Fawwaz Khan SCH 4U1 12 University Chemistry CPT Review UNIT 1: ORGANIC CHEMISTRY Lesson 1: Alkanes & Cyclic Alkanes - Alkanes - Structural Isomers - Alkyl Halides - Cyclic Hydrocarbons - Examples Lesson 2: Alkenes and Alkynes - Alkenes - Alkynes - Geometric Isomers of Alkenes - Reactions of Alkenes and Alkynes - Examples Lesson 3: Aromatic Hydrocarbons - Properties of Aromatic Hydrocarbons - Naming - Phenyl Group - Common Names - Reactions - Examples Lesson 4: Alcohols, Ethers and Thiols - Properties Alcohol - Naming Alcohols - Reactions Alcohols - ETHERS - Naming Ethers - Preparation of Ethers - Thiols Lesson 5: Aldehydes and Ketones - General Formula - Properties of Aldehydes and Ketones - Naming Aldehydes - Preparation (Oxidation) - Naming Ketones - Hydrogenation - Examples Lesson 6: Carboxylic Acid, Esters - Properties of Carboxylic Acids - Naming CA - Properties of Esters - Naming Esters - Reactions ………...…………………………………………1 ……...……………………………………………5 ………..…………………………………………9 ………...………………………………………..11 ………..………………………………………..13 ………...………………………………………..15 Fawwaz Khan SCH 4U1 - Esterification - Hydrolysis - Saponification - Examples Lesson 7: Amines and Amides …...……………………………………………..18 - Degree of Amines - Properties of Amines - Naming Amines - General Formula of Amides - Properties of Amides - Naming Amides - Reactions - Preparation of Amides - Reaction of Amides - Examples Lesson 8: Synthesis Reactions …...……………………………………………..23 - Flow Chart - Examples Lesson 9: Polymers and Polymerization …...……………………………………………..25 - General Molecular Structure - Types Polymerization - How are they formed? - Addition Polymerization - Condensation Polymerization - CROSS LINKAGE - Properties - Examples UNIT 2: QUANTUM CHEMISTRY Lesson 1: History of Atomic Theory - John Dalton - J.J. Thomson - Millikan’s Oil Drop Experiment - Discovery of Radioactivity - Rutherford’s Gold Foil Experiment - Nuclear (Beehive) Model - James Chadwick (Discovery of Neutrons) - Atoms and Isotopes Lesson 2: - The Wave Nature of Light - All forms of radiation - Quantized energy photons - Planck’s Assumption - The Photoelectric Effect - Bohr’s Model of the Hydrogen Atom ……………………………………29 ……………………………………31 Fawwaz Khan SCH 4U1 - Continuous Spectrum - Bohr’s Model Lesson 3: The Quantum Mechanic Model - The Wave Behaviour of Matter - The Uncertainty principle - The quantum mechanic model - Orbitals and Quantum Numbers - Pauli Exclusion Principle - Relationships Lesson 4: The Atomic Structure & Periodic Table - Electron Configuration - Shorthand Form - Electron Configuration of Transition Metals - Orbital Diagrams - Aufbau Principle - Hund’s Rule - Configurations and periodic table - Magnetic Properties - Ferromagnetism Lesson 5: Types of Chemical Bonds - Ionic Compound - Covalent Bond - Lewis Structure and Octet Tule - Valence Shell Electrons - Lewis Dot Diagrams - Rules for Drawing LD - Exception (Less or More) - Coordination Covalent Bonding Lesson 6: Molecular Geometry & Bonding Theories - Molecular Shapes - VESPR Model - Electron pair geometry - Molecular geometry - Rules for predicting - Two central atoms - Effective of nonbonding electrons and multiple bond on bond angles - Multiple bonds Lesson 7: Electronegativity & Polarity of Bonds - Electronegativity and Polarity of Bonds - Electronegativity and Covalent Bonds - Polarity of Molecules Lesson 8: Covalent Bonding & Orbital Overlap - Covalent Bonding - Hybrid Orbitals - Single Bonds ……………………………………33 ……………………………………35 ……………………………………39 ……………………………………40 ……………………………………42 ……………………………………43 Fawwaz Khan SCH 4U1 - Multiple Bonds Lesson 9: Intermolecular Forces - Ionic Dipole - Dipole-Dipole - Hydrogen Bonding - London Dispersion Lesson 10: Structure & Properties of Solids - Ionic Crystals - Metallic Crystals - Molecular Crystals - Covalent Networks Crystals - Semiconductors ……………………...Separate Page ……………………...Separate Page UNIT 3: THERMOCHEMISTRY Lesson 1: Introduction - Heat and Energy Changes - Types of Systems - Energy - Law of Conservation of Energy - Thermal Energy - Heat - Temperature Lesson 2: Calorimetry - Calorimetry - Types of Calorimetry - Coffee Cup - Bomb - Assumptions (Coffee Cup) Lesson 3: Enthalpy - Molar Enthalpy Change Lesson 4: Representing Enthalpy Changes - Endothermic - Exothermic Lesson 5: Bond Energies - Bond Energies - Additivity of Bond Energy Lesson 6: Hess’s Law - Hess’s Law of Summation - Rules Lesson 7: Standard Enthalpy of Formation - Equation Lesson 8: Rates of Reaction - Chemical Kinetics - Reaction Rate - Calculating Average Reaction Rates ……………………………………………47 ……………………………………………49 ……………………………………………51 ……………………………………………54 ……………………………………………55 ……………………………………………57 ……………………………………………60 ……………………………………………61 Fawwaz Khan SCH 4U1 - Calculating AROR - IROR - When ratios are not 1:1 Lesson 9: Explaining Reaction Rates - Collision theory - Activation energy - Activated complex - Transition States - Catalysts - Chemical Nature of Reactants - Concentration - Surface Area Lesson 10: Rate Law - Rate Equation Lesson 11: Reaction Mechanisms - Explanations ……………………………………………63 ……………………………………………65 ……………………………………………66 UNIT 4: EQUILIBRIUM Lesson 1: Introduction - Examples Lesson 2: Equilibrium Law & Constant - Equilibrium Constant Expression - General Equation - Constant vs Reaction Rates - Effects of Temperature - Magnitude Lesson 3: Equilibrium Calculations & Constant - Examples - Quotient (Q) Value Lesson 4: Le Chatelier’s Principle - Adding/Removing Product or Reactant - Effects of Pressure - Effects of Temperature - Effects of Catalyst Lesson 5: Solubility Equilibrium & Product Constant - Solubility Product constant - Common Ion effect Lesson 6: Acid and Bases Summary of Theory - Arrhenius Theory - Bronsted Lowry Theory - Conjugate Acid/Base - Ionization Lesson 7: Strong & Weak Acid & Bases - Types of Acids - Weak Acids/Bases ………………………………….67 ………………………………….68 ………………………………….70 ………………………………….72 ………………………………….73 ………………………………….77 ………………………………….78 Fawwaz Khan SCH 4U1 - Self Ionization of Water Lesson 8: pH Scale - pH - pOH - How to measure? - Weak Acids - Calculating Ka - Precent Ionization - pH for polyprotic acids - pH of Weak acids Lesson 9: Salt Solutions - Rules - Neutral Solutions - Weak Solutions Lesson 10: Acid Base Titrations - Titration Curves - Strong and Weak Acid and Base - Weak Acid & Strong Base ………………………………….79 ………………………………….82 ………………………………….83 UNIT 5: ELECTROCHEMISTRY Lesson 1: Electron Transfer Reactions …………………………………………………...92 - Electrochemistry - Oxidation Reduction Reactions - Rules for Oxidation Numbers - Identifying Agents Lesson 2: Balancing Redox Reactions …………………………………………………...94 - Requirements - Half Reactions Lesson 3: Galvanic Cells …………………………………………………...96 - Household Battery - How galvanic cells work? - Line notation - Diagrams Fawwaz Khan SCH 4U1 Lesson 9: Intermolecular Forces Ionic Dipole Forces: - Forces that exist between an ion and a partial charge at the end of a polar molecule. London Dispersion Forces - Forces that exist between non-polar molecules. Fawwaz Khan SCH 4U1 Dipole-Dipole Forces: - Forces that exist between neutral polar molecules - They attract each other when the positive end of one molecule is close to the negative end of another molecule - They are effective only when polar molecules are close together, generally in solution - They are weaker than ion-dipole forces - at some instance, the 2e- of helium will be on the same side creating a partial dipole - when it comes in contact with another helium atom, it will cause the electrons of the other helium atom to move to the opposite end of the molecule - the negatively charged original helium atom will be attracted to the positively charged nucleus of the second helium atom - the strength of London Dispersion Forces increases with increasing molecular size, mass and number of electrons. Hydrogen Bonding - Attraction that exists between the hydrogen atom in a polar bond (particularly an H-F, H-O or H-N bond) and an unshared electron pair on a nearby electronegative ion or atom (usually O, F or N atom) - They are stronger than both dipole and dispersion forces. - They are significant to biological activities such as the structure of proteins. Fawwaz Khan SCH 4U1 Lesson 10: The Structure and Properties of Solids - A crystalline solid is a solid whose atoms, ions or molecules are ordered in well defined arrangements - The physical properties of crystalline solids, such as melting point and hardness, depends on both the arrangement of particles and on the attractive forces between them. Ionic Crystals - Ionic solids are held together by ionic bonds - T he strength of the bond depends on the charges of the ions Typical Properties: - Hard, high melting points, non-conductors of electricity as solids but good conductors when melted Metallic Crystals - These crystals consist entirely of metal atoms - The bonding is due to valence electrons delocalized throughout the entire solid - The strength of the bonding increases as the number of electrons available for bonding increases Typical Properties: - Range from hard to soft, melting points range from high to low, conduct electricity well, have characteristic lustre Molecular Crystals - Consists of atoms or molecules held together by intermolecular forces - The properties depend on both the strength of the forces that operate between molecules and also on the ability of the molecule to pack efficiently in three dimensions. Examples: Water/Ice Typical Properties: - Soft, low melting points, non-conductors of electricity Covalent Networks Crystals - Consists of atoms held together in large interlocking networks or chains by covalent bonds Fawwaz Khan SCH 4U1 - Can be one non-metal (graphite or silicon) or two nonmetals (SiC, SiO2) - 2D or 3D Typical Properties - Very hard, very high melting points, non-conductors of electricity Semiconductors - Increase temperature causes the vibration of silicon atoms - Electricity can be controlled through doping - N-type doping involves adding electrons to the network by replacing Si with atoms in group 5 (ex. P) - P-type doping involves removing electron from the network by replacing Si with atoms in group 3 (ex. B)
