, empirical and molecular formulas

- calculations involving balanced equations

- limiting reagents and percentage yield

- molarity and calculations on solutions

The Periodic Table

- chemical basis of the periodic table using main group element

Atomic Energy Levels

- shapes of atomic orbitals and quantum numbers

- Aufbau principle

Lewis Model of Bonding

- Lewis structure

- pi bonding

- resonance

- bonding in O₃, CO₃^2-, NO₃^-, benzene, etc

VSEPR

- molecular shape

- application to larger molecules including organic molecules

- shape and bonding of common functional groups

Liquid Crystals

- packing determined by shape

Gas Laws

- effects of temperature and pressure on volume

- ideal gas law

Thermochemistry

- heat and temperature

- greenhouse effect

- kinetic and potential energy

First Law of Thermodynamics

- heat capacity

- enthalpy

- enthalpy change in a reaction (endo- and exothermic)

- enthalpy as a state function

- Hess's Law

- heat of formation

- CO₂ /energy release from fuels

- use of H₂ as an alternative fuel

Types of Intermolecular Forces

- dipole, induced dipole, dispersion, hydrogen bonding

- effects on boiling points

Oxidation Numbers

Nitrogen Chemistry & Compounds

- high explosives

- nitrogen biocycle, nitrification and denitrification

- hydrides, halides, oxides, oxoacids

Nitrogen in the Atmosphere

- NO/NO₂ cycle

- formation of pollutants

Chemical Equilibrium

- equilibrium as a dynamic process

- the equilibrium constant

- the reaction quotient

- predicting direction of chemical change

- equilibrium calculations

- introduce particular equilibrium constants

- K_p and partial pressures

- K_c and units of concentration

- K_sp

- equilibrium calculations

- K_a and K_b; pK_a and pK_b

- Le Chatelier’s principle

Equilibrium and Thermochemistry in Industrial Processes

Mining

- general principles

- example: Mining of copper

- example: The Steel Story

Top 10 chemicals produced in the world:

- special example, sulfuric acid, ammonia

Introduction to Electrochemistry

-oxidation states

-redox reactions

-cell potential

-half-reactions

-voltaic Cells

Electrochemistry

-voltaic or galvanic cells

-using half-reactions

-table of standard reduction potentials

- effect of concentration

-Nernst Equation

-link between E and K

-concentration cells

Electrochemistry (Batteries & Corrosion)

- difference between primary and secondary batteries

- how common batteries work

- fuel cells and how they work

- corrosion and corrosion protection

Electrolytic Cells

- how does electrolysis work?

- concept of overpotential

- chlor-alkali process (H₂, NaOH, Cl₂ from seawater)

Week	Topics covered
1	Introduction - admin. matters - overview of course Elements and Atoms - elements, compounds and mixtures - physical and chemical change - chemical symbols - allotropes
2	Elements and Atoms (continued) - atomic structure - protons - electrons - neutrons - atomic number - isotopes - radioactivity - shell structure Molecules and Ions - formation of ions - ionic compounds: formation, formulas, naming - covalent bonding, valence, bonding/nonbonding pairs
3	Molecules and Ions (continued) - double and triple bonds - naming covalent compounds - polyatomic ions - empirical, molecular, and structural formulas - types of bonding in solids Chemical Equations - reaction types: combintaion, precipitation, decomposition, replacement, acid/base - molecular/ionic equations - specification of phase - balancing equations for neutral and charged species - reactions involving acids
4	Stoichiometry - atomic, formula and molecular weights - the Avogadro constant, the mole and molar mass - % composition, empirical and molecular formulas - calculations involving balanced equations - limiting reagents and percentage yield - molarity and calculations on solutions
5	The Periodic Table - chemical basis of the periodic table using main group element Atomic Energy Levels - shapes of atomic orbitals and quantum numbers - Aufbau principle Lewis Model of Bonding - Lewis structure - pi bonding - resonance - bonding in O₃, CO₃^2-, NO₃^-, benzene, etc
6	VSEPR - molecular shape - application to larger molecules including organic molecules - shape and bonding of common functional groups
7	Liquid Crystals - packing determined by shape Gas Laws - effects of temperature and pressure on volume - ideal gas law Thermochemistry - heat and temperature - greenhouse effect - kinetic and potential energy
8	First Law of Thermodynamics - heat capacity - enthalpy - enthalpy change in a reaction (endo- and exothermic) - enthalpy as a state function - Hess's Law - heat of formation - CO₂ /energy release from fuels - use of H₂ as an alternative fuel
9	Types of Intermolecular Forces - dipole, induced dipole, dispersion, hydrogen bonding - effects on boiling points Oxidation Numbers Nitrogen Chemistry & Compounds - high explosives - nitrogen biocycle, nitrification and denitrification - hydrides, halides, oxides, oxoacids Nitrogen in the Atmosphere - NO/NO₂ cycle - formation of pollutants
10	Chemical Equilibrium - equilibrium as a dynamic process - the equilibrium constant - the reaction quotient - predicting direction of chemical change - equilibrium calculations - introduce particular equilibrium constants - K_p and partial pressures - K_c and units of concentration - K_sp - equilibrium calculations - K_a and K_b; pK_a and pK_b - Le Chatelier’s principle
11	Equilibrium and Thermochemistry in Industrial Processes Mining - general principles - example: Mining of copper - example: The Steel Story Top 10 chemicals produced in the world: - special example, sulfuric acid, ammonia
12	Introduction to Electrochemistry -oxidation states -redox reactions -cell potential -half-reactions -voltaic Cells Electrochemistry -voltaic or galvanic cells -using half-reactions -table of standard reduction potentials - effect of concentration -Nernst Equation -link between E and K -concentration cells
13	Electrochemistry (Batteries & Corrosion) - difference between primary and secondary batteries - how common batteries work - fuel cells and how they work - corrosion and corrosion protection Electrolytic Cells - how does electrolysis work? - concept of overpotential - chlor-alkali process (H₂, NaOH, Cl₂ from seawater)