Page Two <===> Units 3, 4, 5 & 6

Unit III Energy & Enthalpy

Note: There are three sub units in this Unit

Enthalpy and Heat
Rates of reactions and reaction Kinetics
Nuclear Reactions

Introduction to Thermodynamics.

What is energy, specific heat capacity & specific heat (know the difference) and calorimetry.
Heat question using Q = m/\tc with molar amount.
Specific Heat and Specific Heat Capacity, Numerical problems
Lab on Heats of Combustion; A lab on Heats of Reaction, NaOH + H₂SO₄ (neutralization)
Thermodynamics: Energy changes in a chemical reation, Enthalpy /\H State functions and the Law of Conservation of Energy
Calorimetry and Molar Heats of a Reaction Candle & alcohol experiment; Data given
Using reaction mechanisms to calculate an overall heat of reaction; another experiment, Ca + O₂; write up required.
This is a Hess's Law experiment
Standard Heats of Reactions and Thermodynamic Equations ==> Hess's Law.

Reaction rates:

Theory ===> Anything that either effects the collision of molecules or the pathway of a reaction mechanism will affect the rate of a reaction.BR> 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.
Collison Theory, Energy of Activation Theory & Transition State Theory. Be able to use these theories to explain the above mentioned FACTORS.
Make sure you understand each of the graphs that are shown here.

Nuclear reactions

==> fusion, fission and transmutation of elements under radioactive decay. Here's a picture of a nuclear reaction!

Heres a series of slides depicting the various nuclear reactions that you must know

Unit IV Equilibrium: The Theory

Starting in chapter 10
What is equilibrium; physical and chemical examples. The reversibility of a reaction
What effects equilibrium conditions
The Equilibrium Law for a reaction; how to handle mathematically
Equilibrium constants; what they mean. What is a reaction quotient (Q) and how does it relate to equilibrium conditions
Arriving at equilibrium and how to change its position
Le Chatelier's Principle; using to predict equilibrium shifts: right or left or not at all.

Equilibrium calculations
To use the quadratic formula or not; how does the concentration compare with the K_c?

Unit V Equilibrium;
Applications as applied to Acids/Bases and Solutions

Make sure you are aware of the terms related to solubility; opening sections of the chapter.
A saturated solution will be in dynamic equilibrium between insolubule solute and dissolved solute.

Working with K_sp
Equilibrium of insoluble salts. Know what a K_sp means and how to us it in calculations.
Common ion effect and Q, the reaction quotion; comparison of Q and K_sp to predict solubility.

Introduction to acids/bases:

see terms of reference -- indicator colours.
Acid Base Theories; Arrhenius and Bronsted-Lowery theories.
Conjugate acid base pairs
pH & pOH and how to convert to hydrogen ion concentrations and of course the reverse question.
pH + pOH = K_w
Using K_a of a weak acid to determine the pH of the solution, same can be done using a weak base.
How an indicator works; pH related colour changes in different indicators, bromthyol blue, methyl orange (orange IV) and phenolphthalein
Strong and weak electrolytes and strong & weak acids and bases.
Salts of weak acid and weak bases. Why some salts are considered neutral like NaNO₃

The Henderson-Hasselbach equation: a derivation is below

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)

Monitoring the pH of a solution when and acid or basic salt is added to its conjugate weak acid or base and calculating the pH when a strong acid or base is added to the buffered solution. Theory is based LeChatelier's principle.
Titration experiment:

This diagram illustrates how a titration is to be carried out.
Indicators and their respective pH colour range changes.

Those with range changes less than seven are useful when the equivalence point is under a pH 7. This occurs when a strong acid is titrated with a strong base.
When titrating a weak acid with a strong base indicator colour changes must occur in pH's greater than 7. A three titrations curves: make sure your know their differences. Two are shown here.

A Bit of a Summary

as to what you should know.

theory of; strong weak acids (bases), with experimental evidence, reaction quotient, pH, indicators (with examples) what a buffer how it works and why used with examples, conjugate acid and bases
How to prepare a buffered solution; mathematical calulations of the pH of a buffered solution.
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
Working with concentration problems. See problem set called "Equilibrium Problems #2"
Predicting preciptation using Q
Common ion effect; new solubility of effected anion or cation
Acid base theories
Working with acid or base concentrations to determine pH
The buffer solution
Polyprotic acids
Titration terminology

Unit VI Electrochemistry and Redox Reactions (Balancing)

Balancing equations using redox methods: two ways.
The importance of the standard hydrogen electrode
Using reduction potential tables to predict
will the reaction occur and
and the voltage of a given reaction.
constructing galvanic, voltaic cells. A demo lab will be done . Using a voltmeter to indicate current flow and the conclude which electrode is the anode.
Using oxidation potentials to varify experimental results and calculate the E^o of the two half cells.
electroplating potentials and reactions
corrosion
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.