This page is meant for summer school students at Bateman who wish to keep up to date with the program.
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Final exam hints ==> pages to look at and material to know Click here
Exam Hints

Below is a course outline based on date. It is a rough guideline as to when material will be taught. A more detailed outline based on subject matter can be found at OAC Chemistry Page

Course Outline per Date

Day One July 4 Tuesday Atomic Structure Chapters 3 & 4

1. Nomenclature of acids and bases, diatomic gases, criss-crossing valencies
2. The mole and stiochiometry, finding formula weights from a formula and number of moles given a weight.
   Using the balanced equation to deduce mole ratios of reactants and products
   Exothermic and endothermic reactions.
3. Periodic table, information that can be read from it.
4. Lewis dot diagrams of the elements; valence electrons only.
5. Introduction to organic nomenclature, alkanes, alkenes, alkynes, and cyclo compounds
   How to name a compound with add on elements or substituent groups; remember to say what it is and where it goes. Entries are separated by dashes.
6. Quick mention of ideal gas law PV = nRT

Chapter 3

• The atom according to Bohr-Rutherford, shell structures to derived atomic orbitals.
• Experiment to show spectroscopic analysis of H₂ gas. 3/4 visible lines
  Hydrogen atom spectrum; 4 colours; n = 6, 5, 4, 3 to n = 2 transitions (The Balmer series) Lyman and Paschen series mentioned, one is ultraviolet and the other is infrared.
  Zeeman effect and what it leads to ===> Shells are composed of orbitals or sub-shells.
  
• Filling in shells with the correct number of electrons; maximum number of electron per shell, 2, 8, 18, 32 etc.
• Identifying orbital (s, p, d, f) and how many electrons each can hold; 2, 6, 10, 14 etc.

Day Two July 5 Wednesday

• Video presentation: Atoms and Their Electrons; Arrangement of electrons and how/why atoms combine.
  
• Energy level diagrams with proper sequencing.
• Energy level diagrams and/or electron configurations based on these principles
• The four quantum numbers; n, l, m, & s
• Shapes of the s, p, d, f orbitals
  
• The Quantum Numbers and their relationship to each other.   Selection Rule ===> n > l ≥ |m_l|
  
  • Aufbau Principle
  • Pauli Exclusion Principle
  • Hund's Rule
• Electron Energy Level Diagrams and Electrons Configurations; Know what they are and the difference
  
• The Heisenberg Uncertainty Principle Propability distribution of electrons in a shell ==> the electron cloud concept.

Day Three July 6 Thursday

• Identifying bonding and non-bonding (lone pair) orbitals . Bonding types: ionic & covalent.
  Terms:
  • Ionization energy
  • Electronegativity
  • Electron affinity
  • Polar bond
  • dipole moment
  • bonding continuum
  • What does 1.7 mean

  Chapter 4

• Lewis dot diagrams for atoms molecules and polyatonic ions

Day Four July 7 Friday

• Lots of handouts on this section
• Make sure you get my note on Intermolecular forces
• Shapes of molecules based on Valence Shell Electron Pair Repulsion Theory (VSEPR). How to develope the chart; Total number of electron pairs versus coordination number. AXE formulation
• Polar and non-polar molecules. Electronegativity differences and the bonding continuum. 1.7, what does it infer.
• Dipole moments and poplar molecules vs polar bonds.
• Three modes of molecular motion: translation, rotation and vibration and how these are effected by temperature.
• Intra and inter-molecular forces. Bonding in solids: ionic, metallic, molecular, network & amorphous.
  Hydrogen bonding, dipole forces and induced dipole - induced dipole interactions (London forces)all of which are the Van der Waals forces, the weak ones.

Day Five July 10 Monday

• Video on Ionic and Covalent Bonding with worksheet
• Energy values for the forces holding aggragates together.
• Shape and bonding in two & three dimensional network solids and relate to various physical properties such as electrical conductivity, hardness, melting point, volatility.
• Using the periodic table to predict which elements will form network solids or molecular solids.
• Recognize and explain which elements form liquids or solids held together predominantly by Van der Waals forces.
• The four types of molcular solids as define by the interforces of attraction.
• Lots of handouts and summative board note

Chapter 1

1. family of compounds
2. IUPAC nomenclature
3. Reactions and synthesis of the above family
4. text seems very heavy on isomers especially within families

• Review: Introduction to the alkane family. Memorize these names folks; all ten of them. (Was done on Monday).All nomenclature will depend on you knowing these root names.
  
• The alkane may lose a hydrogen and become a alkyl unit. Example; ethane C₂H₆ becomes ethyl -C₂H₅
  Four main substituents groups methyl, ethyl, propyl and butyl with isomers were looked at.
• When attached to another hydrocarbon it becomes a substituent "add-on" unit to a given compound. Must say what it is and where it goes.
  
• Naming simple organic compounds from structural formulae by IUPAC method.(Organic nomenclature). Writing organic formulae from organic names.
• The Prioriety List. The main compounds formed when oxygen is added to the mix. Developed on the board with examples.
• Recognizing carbon chains and various substituent groups Drawing structural formulae. Using structure and formula to determine the number and structure of isomers. Examine and compare the properties of several isomers.
• naming organic functional groups in long carbon chains. Benzene and its derivatives (aromatic compounds)
  Test on Organic Unit & Polymers next Thursday or Friday
  Start looking at the polymer assigmnent. Due next week.

Day Six July 11 Tuesday

• Chapter 4 Test
• Drawing organic compound given a structural diagram and drawing diagrams from the name; many examples done in class with a complimentary work sheet.
• Hybridization of carbon atom; sigma, pi bonding molecular orbitals
  1. sp³ for single bonds bond - rotation is allowed.
  2. sp²) and one p orbital for double bonds - rotaion is not allowed; cis - trans isomers result.
  3. sp hybridization with two p orbitals for triple bonds - rotion is not allowed.
• Be aware of the general physical and chemical properties and uses of representative samples of the various organic series.
  Summary sheet given out on this, please read.
• Reactions of alkanes and alkenes
• Hydrogenation, halogenation, elimination E1 & E2 reactions, dehydration.
• Test review and preparation for tomorrow's test.

Day Seven July 12 Wednesday

• Required LabsOrganic reactions: Synthesis & Reactions of will be the general way the topic is covered. Handouts on what labs would/should be done in this unit. You are expected to know the procedures and results of these lab activities.
• Identify saturated and unsaturated hydrocarbons: various tests using Baeyer's solution or bromine water.
• Experiment: saturation vs unsaturation, addition reaction preparation and collection of acetylene. Test with KMnO₄: observations and conclusions.
• Video called Carbon Chemistry about 45 minutes.
  A set of worksheets will be provided so that you can record info as video proceeds. (3 pages)
  
• Oxidation of 1^o, 2^o, 3^o, alcohols with oxidizing reagent K₂Cr₂O₇
• Hot copper + alcohol
• esterification === making an ester from an alcohol and an acid
  ester identification by smell.
• polymerization

Day Eight July 13 Thursday

Chapter 2

• Physical properties ==> three types of solid polymers
  • elastomers
  • thermoplastics
  • thermosetting polymers
• carbohydrates, sugars and starches

Start of Thermodynamics Chapter 5

• Some math examples; how good is your algebra
• Introduction to thermodynamics: definitions with units of heat, temperature, specific heat capacity, Principle of heat flow, equilibrium, closed-open systems, calorimetry
• Q = mΔtc and its use (calculations) when mixing quantities of water

Day Nine July 14 Friday

• Define or state the meaning of the following: energy (endothermic, exothermic, enthalpy.); change of enthalpy or heat of reaction; Hess’s Law ; standard heat’s of formation; translational, vibrational, rotational modes of motion; molar enthalpy; enthalpy from bond formation.
  
• Experiment: Calorimetry:
  Two experiments: Heats of combustion, simulated experiment with data values being given; you do the write up.
  and adding sulfuric acid to water, carried out in the lab with proper write up. Reporting experimntal error
• Hess' law and using either given equations or standard heats of formation to solve for ΔH of a reaction
  
• End of period was devoted to an organic unit review with help from a video.

Day Ten July 17 Monday

• Mathematical calculations involving heats of reaction and standard heats of formation. to determine the enthalpy of a reaction.
  Using table found on page 799, 800 of text book.
• Explanation of energy storage by molecules in terms of kinetic and potential energy.
• Relate the heat of a reaction to the change in enthalpy in a chemical reaction. Interpret potential energy diagrams.
  
• Using Standard Heats of Formations Tables to calculate molar enthapies of reactions.(Actually done yesterday). More review on this topic.
  
• Bond energies and Born-Haber cycles
  
• Entropy and the spontaneous reactions
  

  ---

• Working with entropy changes. This is ths ΔS function
  Gibbs Free Energy ΔG = ΔH - TΔS and predicting the spontaneity of a reaction. A copied note
  Spontaneity pops up in equilibrium also.
• Video on what drives a reaction; entropy and enthalpy

Day Eleven July 18 Tuesday

• Experiment: Hess Law: Heats of reaction: To experimentally determine the heat of combustion of calcium by reacting calcium in hydrochloric acid and calcium oxide in hydrochloric acid (formation of water from tables).
  
• Explination of lab activity, with demonstration as to how the experiment was done. Data given to student groups with write handed in at the end of the period.
• Move on to the next topic or chapter

Rates of Reactions:Chemical Kinetics Chapter 6

• define and set up reaction rate parameters.
  Note on factors that affect a reaction rate; this was aa grade 10 topic.
  Concentration, surface area, temperature and catalysts.
• Video seen on Chemical Kinetics and what effects the rate of a reaction. A Chem Study video.
• Use of LEGO to demonstrate rate concepts
  How fast can Y₂R be built? Linearized data given to assit understanding.
• Simple linear example; graphical analysis; slope of graph to calculate rate
  
• Using initial rate values for several trial runs to calculate the Rate Law expression ( deducing the m & n's ) Finding the order of the reaction and the value of k.
  More mathematical calculations (continued practice).
  
• Experiment to illustrate the factors that effect the rates of a reaction.

Day Twelve July 19 Wednesday

• More questions to dermine reaction order and find k, a little more complex.
• Video titled Rates of Chemical Reactions Wards
• Introducing the energy of activation and the activated complex
  
• Rate determining steps.
  
• Explain on the basis of collision theory, how various factors create differences in reaction rates. What is a reaction mechanism, activation energy, activated complex and how it determines the chemical reaction rate.
  
• Collision theory and the activated complex; how catalysts effect reaction rates. Types of catalysis and how they work with example of each.
  
• Experiment: Several reactions are carried out with and without a catalyst to compare reaction rates and make quantitative measurements as seen in the videos.
  Hydrogen peroxide decomposition with MnO₂ and potato.
• Time to practice questions from chapters 5 & 6, help as needed.

Day Thirteen July 20 Thursday

Introduction to Chemical Equilibrium Chapter 7
The Theory of Equilibrium

• Introductory definitions, terms and general concepts
  
• The N₂O₄ <====> NO₂ system and the effect of temperature on this system in an ice-water / hot water bath.
  and the H₂ + I₂ <====> 2HI system
  
• Using experimental values to derive an equilibrium expression.
  
• Intoducing K_c and K_p, what they mean and how they can be equated.
• Define or state the meaning of the following terms: homogeneous system, heterogeneous system, closed, open systems, law of chemical equilibrium, dynamic equilibrium, LeChatelier’s principle, entropy.
• List the conditions that are necessary for chemical equilibrium.
• Comparing rate and equilibrium graphs as equilibrium is reached.
• Reaction quotient Q; how it can be used to determine if a give set of concentrations are at equilibrim with each other and how the reaction must shift to attain equilibrium.
• State LeChatelier’s principle and apply it to systems at equilibrium; when a strain is applied to a system at equilibrium which way will the equilibrium shift and why. Define and use the equilibrium constant. Establish conditions for equilibrium and the dynamic nature of equilibrium. by observing the effect of temperature, pressure or concentration on a system in equilibrium.. Closed and open systems.
• Review for tomorrows test using text book quizzes.

Day Fourteen July 21 Friday

Test on Enthalpy, Reaction Rates: Chapters 5 & 6

Equilibrium - Applications Part I

• Mathematical calculations using the equilibrium constant and being able to determine new concentrations when the equilibrium has been shifted due to a change put on the system..
  
• Define or explain the meaning of the following: solubility product, salt,
  
• Comparison of solubility rules and K_sp values to determine concentration. Mathematical problems using K_sp
• Working with K_sp either to find K_sp given molar solubilities or else when given the K_sp you must find molar solubilities.
  Always remember to start with the balanced equation, you need the coefficients to solve the problems.

Day Fifteen July 24 Monday

• The common ion effect. Mathematical calculations using K_eq and a given ion; how increasing one of the ion's concentration shifts the equilibrium.
  Based on LeChatelier’s principle.
• Comparison of Q and K_sp; will a precipitate form?
  Make sure you dilute the final mixed solution in order to use the correct concentration.
  Use the formula Conc_i X Vol_i = Conc_f X Vol_f
• Video on equilibrium

Applications Part II Acids & Bases

• Review of the "I should know" material of acids and bases.
  pH, [H⁺¹], K_w, K_a, K_b. Know the various theories of acid/bases: Arrhenius, Bronsted-Lowry, and Lewis.
  
• The ion product of water and k_w
• The definition of pH. Working with pH. pH to concentration and concentration to pH
  pH and pOH when added together equals 14
  K_a, K_b, K_w to determine final concentrations. Doesn't look like much but there is a lot of math here folks.
• Video experiment to investgate the colour changes of methyl orange (4), methyl red (5), bromthymol blue (7), and phenolphthalein (9) in acid, water and base and at what concentration they change colour.

Day Sixteen July 25 Tuesday

• Calculating either the H⁺¹ conentration or pH of a solution of either a weak acid or weak base. Strong acid or base determination is to trivial because of complete ionization.
• Determining the K_a or K_b for weak acids & bases.
• Calculations involving buffer solutions. Adding a salt to a solution; how its pH is affected.
  pH calculations when HCl is added to a buffered acetic acid solution
• End points and equivalence points and their importance in weak acid/weak base titration. A quick explination before you do the experiment. See graph on the other site; the OAC Page based on material covered not time lines.
  
• The three types of salts; acidic, basic and neutral. What the anion cations tell you.

Day Seventeen July 26 Wednesday

• Review titration techniques. Graphical analysis of pH vs volume of titrant added for strong /weak acid base combinations
• Experiment: simple titration using phenolthphalien indicator. An I hope or wish experiment.
  
• More buffer calculations. Using a base this time.

Electrochemistry and Redox Reactions

• Define the following redox terms: oxidation reduction, oxidizing agent, reducing agent, oxidation state, oxidation number. Rules for determining oxidation state numbers.
• Balancing redox reactions using charge then mass balance techniques.
• Describe the process that occurs when an electric current is applied to a chemical reaction, with examples. Define the terms; anode cathode electrode, half-cell, half-cell reaction. voltage potential, electron flow when two half-cells are connected.
• Standard oxidation potentials and how to read the table. Applying the table to predict the spontaneity of a reaction. Electrochemical cell and electrolytic cells. .
• Experiment using two half cells /Zn⁺⁺\\Cu⁺⁺/Cu.
• Predicting the voltage of this cell using oxidation tables
• The standard hydrogen electrode
• Using either oxidation or reduction potential tables
  
• Commercial applications of electrochemical cells and electrolysis of water and electroplating.
• Experiment: Electrochemical cells and standard Potential table
  

Day Eighteen July 27 Thursday

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Day Ninteen July 27 Thursday

Day Twenty July 28 Friday

EXAM

This exam will be broken into two parts. You do one part then hand it in and then commence the second part. Exam will be marked by the end of the day and final grade submitted to the office.

Exam Hints

Exam Format

• Multiple Choice about 35 of 'em. Covers all units. Something for everyone
  
• Fill in the blanks: its like multiple choice without the choice.
• Written, full answer questions, on foolscap
• An organic page; standard organic material
• The math page: I try to cover all the major types of problems involving calculations; heat, rates, equilibrium, common ion, buffers.
• The Lab Page: questions based on the lab activities that you did. (Some small some Big) Make sure you review and know this material well. Not just one lab. Check out all labs that we did.
  
• Analysis question

These page probably cover at least 80% - 85% of this exam.

• Draw an energy level diagram for any atom or ion
• Name organic molecules from a picture
• Draw a projection diagram of an organic molecule given a name
• complete an organic reation
• isomers, polymers ---> what are they with examples
• electromagnetic radiation and the spectrums of hydrogen
• enthalpy pathways and using standard heats of reaction
• draw an electrochemical cell, properly labled, of course. Electron flow and half-cell voltages
• work with initial reaction rates to find a rate law expression & the value of K
• factors effecting the equilibrium of a reversible reaction and how the reactions shifts in response to a given stress
• enthalpy graphs ---> how to read and draw
• nuclear decay and transmutation
• all of the labs we did
• Work with K_sp K_a K_b in all problem modes or formats
• common ion effect & buffer solutions (are essentially the same type of problem)
• determine oxidation numbers of atoms in a molecule
• balance redox equations
• shape of aggragates
• types of intermolecular forces
• properties of these forces
• calculating heats of combustion from measured data or using enthalpy tables
• working with lab results similiar to what was done in class
• calculating theoretical voltages from either oxidation potentials or reduction potentials
• titration curves, indicators, equivalence points and end points for weak acid - strong base or weak base - strong acid curves. Picking the right indicator.
• pH and pOH conversions to and from hydrogen ion concentrations
• given initial concentrations find equilibrium concentrations
• given solubility find K_sp and visa versa (watch out for the quadratic)
• finding [H⁺] or pH of weak acid using K_a (same type of problem for bases)
• will a precipitate form ==> using the reaction coeffient (Q)
• acid salts / basic salts When added to water or a solution what's the pH (or pOH)
• orbital shapes diagrams of, relation between the 4 quantum numbers

Good LUCK to All and STUDY STUDY STUDY
Just "remember what the door mouse said, "Feed your head"" Do you know what song this is from and who sings it ?