A chemistry course to cover selected topics covered in advanced high school chemistry courses, correlating to the standard topics as established by the American Chemical Society.
Prerequisites: Students should have a background in basic chemistry including nomenclature, reactions, stoichiometry, molarity and thermochemistry.
Advanced Chemistry
von
University of Kentucky
Lehrplan - Was Sie in diesem Kurs lernen werden
Woche
13 Stunden zum Abschließen
Kinetics
The study of chemical kinetics is the study of change over time. It answers questions like:
How fast are reactants consumed?
How fast are products formed?
This unit is dedicated to the exploration of how these questions are answered. We will look at the experimental evidence of how concentration affects these rates.
We will also examine what occurs on the molecular level, especially with respect to the motion of molecules, that affects rates of reactions.
19 Videos (Gesamt 153 min), 2 Lektüren, 1 Quiz
19 Videos
1.02 Comparing Rate of Change for Reactants and Products13m
1.02a Obtaining a Rate Law from Experimental Data Equations4m
1.03 The Rate Law9m
1.04 Obtaining a Rate Law from Experimental Data16m
1.04a Rate Law Calculations8m
1.05 First-Order Kinetics and the Integrated Rate Law
1.05a Graphic 1st Order7m
1.06 First-Order Kinetics and the Half-Life9m
1.07 Second-Order Reactions8m
1.07a Graphics 2nd Order6m
1.08 Collision Theory13m
1.08a Activation Energy3m
1.09 The Arrhenius Equation15m
1.09a Graphic Activation Energy2m
1.10 Reaction Mechanisms12m
1.10a RDS Fast Equilibrium4m
1.10b Rate Determining Step2m
1.11 Catalysis4m
2 Lektüren
Syllabus10m
Kinetics Lecture Notes and Practice Problems10m
1 praktische Übung
Kinetics28m
Woche
23 Stunden zum Abschließen
Chemical Equilibrium
This unit introduces the concept of chemical equilibrium and how it applies to many chemical reactions. The quantitative aspects of equilibrium are explored thoroughly through discussions of the law of mass action as well as the relationship between equilibrium constants with respect to concentrations and pressures of substances. Much of the discussion explores how to solve problems to find either the value of the equilibrium constant or the concentrations of substances at equilibrium. ICE (initial-change-equilibrium) tables are introduced as a problem-solving tool and multiple examples of their use are included.
From a qualitative standpoint, Le Châtelier’s principle is used to explain how various factors affect the equilibrium constant of a reaction along with the concentrations of all species.
16 Videos (Gesamt 115 min), 1 Lektüre, 1 Quiz
16 Videos
2.02 Law of Mass Action7m
2.03 Law of Mass Action for Combined Reactions4m
2.04 Relationship Between Kc and Kp6m
2.04a Relationship Between Kc and Kp2m
2.05 Calculating the Equilibrium Constant13m
2.05a Finding Kc5m
2.06 Reaction Quotient5m
2.06a Predicting Reaction Progress with the Reaction Quotient1m
2.07 Calculating Equilibrium Concentrations12m
2.07a Finding Equilibrium Concentrations, part 14m
2.07b Finding Equilibrium Concentrations, part 23m
2.07c Finding Equilibrium Concentrations, part 34m
2.08 Le Chatelier's Principle Part A9m
2.08a Le Chatelier's Principle Part B19m
2.08b How Changes Shift the Equilibrium5m
1 Lektüre
Chemical Equilibrium Lecture Notes and Practice Problems10m
1 praktische Übung
Chemical Equilibrium26m
Woche
32 Stunden zum Abschließen
Acid-Base Equilibria
The concept of equilibrium is applied to acid and base solutions. To begin, the idea of weak acids and bases is explored along with the equilibrium constants associated with their ionization in water and how the value of the equilibrium constant is associated with the strength of the acid or base. The autoionization of water is discussed and how temperature affects this process. A variety of problem types are covered including calculations of pH, pOH, [OH-], and [H+] for both strong and weak acids and bases.
Aqueous salt solutions are classified as acids and bases and the multi-step ionization of polyprotic acids is discussed. Finally, the concept of Lewis acids and bases is discussed and demonstrated through examples.
14 Videos (Gesamt 101 min), 1 Lektüre, 1 Quiz
14 Videos
3.02 pH and Kw13m
3.02a Finding Kw2m
3.03 Acid Strength6m
3.04 Finding pH10m
3.05 Strong and Weak Bases12m
3.05a Calculating equilibrium concentrations of a weak base, part 12m
3.05b Calculating equilibrium concentrations of a weak base, part 21m
3.06 Ions as Acids and Bases18m
3.06a Acid-base properties of aqueous salts, part 11m
3.06b Acid-base properties of aqueous salts, part 21m
3.06c Acid-base properties of aqueous salts, part 34m
3.07 Types of Acids12m
3.08 Polyprotic Acids4m
1 Lektüre
Acid-Base Equilibria Lecture Notes and Practice Problems10m
1 praktische Übung
Acid-Base Equilibrium38m
Woche
45 Stunden zum Abschließen
Aqueous Equilibria
This unit continues and expands on the theme of equlibria. You will examine buffers, acid/base titrations and the equilibria of insoluble salts.
30 Videos (Gesamt 258 min), 1 Lektüre, 1 Quiz
30 Videos
4.02 pH of Buffer Solutions14m
4.02a Aqueous Equilibria Worked Example 13m
4.03 Buffer Action25m
4.03a Aqueous Equilibria Worked Example 25m
4.03b Aqueous Equilibria Worked Example 35m
4.04 Buffer: Preparation and Capacity8m
4.05 Strong Acid - Strong Base Titration17m
4.06 Titrations Involving Either a Weak Acid or a Weak Base36m
4.06 Part 1 Aqueous Equilibria Worked Example3m
4.06 Part 1.a - Aqueous Equilibria Worked Example4m
4.06 Part 1.b - Aqueous Equilibria Worked Example4m
4.06 Part 1.c - Aqueous Equilibria Worked Example4m
4.06 Part 1.f Aqueous Equilibria Worked Example8m
4.06 Part 1.h Aqueous Equilibria Worked Example3m
4.06 Part 2.a Aqueous Equilibria Worked Example8m
4.06 Part 2.b Aqueous Equilibria Worked Example5m
4.07 Polyprotic Acid Titrations5m
4.08 Indicators10m
4.09 Solubility Equilibria4m
4.10 Molar Solubility and the Solubility Product10m
4.10.a Aqueous Equilibria Worked Example2m
4.11 Molar Solubility and the Common Ion Effect7m
4.11 2.b - Aqueous Equilibria Worked Example4m
4.11 2.c Aqueous Equilibria Worked Example3m
4.12 The Effect of pH on Solubility7m
4.12.b Aqueous Equilibria Worked Example3m
4.12c Aqueous Equilibria Worked Example3m
4.13 Precipitation Reaction and Selective Precipitation15m
4.13a Aqueous Equilibria Worked Example9m
1 Lektüre
Aqueous Equilibria Lecture Notes and Practice Problems10m
1 praktische Übung
Aqueous Equilibria36m
Woche
54 Stunden zum Abschließen
Thermodynamics
The overarching theme of thermodynamics is the prediction of whether a reaction will occur spontaneously under a certain set of conditions. Entropy and Free Energy are defined and utilized for this purpose.
20 Videos (Gesamt 128 min), 1 Lektüre, 2 Quiz
20 Videos
5.01a Enthalpy of Reaction Refresher2m
5.02 Spontaneous vs. Nonspontaneous7m
5.10 Standard versus Nonstandard Free Energy Change15m
5.03 The Second Law of Thermodynamics2m
5.04 Entropy5m
5.05 Entropy of the Universe8m
5.06 Gibbs Free Energy8m
5.06a Gibbs Free Energy Example Problem 15m
5.06b Gibbs Free Energy Example Problem 24m
5.07 The Third Law of Thermodynamics6m
5.08 Calculating Standard Entropy Change6m
5.08a Thermodynamics Worked Example3m
5.09 Calculating Standard Free Energy Change11m
5.09a Thermodynamics Worked Example2m
5.09b Thermodynamics Worked Example2m
5.11 Comparing ∆G° and K18m
5.10a Thermodynamics Worked Example3m
5.10b Thermodynamics Worked Example1m
5.02a Spontaneous vs Nonspontaneous Example Problem1m
1 Lektüre
Thermodynamics Lecture Notes and Practice Problems10m
2 praktische Übungen
Thermodynamics28m
Advanced Chemistry Final Assessment
14%
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Top-Bewertungen
Excellent lecture videos with practice problems that are very helpful in recalling the chemical concepts. Really wish this course could offer at least an SOA so learners can be more motivated.
Excellent course. If you are struggling with high school chem, or need a good foundation for college chem - this course moves you through the concepts and gives you lots of practice problems.
Dozenten
Dr. Allison Soult
LecturerChemistry
Dr. Kim Woodrum
Sr. LecturerChemistry
Über University of Kentucky
The University of Kentucky is the Commonwealth’s flagship, land-grant institution of higher learning. With more than 30,000 students and 16 academic colleges and a graduate school, it is one of only eight universities in America with the full range of professional, medical and liberal arts programs on one contiguous campus.
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