1. Instructor: Dr. Jules Carlson
Theory Review Lecture
CHM1111 Section 04
Instructor: Dr. Jules Carlson
Class Time: M/W/F 1:30-2:20
Monday, November 28th

2. Key Concepts – Chapter 2 How is pressure measured? Unit conversions
Gas Laws
Ideal Gas Law
Concept of Mole Fractions (also ppm, ppb)
Dalton’s Law of Partial Pressures
Gas Stoichiometry Problems
Gas Density
Kinetic Molecular Theory
Molecular speeds, energies
Graham’s Law

3. Concepts for Chapter 4 Characteristics of Light
Electromagnetic Spectrum
Photoelectric Effect
Energy-Wavelength-Frequency Relationships
DeBroglie Wavelengths
Momentum (mass x velocity)
Heisenberg’s Uncertainty Principle
Describing Electron Orbitals
4 quantum numbers
Ways of depicting orbitals
Orbital Shapes

4. Concepts for Chapter 5 Extent of screening for different orbitals
Electron configurations
Structure of Periodic Table
Pauli Exclusion Principle
Aufbau Principle
Hund’s Rule
Exceptions to electron configurations for transition metals
Magnetic Properties
Atomic Properties
Orbital size
Size of atoms
Ionization Energy
Electron Affinity
Size of Atomic ions

5. Concepts for Chapter 6 Dipole Moments Bond Length and Energy Trends
Types of Bonding
Interaction Energy in Covalent Bonds
Electronegativity and Bond Polarity
Lewis Structures
Octet rule for n <= 2
Resonance structures
Minimize formal charge, optimizing
Molecular shapes
Bonding with p orbitals at 90 for H2S, PH3.
VSEPR – linear, planar, tetrahedral, trigonal bipyramidal, octahedral, pentagonal bipyrimidal
Dipole Moments
Bond Length and Energy Trends

6. Concepts for Chapter 7 Electron Delocalization
Orbital Overlap – s-s overlap, p-p overlap
Orbital Overlap Model and Drawings
Hybridization – Relation to Geometry
Linear sp, planar sp2, tetrahedral sp3, trigonal bipyrimidal sp3d, octahedral sp3d2, pentagonal bipyrimidal sp3d3
Molecular Orbital Theory
Bonding and Antibonding Concept and Overlap
Filling MO Diagrams
Calculating Bond Order, Magnetic Properties
Understanding the Shapes of s and p MOs with Positive and Negative Overlap

7. Concepts for Chapter 8 Intermolecular Forces in Different Phases
Phase Changes
Types of Intermolecular Forces
Strength of Intermolecular Forces – Influence on MP, and BP
Surface Tension, Capillary Action, Viscosity
Vapour Pressure
Forces in Solids
Types of Solids and Intermolecular Forces
Network Solids, Molecular Solids, Ionic Solids, and Metallic Solids
Solid Classification

8. Concepts for Chapter 9 Colligative Properties
Ways to Measure Solution Concentration
Mole Fraction, Mass Percent, Molarity, Molality
Miscibility of Solvents and Intermolecular Interactions
Solubility of Solids in Polar and Non-Polar Solvents
Energetics of Solubility
Gas Solution Equilibria and Henry’s Law
Solubility and Vapour pressure and Temperature
Solublility and Vapour pressure and Intermolecular Forces
Concept of Distillation
Colligative Properties
Raoult’s Law
Boiling Point Elevation and Freezing Point Depression
Osmosis and Osmotic Pressure

9. Unit Conversions Pascal: 1 Pa = 1 N/m2 = 1 kg/ms2
Bar: 1 bar = 100 kPa = 750 torr
Atmosphere: 1 atm = bar = Pa = 760 torr
Torr: 1 torr = 1 mm Hg = Pa
1 nm = 10-9 m
1 g/mL = 1 kg/L
Standard Temperature and Pressure (STP) – 1 bar, K
Convert from Celcius to Kelvin ⁰K = ⁰C

10. Constants
Ideal Gas Law Constant: R = L kPa mol-1 K-1 Ideal Gas Law Constant: R = L bar mol-1 K-1 Energy of molecules at 300K: 4.13x10-21 J/molecule Electron Mass: me = x kg Proton Mass: mp = x kg Neutron Mass: mn =1.675 x kg Avogadro’s Number: NA = x 1023 molecules/mol 1 Einstein is x 1023 photons Planck’s Constant: x J s Speed of light: c = x 108 m s-1 Ionization Energy of H: IE = 2.18 x J Density of Pure Water: ρ = 1.00 g/mL FP Depression Constant for Water: KfH2O = 1.86 C kg/mol BP Elevation Constant for Water: KbH2O = 0.51 C kg/mol

11. Chapter 2 Relationships

12. Most probable Kinetic Energy and velocity

13. Average Kinetic Energy, Velocity, Graham’s Law
Graham’s Law:
Called root-mean-square speed

14. Energy of Photons, Photoelectric Effect, Quantized Energies of H
Speed of light and wavelength:
Energy and Frequency:
Energy and Wavelength:
n is energy level
Photoelectric Effect:

15. Particle and Wave Equations + Heisenberg’s Uncertainty Principle
Table 4-1 p. 215

16. Concentration Relationships
Common ways to describe solution concentration:
Mole Fraction:
Henry’s Law:
1 Molar is 1 mol/L, and 1 Molal is 1 mol/kg

17. Colligative Property Equations
Raoult’s Law:
Osmotic Pressure:
Molar Mass from Osmotic Pressure: