The course presented here is the exact General Chemistry II course that I taught as a university professor in a Chemistry Department that was certified by the American Chemical Society, the professional organization for chemists. All topics that are essential to any General Chemistry II course are covered here in detail. My teaching style for this Udemy course is exactly how I taught in the lecture halls. Each topic is explained in detail, terms are defined and then examples are done to show how the theory is applied in practice.
As was the case when I was teaching at the university, students have access to ample supplemental material, all of which will be in the Resource Folders. In addition to the 25+ hours of lectures, I have included a downloadable audio mp3 file of each lecture. For each lecture, I’ve included a Practice Assignment where you can test your understanding of the material. Also included is a detailed answer key for each Practice Assignment. A total of nearly 100 examples are worked out in the lectures and for each section I have included a list of the problems that you can download and follow along. Any graphs, figures or tables presented in the lectures are also available as downloadable files.
This course assumes that you have completed a General Chemistry I course but may not have taken any chemistry in high school. This course, and my First Semester General Chemistry course also available on Udemy, are ideal for anyone who needs to take General Chemistry at the college level but did not have it in high school. These courses are also well-suited for those who need to refresh their knowledge of General Chemistry before taking it at the college level.
Since chemistry is a quantitative science, a working knowledge of high school algebra is needed. In this course, you will also need to be familiar with logarithms and exponential functions. If your math skills are weak, this course will show you what types of math calculations are needed and you can hone those skills prior to your taking the course at a college level.
For this Udemy course, I used the Openstax Chemistry textbook which is also available in PDF format in the Resource Folder of the first lecture for this course. However, if you already have an old textbook, that may also work for you. Topics may be presented in somewhat different order, however.
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1
Intermolecular ForcesEach of the four Intermolecular Forces is identified and defined. Example compounds are given for each force.
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2
Strength of Intermolecular Forces in Molecules
The strengths of the Intermolecular Forces are compared. Higher and lower boiling points of compounds are compared based on the different Intermolecular Forces, sizes and shapes of the molecules.
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3
Properties of Liquids
The properties of liquids including viscosity, surface tension, adhesive forces and capillary action are described.
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4
Phase Transitions
Intermolecular Forces are used to explain the phase transitions of matter including freezing, melting, evaporation, condensation, sublimation and deposition.
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5
Vapor Pressure and Boiling Points of Liquids
Vapor Pressure and boiling points are defined in terms of Intermolecular forces. The relationship between the two is explained.
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6
Determining Heats of Vaporization
Derivation of the Claussius-Clapeyron Equation used to determine heat of vaporization.
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7
Heating and Cooling Curves
Heating and cooling curves are explained and an example calculation is done.
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8
Phase Diagrams
Phase Diagrams are defined and constructed for water and carbon dioxide.
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9
Properties of Solids
Types of Solids are discussed and properties of crystalline solids are given.
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10
Lattice Structures in Crystalline Solids
The crystal structure of solids is discussed including the Bragg equation, unit cell structure, stacking patterns, coordination number and the number of atoms in a unit cell based on unit cell type.
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11
The Dissolution Process
Solutions are defined and reasons why certain chemicals form solutions are given. Discussion of how salute and solvent intermolecular forces determine the Heat of Solution.
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12
Electrolytes
Electrolytes and Non-Electrolytes are defined with examples of each given.
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13
Solubility
Solubility is defined and the solubility of solid solutes in liquid solvents as a function of temperature is discussed.
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14
Solubility of Gases in Liquids
Application of Henry's Law which governs the solubility of Gases in Liquids.
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15
Concentration Units
The concentration units of mass percent, mole fraction, molarity, molarity, parts per million and parts per billion are explained.
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16
Converting Concentrations
Procedures are given for converting concentration units.
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17
Colligative Properties - Vapor Pressure Lowering
Colligative Properties are defined and listed. Vapor Pressure Lowering and Raoult's Law is introduced. Examples for both cases of Raoult's Law are given.
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18
Freezing Point Depression and Boiling Point Elevation
The two colligative properties of freezing point depression and boiling point elevation are introduced. Discussion and example of using freezing point depression to calculate the molar mass of an unknown is also presented.
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19
Osmosis and Osmotic Pressure
Discussion of osmosis and Osmotic pressure with examples in everyday life.
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20
Colligative Properties of Ionic Solids
The effect of Ionic solutes instead of molecular solutes on colligative properties is discussed. The Van't Hoff factor is introduced and defined.
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21
Chemical Reaction Rates
Rates of chemical reactions are introduced and discussion of how they can be expressed.
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22
Factors Affecting Reaction Rates
The five factors affecting the rate of a chemical reaction are presented with examples of each.
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23
The Rate Law
The rate law for chemical reactions is introduced with interpretation for reactions of different orders with respect to each reactant.
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24
Determining Rate Laws
The method for determining the rate law for a given reaction is explained and applied to several examples.
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25
Reaction Order and Rate Constant Units
A method is explained on how to determine the correct rate constant units from the rate law for a chemical reaction.
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26
Integrated Rate Law - 1st Order Reactions
The integrated rate law is defined and the equation is given for 1st order reactions. An example calculation is given.
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27
Half-Life of 1st Order Reactions
Half-Life is defined and the equation for 1st order reactions is derived. An example is given.
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28
Integrated Rate Law - 2nd Order Reactions
The integrated rate law equation for 2nd order reactions is given and explained along with the Half-Life equation. A problem is solved using both equations.
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29
Integrated Rate Law - Zeroth Order Reactions
The zeroth order integrated rate law and Half-Life equations are given and explained.
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30
Collision Theory
In addition to collisions occurring between the reactant particles for a reaction to occur, other necessary requirements are discussed in this lecture.
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31
Activation Energies
The Arrhenius equation is explained with respect to Activation Energy and used to calculate the activation energy of a given reaction.
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32
Reaction Mechanisms
Reaction Mechanisms are defined as well as elementary reactions that make them up. Rate Laws for overall reactions are determined from reaction mechanisms when either the first or second step of the mechanism is the slow, rate determining step.
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33
Catalysts
Catalysts are defined and the distinction is made between homogeneous and heterogeneous catalysts. Examples of both types are given.
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34
Fundamental Equilibrium Concepts
Chemical Equilibrium is introduced in this lecture and the two requirements for dynamic chemical equilibrium is discussed.
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35
Equilibrium Constants
A procedure is shown to write the equilibrium constant equation. Methods are shown for calculating the numerical value of K when reactions are reversed and when they are added. The effect of changing the coefficients of the balanced chemical equation on the numerical value of K is given.
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36
Significance of the Equilibrium Constant
In this lecture the significance of the numerical value of the equilibrium constant is explained.
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37
Homogeneous Equilibrium
Detailed discussion of homogeneous equilibrium is covered in this lecture including the equilibrium constant equation expressed in terms of the partial pressures of reactant and products. An equation is derived which allows the calculation of Kp given KC. An example of this type of calculation is given.
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38
Heterogeneous Equilibrium
The method for writing the equilibrium constant equation for a heterogeneous equilibrium system is shown for both Kc and Kp. Also, the correct procedure for calculating delta n for these systems is given.
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39
Shifting Equilibria: Le Chatalier's Principle
Le Chatalier's principle is introduced and used to show how a reaction will shift to establish a new equilibrium position when stressed by a change in concentration, volume or temperature.
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40
Equilibrium Calculations - Calculating K
In this lecture the method for calculating the numerical value of K from equilibrium concentrations is explained.
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41
Equilibrium Calculations - Calculating Concentrations
In this lecture the method for calculating the reactant and product equilibrium concentrations given the value for K is explained.
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42
Bronsted-Lowry Acids and Bases
Definitions of acids and Bases are given. Conjugate Acid-Base pairs are determined from reactions. How to identify an acid and base by their chemical formula is explained.
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43
Auto-Ionization of Water
The Auto-Ionization reaction of water is explained, the equilibrium constant equation for that reaction is given, the equilibrium concentrations of the hydronium and hydroxide ions are calculated and several examples are given.
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44
pH and pOH
The shorthand notation of pH and pOH is introduced. Methods are given for converting between pH, pOH and hydronium ion concentration. pH and pOH values for acidic, basic and neutral solutions are given. Several examples are shown.
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45
Relative Strength of Acids and Bases
Strength of acids and Bases is determined by degree of ionization in aqueous solution. The relationship between strength of acid and it's conjugate base is given.
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46
Ionization of Weak Acids and Bases
The equilibrium constant equation for weak acids and bases is given. pKa and pKb terms are defined. Methods for determining weak acid and base strength based on Ka, Kb, pKa and pKb values are given.
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47
Determining Ka and Kb Values
Ka and Kb values are calculated using pH or % ionization.
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48
pH of Strong Acid-Base Solutions
The method for calculating the pH of strong acids and Bases is shown. An example for each is given.
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49
pH of Weak Acid-Base Solutions
A method for calculating the pH of weak acid and weak base aqueous solutions is shown. An example of each is given.
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50
Effect of Molecular Structure on Acid Strength
The Criteria for determining the strength of binary and oxoacids are explained in this lecture.
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51
Hydrolysis of Salt Solutions
A method is shown for determining whether a salt is neutral, acidic or basic. An example of calculating the pH of a basic salt solution is given.
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52
Ionization of Hydrated Metal Ions
The acidic properties of transitional and post-transitional metals is explained.
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53
Polyprotic Acids
The ionization of polyprotic acids is explained. The calculation of the pH of polyprotic acids is shown as well as the calculation of the pH for a salt solution of a polyprotic acid.
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54
Buffer Solutions
Buffer solutions are defined and described. Three ways of preparing a buffer solution are given. Buffer capacity is defined.
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55
Calculating the pH of buffer solutions
The Henderson-Hasselbalch equation is derived and used to calculate the pH of a buffer solution. pH limits for buffer solutions based on weak acid pKa values is explained. An example is given showing how to prepare a buffer solution to a specific pH.
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56
Calculating Change in pH of Buffer Solutions
A procedure is given for calculating the change in pH of a buffer solution if an acid or base is added.
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57
Acid-Base Titrations
Titration is defined and titration curves are presented for three different types of Acid-Base titrations: strong acid with strong base, strong acid with a weak base and a weak acid with a strong base.
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58
Precipitation and Dissolution
The equilibrium reactions for slightly soluble salts are introduced and the solubility product constant equation is discussed.
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59
Determining Ksp from Solubilities
The method for calculating Ksp values from the solubility of a salt is explained.
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60
Determining Molar Solubilities from Ksp
The method for calculating the molar solubility of a slightly soluble salt is explained.
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61
Predicting Precipitation
Predicting whether or not a precipitate will form when two solutions are combined is explained by calculating the reaction quotient, Q, and comparing its value to Ksp.
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62
Common Ion Effect
The common ion effect is explained and a calculation is done to show its effect on the solubility of a slightly soluble salt.
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63
Lewis Acids and Bases
Lewis acids and bases are defined with examples given. The application of Lewis acids and bases to complex ion formation is explained. The increase in solubility of slightly soluble salts with the addition of a ligand to the system is explained and an example calculation is done.
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64
Spontaneity
A spontaneous process is defined with several examples given. Temperature was shown to be a determining factor for some spontaneous processes. It was shown that enthalpy alone is not a predictor of spontaneity.
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65
Entropy
Entropy is defined and the factors that will cause a change in entropy for any process are listed with several examples given.
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66
Second Law of Thermodynamics
The second law of thermodynamics is introduced and explained.
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67
Third Law of Thermodynamics
The third law of thermodynamics is defined and a method for calculating the change in entropy for a chemical reaction is given.
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68
Gibbs Free Energy
The details of using the Gibbs Free Energy equation is given and it is explained how a change in temperature can change the sign of delta G.
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69
Calculating delta G from delta H and delta S
Delta G is calculated for a chemical reaction using the Gibbs Free Energy equation.
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70
Calculating Delta G from Gibbs Free Energy of Formation
Gibbs free energy of formation is defined and used to calculate delta G for a chemical reaction.
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71
Free Energy and Equilibrium
In this lecture we learn how to calculate the boiling or freezing point of a substance using the Gibbs Free Energy equation.
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72
Equilibrium Constant and Delta G
The process for calculating delta G at non-standard conditions is given. The relationship between K and delta G is explained.
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73
Galvanic Cells
Electrochemistry is defined. A quick review of oxidation and reduction is given. Galvanic cells are defined and one is constructed using the zinc + copper(II) sulfate redox reaction.
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74
Standard Cell Notation
The method for writing the standard cell notation for a Galvanic cell is shown. Several variations of the overall galvanic cell chemical equation are used as examples.
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75
Standard Reduction Potentials
Standard reduction potentials are defined and used to determine whether a particular chemical reaction can be used to make a Galvanic cell.
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76
Cell Reactions, E-Zero and Delta G
An equation is derived that allows us to calculate delta G given E-Zero or vice versa.
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77
The Nernst Equation
The Nernst equation is derived and used to calculate cell voltage at non-standard conditions.
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78
Batteries and Fuel Cells
Examples of single-use and rechargeable batteries are given along with a discussion of fuel cells.
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79
Corrosion
The corrosion process is described and the chemistry of sacrificial acidic protection is explained.
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80
Electrolytic Cells
Electrolytic cells are described and two examples are given. The quantitative aspect of electrolysis are explained with example calculations.
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