Page Two

UNITS 3, 4, 5 & 6

Revision Date: April 1 2009

From Enthalpy to Electrochemistry

Day Twelve: Monday April 6 moved to Tuesday April 7

Organic reaction assignment to be handed in today or I really don't want it!
Quick discussion of polymers.

Unit III Energy & Enthalpy

Test on this unit will be on Wednesday the 15^th What is energy and its units
Review of Specific Heat and Specific Heat Capacity, Numerical problems, br> The calorimeter and Principle of Heat Exchange
Sample problems with one homework question + the usual stuff from the book, which I hope you are completing without being told. Favorite problem HCl + KOH ---> KCl + H₂O where you find the molar heat of this reaction. Your text is light in this area, hence I will not do this problem. May have been done on the last day depending on time (#6 on worksheet.
The next three days will intertwine. Introduction to Heat of a Reaction Enthalpy, a quick look at experimental procedures in order to determine the Entalpy of a Reaction.
Heats of Combustion: How much heat is given off when one mole of a substance is burned
Candle &/or alcohol experiment, write up required; Data given out; Make sure you include your letter
Make sure you do questions assigned from the test book.
Look at the Internet notes provided, I do tend to add to the list.

Day Thirteen: Thursday April 9 move to Wednesday April 8

Organic Test
Thermodynamics: Energy changes in a chemical reation, Enthalpy /\H State functions and the Law of Conservation of Energy
Thermodynamic equations with and without /\H notation
Calorimetry and Molar Heats of a Reaction:
Enthalpy of a Reaction: two methods:
a)Using reaction mechanisms to calculate an overall heat of reaction; Pathway doesn't matter.
b) Using tables; Standard Heats of Formation (the easier of the two)
Again, make sure you do assigned book questions. The NaOH or KOH + HCl experiment; data given & explained - write up to be done by student.

Day Fourteen: Tuesday April 14 moved to Wednesday April 15

Thermodynamic test is tonight.
Another experiment, Ca + O₂ ----> CaO. Determining the /\H for this reaction; experimental write-up.
write up required, hand in next Monday. This is a Hess's Law experiment. Proper write up required; your individual data letter is important.
Standard Heats of Reactions and Thermodynamic Equations ==> Hess's Law.
Bond enthalpies

Day Fifteen: Thursday April 16

Mid-Term marks are handed in.

Hess's Law using Standard Enthapies of Formations (Tables)
Review questions from the book

Energy of Activation and how it compares to kinetic energy distribution curve

Reaction Rates: Theory ===> you get out of the text. Factors effect rates are:

Temperature
Concentration Effects
Nature of Reactants
State of subdivision
Presence of a cataylst

I will concentrate on the numerical problems; LEGO example and working with experimental rate data.
Rate Law and determining the exponents in the rate law expression
Collison theory and energy of activation. Theory in text.
Temperature and potential energy & collision frequency distribution curves.
How a catalyst and a change in temperature will effect these curves.
Working with inital reaction rates to determine the rate law Test on this unit, next week if possible.

Day Sixteen: Monday April 20

Reaction orders and what they mean
More rate law questions

Start of Equilibrium
Equilibrium & what it means, open and closed systems and why equilibrium is not all that obvious
Forward & reverse reactions
Three types of equilibrium; phase, solubility, & chemical
Calculating the final equilibrium concentrations given final concentration of one of the species. The ICE Table

Day Seventeen: Thursday April 23

Parents night no class Full Disclosure Day: either drop out now or your mark will be recorded on your transcript.
Summary sheet

Homework assigned with time to work on

Day Eighteen: Monday April 27

Test Next day

Unit IV Equilibrium: The Theory

Starting in chapter 10
What is equilibrium; physical and chemical examples. Hand out notes. The reversibility of a reaction
Lego model to show equilibrium
Click here for a slide on NO₂ equilibrium
What affects equilibrium conditions, see note!
NO₂ <===> N₂O₄ equilibrium in ice water and when heated
Equilibrium constants; what they mean
The Equilibrium Law for a reaction; how to use concentration date to arrive at an equilibrium law expression.
H₂ + I₂ <====> 2HI reaction data

Day Nineteen: Thursday April 30

Test Unit Three ==> Enthalpy, Nuclear Reactions & Reaction Rates

A continuation with equilibrium; Le Catelier's Principle
Arriving at equilibrium and how its equilibrium position changes when a stress is applied ===>Le Chatelier's Principle
A look at last days handout notes.
Applying Le Chatelier's Principle to different reactions and making equilibrium shift predictions.
Doing the math ==> working with equilibrium expressions. Calculating the K_eq given equilibrium concentrations and the reverse: giving an initial concentration of reactants and the K_eq, determine the equilibrium concentations.
The mathematics of equilibrium; working with quadratic equations, short cut assumptions
Homework questions from this chapter (See Homework Site)

Day Twenty: Monday May 4

Equilibrium practice

Day Twenty One: Thursday May 7

More practice with Equilibrium calculations
Work sheet handed out, maybe. Quick look at ENTROPY Follow-up notes on entropy.

Day Twenty Two: Monday May 11

Introduction to Equilibrium Applications: Solubility;
Definitions, solubility, solvent solute, saturated, unsaturated etc. Entropy and solubility, Polar and non-Polar solutions, Gases in solution. This material is in the text. Read it.
Solubility rules ====> solubility product constant K_sp
Working with K_sp to determine solubility concentration when equilibrium is reached. Know what a K_sp means and how to us it in calculations.
Be able to determine K_sp given equilibrium concentrations and when K_sp is given calculate the equilibrium concentrations; be careful and watch out for mole ratio coefficients. (Don't forget to double pump these numbers). Common ion effect ; calculating the new solubility when a common ion is added. Q the reaction quotient; comparison of Q and K_sp to predict solubility. Questions done on the board.

Day Twenty Three: Thursday May 14

Small Test on Equilibrium Theory, Using LeChatelier's Principle and K_eq problems
If you plan on an ISU I should be aware of it & what you plan on reporting on.
Working with concentration values
Introduction to acids/bases: Notes handed out.
Two main theories of acids/bases: Arrhenius and Bronsted-Lowery; acid base pairs.
Mono, di and tri protic acids
pH ==> definition and calculating pH from concentration and the reverse using log button on your calculator.
Back to acids and bases but first we will look at the dissociation reaction that takes place in water
Electrolytes: strong and weak ===> demonstration.
Indicator colours. A demonstration using three indicators.
How an indicator works; pH related colour changes in different indicators
Strong and weak electrolytes and strong & weak acids and bases

Day Twenty Four: Thursday May 21

Test on Equilibrium ---> to Acids & Bases no buffer calculations.
Below is a more precise commentary on this upcoming test.

theory of; strong weak acids (bases), remember the light bulb experiment, reaction quotient, pH, indicators (with examples) what a buffer how it works and why used with examples, conjugate acid and bases
writing equilibrium law expressions
Using Le Chatelier's principle to predict equilibrium shifts
Numerical problems; K_sp K_eq problems going both ways molar solubility to K_sp and visa versa
pH to [H⁺] and visa versa
Arrhenius theory and Lowery-Bronsted theories of acid bases
proton donor and proton accepter

Work sheet on Balancing Equations; make sure you can do these.
Working with buffers, the math.
Acid salts, neutral salts, and basic salts. Note given out. Make sure your read, comprehend and if needed ask questions.
Calculating the pH of either an acid salt or basic salt. This is also part of the note.

Day Twenty Five: Monday May 25

Review of Salts of weak acid and weak bases. Why some salts are considered neutral like NaNO₃
End point and equivalence points ==> titrations of strong acid/strong base, titration of weak acid/strong base etc.
Buffering effects (same as common-ion effects) Using LeChatelier's principle.
Solving the "buffer" problem

Test should be the next day

Day Twenty Six: Thursday May 28

Equilibrium test;

Unit VI Electrochemistry and Redox Reactions (Balancing)

Determining oxidation state numbers
Oxidation reductions terms defined; see handout Balancing equations using redox methods: two ways. We only did one method

13-4, Balancing using half cell method
13-5 Electrochemical cells: Make sure you know what these terms are:
- electrode, anode, cathode
- cell potential, potential difference
- study carefully the diagrams on page 591
- half cell; note: two half cells equals one cell or a "battery"
- each half cell contibutes to the total voltage of the electrochemical cell. These values are listed in either the standard reduction potential tables or standard oxidation potential tables.
- the hydrogen half cell: (you will copy a note on this)
various examples of half-cell combinations are given in text 17-6, 17-8, 17-9
Calculating standard cell potentials: experimentally and using tables. Section 17-11

Day Twenty Seven: Monday June 1

Buffer problem revisited
Second method of balancing: Half cell method. When H₂O must be added. (Not emphasised) Using reduction (or oxidation) potential tables to predict
a) will the reaction occur.
b) voltage of a given reaction.
c) constructing galvanic, voltaic cells. A demo lab will be done. (ZINC COPPER & LEAD half cells were used). Measuring the voltage of two half cells and how an oxidation table is actually constructed. This will be another lab write up.
d) electroplating and reactions
e) corrosion
f) standard reduction potentials and how to use the values to predict reaction spontaneity. Check out the Nernst equation. E^o_cell can be positive, zero and negative; what does each mean. As the Doors once said

"THIS IS THE END, MY ONE AND ONLY FRIEND, THE END"

Do give my practice exam a shot ---> this should generate some questions

Day Twenty Eight: Thursday June 4

This should be an exam review day. Come with all your questions to be answered. You should have looked at the practice exam and be prepared to entertain questions.
Any review should be driven by YOU, not me!

Day Twenty Nine: Monday June 8

EXAM DAY ! Make sure you are on time. The clock begins ticking from 6:30, not when you walk into the room. Time permitted is 2.5 hours but it shouldn't take you that long. Make sure you have a pencil for the SCANTRON.

Note that there is no class this Thursday June 11 of this week. This is when the exam is to be marked.

Day Thirty: Monday June 15

Exam take up day. Come and see what you got! I would like to start this class a 6:00 so that any adjustments to be made are take care of, and the marks can be handed in by 6:30, as will be requested by the administration. Show up late and if an error has been made, a correction may be difficult.

All questions can be sent to me at rjwarren_stm@yahoo.com