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.
Read more
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.
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.
What's inside
Learning objectives
- All topics covered in a second semester of college chemistry course are contained in this udemy course.
- Each topic is covered is great detail with plenty of examples.
- Course topics include:
- Intermolecular forces
- Properties of liquids
- Phase transitions
- Phase diagrams
- Lattice structure in crystalline solids
- The dissolution process and solutions
- Concentration units
- Colligative properties
- Chemical reaction rates
- Factors affecting rates of reactions
- The rate law
- Integrated rate laws for zeroth, first and second order reactions
- Collision theory
- Reaction mechanisms
- Catalysis
- Chemical equilibria
- Equilibrium constants and reaction quotient
- Le chatelier’s principle
- Equilibrium calculations
- Bronsted-lowry acids and bases
- Ph and poh
- Relative strength of acids and bases
- Hydrolysis of salt solutions
- Polyprotic acids
- Buffer solutions
- Acid-base titrations
- Precipitation and dissolution
- Solubility products
- Lewis acids and bases
- Complex ion equilibrium
- Spontaneity
- Entropy
- The second and third laws of thermodynamics
- Gibbs free energy
- Galvanic cells
- Standard reduction potentials
- The nernst equations
- Batteries and fuel cells
- Corrosion
- Electrolysis
- Show more
- Show less
- All topics covered in a second semester of college chemistry course are contained in this udemy course.
- Each topic is covered is great detail with plenty of examples.
- Course topics include:
- Intermolecular forces
- Properties of liquids
- Phase transitions
- Phase diagrams
- Lattice structure in crystalline solids
- The dissolution process and solutions
- Concentration units
- Colligative properties
- Chemical reaction rates
- Factors affecting rates of reactions
- The rate law
- Integrated rate laws for zeroth, first and second order reactions
- Collision theory
- Reaction mechanisms
- Catalysis
- Chemical equilibria
- Equilibrium constants and reaction quotient
- Le chatelier’s principle
- Equilibrium calculations
- Bronsted-lowry acids and bases
- Ph and poh
- Relative strength of acids and bases
- Hydrolysis of salt solutions
- Polyprotic acids
- Buffer solutions
- Acid-base titrations
- Precipitation and dissolution
- Solubility products
- Lewis acids and bases
- Complex ion equilibrium
- Spontaneity
- Entropy
- The second and third laws of thermodynamics
- Gibbs free energy
- Galvanic cells
- Standard reduction potentials
- The nernst equations
- Batteries and fuel cells
- Corrosion
- Electrolysis
- Show more
- Show less
Syllabus
Liquids and Solids
Each of the four Intermolecular Forces is identified and defined. Example compounds are given for each force.
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.
Read more
Syllabus
Each of the four Intermolecular Forces is identified and defined. Example compounds are given for each force.
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.
The properties of liquids including viscosity, surface tension, adhesive forces and capillary action are described.
Intermolecular Forces are used to explain the phase transitions of matter including freezing, melting, evaporation, condensation, sublimation and deposition.
Vapor Pressure and boiling points are defined in terms of Intermolecular forces. The relationship between the two is explained.
Derivation of the Claussius-Clapeyron Equation used to determine heat of vaporization.
Heating and cooling curves are explained and an example calculation is done.
Phase Diagrams are defined and constructed for water and carbon dioxide.
Types of Solids are discussed and properties of crystalline solids are given.
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.
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.
Electrolytes and Non-Electrolytes are defined with examples of each given.
Solubility is defined and the solubility of solid solutes in liquid solvents as a function of temperature is discussed.
Application of Henry's Law which governs the solubility of Gases in Liquids.
The concentration units of mass percent, mole fraction, molarity, molarity, parts per million and parts per billion are explained.
Procedures are given for converting concentration units.
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.
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.
Discussion of osmosis and Osmotic pressure with examples in everyday life.
The effect of Ionic solutes instead of molecular solutes on colligative properties is discussed. The Van't Hoff factor is introduced and defined.
Rates of chemical reactions are introduced and discussion of how they can be expressed.
The five factors affecting the rate of a chemical reaction are presented with examples of each.
The rate law for chemical reactions is introduced with interpretation for reactions of different orders with respect to each reactant.
The method for determining the rate law for a given reaction is explained and applied to several examples.
A method is explained on how to determine the correct rate constant units from the rate law for a chemical reaction.
The integrated rate law is defined and the equation is given for 1st order reactions. An example calculation is given.
Half-Life is defined and the equation for 1st order reactions is derived. An example is given.
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.
The zeroth order integrated rate law and Half-Life equations are given and explained.
In addition to collisions occurring between the reactant particles for a reaction to occur, other necessary requirements are discussed in this lecture.
The Arrhenius equation is explained with respect to Activation Energy and used to calculate the activation energy of a given reaction.
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.
Catalysts are defined and the distinction is made between homogeneous and heterogeneous catalysts. Examples of both types are given.
Chemical Equilibrium is introduced in this lecture and the two requirements for dynamic chemical equilibrium is discussed.
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.
In this lecture the significance of the numerical value of the equilibrium constant is explained.
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.
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.
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.
In this lecture the method for calculating the numerical value of K from equilibrium concentrations is explained.
In this lecture the method for calculating the reactant and product equilibrium concentrations given the value for K is explained.
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.
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.
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.
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.
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.
Ka and Kb values are calculated using pH or % ionization.
The method for calculating the pH of strong acids and Bases is shown. An example for each is given.
A method for calculating the pH of weak acid and weak base aqueous solutions is shown. An example of each is given.
The Criteria for determining the strength of binary and oxoacids are explained in this lecture.
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.
The acidic properties of transitional and post-transitional metals is explained.
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.
Buffer solutions are defined and described. Three ways of preparing a buffer solution are given. Buffer capacity is defined.
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.
A procedure is given for calculating the change in pH of a buffer solution if an acid or base is added.
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.
The equilibrium reactions for slightly soluble salts are introduced and the solubility product constant equation is discussed.
The method for calculating Ksp values from the solubility of a salt is explained.
The method for calculating the molar solubility of a slightly soluble salt is explained.
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.
The common ion effect is explained and a calculation is done to show its effect on the solubility of a slightly soluble salt.
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.
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.
Entropy is defined and the factors that will cause a change in entropy for any process are listed with several examples given.
The second law of thermodynamics is introduced and explained.
The third law of thermodynamics is defined and a method for calculating the change in entropy for a chemical reaction is given.
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.
Delta G is calculated for a chemical reaction using the Gibbs Free Energy equation.
Gibbs free energy of formation is defined and used to calculate delta G for a chemical reaction.
In this lecture we learn how to calculate the boiling or freezing point of a substance using the Gibbs Free Energy equation.
The process for calculating delta G at non-standard conditions is given. The relationship between K and delta G is explained.
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.
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.
Standard reduction potentials are defined and used to determine whether a particular chemical reaction can be used to make a Galvanic cell.
An equation is derived that allows us to calculate delta G given E-Zero or vice versa.
The Nernst equation is derived and used to calculate cell voltage at non-standard conditions.
Examples of single-use and rechargeable batteries are given along with a discussion of fuel cells.
The corrosion process is described and the chemistry of sacrificial acidic protection is explained.
Electrolytic cells are described and two examples are given. The quantitative aspect of electrolysis are explained with example calculations.
Traffic lights
Save this course
Save
Reviews summary
Comprehensive college general chemistry ii
Content aligns well with college syllabus.
Plenty of worked examples demonstrating concepts.
Instructor explains complex topics clearly.
Assignments and answer keys are essential.
Activities
Review General Chemistry I Concepts
Show steps
Reinforce foundational knowledge from General Chemistry I to better understand the concepts covered in General Chemistry II.
Browse courses on
General Chemistry
Show steps
-
Review your notes and textbook from General Chemistry I.
-
Work through practice problems on stoichiometry, thermochemistry, and atomic structure.
-
Focus on areas where you feel less confident.
Read 'Chemistry: The Central Science'
Show steps
Supplement course materials with a comprehensive textbook to gain a deeper understanding of chemical principles.
View
Chemistry
on Amazon
Show steps
-
Read the chapters relevant to the course syllabus.
-
Work through the example problems in the book.
-
Use the book as a reference when you encounter difficult concepts.
Practice Equilibrium Calculations
Show steps
Sharpen your skills in solving equilibrium problems, a crucial aspect of General Chemistry II.
Browse courses on
Chemical Equilibrium
Show steps
-
Find practice problems on calculating equilibrium constants and concentrations.
-
Work through the problems step-by-step, showing all your work.
-
Check your answers against the solutions and identify any errors.
Four other activities
Expand to see all activities and additional details
Show all seven activities
Create Flashcards for Key Concepts
Show steps
Reinforce your understanding of key terms and concepts by creating flashcards.
Show steps
-
Identify the most important terms and concepts from each lecture.
-
Write the term or concept on one side of the flashcard and the definition or explanation on the other side.
-
Review the flashcards regularly to reinforce your memory.
Study 'Physical Chemistry' by Atkins
Show steps
Expand your knowledge of thermodynamics and kinetics with a more advanced physical chemistry textbook.
View
ATKINS PHYSICAL CHEMISTRY 12E SE P
on Amazon
Show steps
-
Read the chapters on thermodynamics and kinetics.
-
Focus on the mathematical derivations and theoretical explanations.
-
Compare the treatment of these topics in this book to the treatment in the course materials.
Tutor Other Students
Show steps
Solidify your understanding of the material by helping other students who are struggling.
Show steps
-
Offer to tutor other students in the course.
-
Prepare for tutoring sessions by reviewing the material beforehand.
-
Explain the concepts in your own words and answer any questions that the students have.
Create a Thermodynamics Cheat Sheet
Show steps
Consolidate your knowledge of thermodynamics by creating a cheat sheet with key equations and concepts.
Browse courses on
Thermodynamics
Show steps
-
Gather all the important equations and concepts from the thermodynamics section of the course.
-
Organize the information in a clear and concise manner.
-
Include examples of how to use the equations.
Review General Chemistry I Concepts
Show steps
Reinforce foundational knowledge from General Chemistry I to better understand the concepts covered in General Chemistry II.
Browse courses on
General Chemistry
Show steps
- Review your notes and textbook from General Chemistry I.
- Work through practice problems on stoichiometry, thermochemistry, and atomic structure.
- Focus on areas where you feel less confident.
Read 'Chemistry: The Central Science'
Show steps
Supplement course materials with a comprehensive textbook to gain a deeper understanding of chemical principles.
View
Chemistry
on Amazon
Show steps
- Read the chapters relevant to the course syllabus.
- Work through the example problems in the book.
- Use the book as a reference when you encounter difficult concepts.
Practice Equilibrium Calculations
Show steps
Sharpen your skills in solving equilibrium problems, a crucial aspect of General Chemistry II.
Browse courses on
Chemical Equilibrium
Show steps
- Find practice problems on calculating equilibrium constants and concentrations.
- Work through the problems step-by-step, showing all your work.
- Check your answers against the solutions and identify any errors.
Create Flashcards for Key Concepts
Show steps
Reinforce your understanding of key terms and concepts by creating flashcards.
Show steps
- Identify the most important terms and concepts from each lecture.
- Write the term or concept on one side of the flashcard and the definition or explanation on the other side.
- Review the flashcards regularly to reinforce your memory.
Study 'Physical Chemistry' by Atkins
Show steps
Expand your knowledge of thermodynamics and kinetics with a more advanced physical chemistry textbook.
View
ATKINS PHYSICAL CHEMISTRY 12E SE P
on Amazon
Show steps
- Read the chapters on thermodynamics and kinetics.
- Focus on the mathematical derivations and theoretical explanations.
- Compare the treatment of these topics in this book to the treatment in the course materials.
Tutor Other Students
Show steps
Solidify your understanding of the material by helping other students who are struggling.
Show steps
- Offer to tutor other students in the course.
- Prepare for tutoring sessions by reviewing the material beforehand.
- Explain the concepts in your own words and answer any questions that the students have.
Create a Thermodynamics Cheat Sheet
Show steps
Consolidate your knowledge of thermodynamics by creating a cheat sheet with key equations and concepts.
Browse courses on
Thermodynamics
Show steps
- Gather all the important equations and concepts from the thermodynamics section of the course.
- Organize the information in a clear and concise manner.
- Include examples of how to use the equations.
Career center
Analytical Chemist
Laboratory Technician
Chemical Engineer
Environmental Chemist
Materials Scientist
Process Engineer
Quality Control Analyst
Forensic Scientist
Research Assistant
Biochemistry Technician
Formulation Scientist
Toxicologist
Environmental Technician
Science Teacher
Chemical Sales Representative
Reading list
Save
Share
Similar courses
OpenCourser helps millions of learners each year. People visit us to learn workspace skills, ace their exams, and nurture their curiosity.
Our extensive catalog contains over 50,000 courses and twice as many books. Browse by search, by topic, or even by career interests. We'll match you to the right resources quickly.
Find this site helpful? Tell a friend about us.
We're supported by our community of learners. When you purchase or subscribe to courses and programs or purchase books, we may earn a commission from our partners.
Your purchases help us maintain our catalog and keep our servers humming without ads.
Thank you for supporting OpenCourser.
