General Chemistry 3

General Chemistry 3 - Chemistry Coach

In-depth study of acids and bases, chemical equilibrium, solubility, chemical thermodynamics, electrochemistry and the chemistry of the transition metals. The main chemical reactivities are studied: titrations, precipitations, oxidation-reduction and electrochemical reactions. Emphasis on chemical calculations (important formula, strategy and examples).
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Concepts
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Exams
Acids and bases are studied in this chapter: Arrhenius, Brønsted-Lowry, Lewis acids and bases, dissociation of water, ion-product constant, definition of pH and pOH, acid and base strength, pH calculations, acid and base ionization constants, percent ionization, conjugate acid-base pairs, diprotic and polyprotic acids.
Acid-Base Concepts Dissociation of Water The pH Scale Acid and Base Strength Acid Ionization Constants Conjugate Acid-Base Pairs Calculating pH from Ka Diprotic and Polyprotic Acids Base Ionization Constants
Buffer solutions and titrations are studied in this chapter: Henderson-Hasselbach equation, buffer solutions and indicators, strong acid - strong base and weak acid - strong base titrations
Neutralization Reactions The Common-Ion Effect Buffer Solutions Acid-Base Indicators Strong Acid-Strong Base Titration Weak Acid – Strong Base Titration
Solubility and precipitation reactions are studied in this chapter: solubility, molar solubility, solubility product constant, calculations of solubility, precipitation of ionic compounds, reaction quotient, factors affecting solubility, common ion effect, fractional precipitation, qualitative analysis.
Solubility Equilibria Calculations of Solubility Precipitation of Ionic Compounds Factors Affecting Solubility Fractional Precipitation Qualitative Analysis
This chapter explores the concepts of entropy, free energy, and equilibrium, covering: spontaneous processes, entropy and Boltzmann’s equation, entropy changes, standard molar entropy, standard entropy of reaction, the first, second, and third laws of thermodynamics, Gibbs free energy, Gibbs free energy change and spontaneity, standard free energy changes, standard free energies of formation and reaction, free energy and chemical equilibrium.
Spontaneous Processes Entropy Entropy Changes Standard Entropies Entropy Changes in the Universe Free Energy and Reaction Spontaneity Standard Free Energy Changes Free Energy and Chemical Equilibrium
Oxidation-reduction reactions are studied in this chapter: oxidation states, redox reactions and oxidizing-reducing agents, half reactions, steps to balance equations under acidic and basic conditions, corrosion
Oxidation States Oxidation-Reduction Reactions Half Reactions Balancing Equations for Oxidation-Reduction Reactions Corrosion
This chapter explores electrochemistry, including electric energy and charge, galvanic cells and cell diagrams, standard reduction potentials, the standard hydrogen electrode, standard cell potential, redox reaction spontaneity, the Nernst equation, batteries, electrolysis, and corrosion.
Electric Energy and Charge Galvanic Cells Cell Diagrams Standard Reduction Potentials Redox Reaction Spontaneity The Nernst Equation Batteries Electrolysis Corrosion
The chemistry of the transition metals is studied in this chapter: d-block transition metal series, transition metal complexes and nomenclature, isomer cis and trans, d-orbital splittings, electronic configurations of transition metal ions, low-spin and high-spin configuration
d-Block Transition Metal Series Transition Metal Complexes Nomenclature of Transition Metal Complexes Isomers d-Orbital Splittings Electronic Configurations
This chapter is an introduction to organic chemistry and covers: the unique nature of carbon, ionic and covalent bonds, functional groups, basic IUPAC nomenclature, representation of organic molecules, resonance forms, isomerism, chirality and optical isomers, organic reactions.
The Unique Nature of Carbon Bonding in Organic Chemistry Functional Groups IUPAC Nomenclature Representing Organic Molecules Resonance Forms Isomerism Organic Reactions
Midterm 1 includes 5 questions and it covers General Chemistry 1, General Chemistry 2 and Chapters 1, 2 and 3 of General Chemistry 3. At the end of the test you can see the answers and determine whether you have solved the questions. You have 1 hour to resolve Midterm 1.
Questions
60 Minutes
Midterm 2 includes 5 questions and it covers General Chemistry 1, General Chemistry 2 and chapters 1 to 6 of General Chemistry 3 (mainly chapters 4, 5 and 6). At the end of the test you can see the answers and determine whether you have solved the questions. You have 1 hour to resolve Midterm 2.
Questions
60 Minutes
Final Exam includes 10 questions and it covers all chapters of General Chemistry 1, 2 and 3. At the end of the test you can see the answers and determine whether you have solved the questions. You have 2 hours to resolve Final Exam.
Questions
120 Minutes