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General Chemistry Study Notes: Aqueous Equilibria, Thermodynamics, Electrochemistry, Main Group & Transition Elements

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Acids Introduction

  • Guided course
    Acid Structure and Types
    02:29
  • Guided course
    Acid Characteristics
    02:59
  • Guided course
    Acid Characteristics Example
    01:23

Bases Introduction

  • Guided course
    Strong Bases Example
    01:12
  • Guided course
    Base Properties
    01:57
  • Guided course
    Base Structure Example
    01:16

Ka and Kb

  • Guided course
    Ka and Kb Example
    01:31
  • Guided course
    Characteristics of Ka and Kb
    03:50
  • Guided course
    Ka and Kb Relationship
    03:01

The pH Scale

  • Guided course
    pH Calculation Example
    02:15
  • Guided course
    Least Acidic Solution Example
    00:48
  • Guided course
    Additional pH and pOH Calculations
    00:58

Intro to Buffers

  • Guided course
    Buffer Solution Example
    02:41
  • Guided course
    Buffer Capacity
    00:45
  • Guided course
    Buffer Creation Methods
    03:04

Henderson-Hasselbalch Equation

  • Guided course
    Buffer Range Calculation
    02:47
  • Guided course
    Buffering Range Example
    01:22
  • Guided course
    Henderson-Hasselbalch Equation
    02:40

Intro to Acid-Base Titration Curves

  • Guided course
    Equivalence Point Example
    01:35
  • Guided course
    Acid-Base Titration Curve Example
    01:35
  • Guided course
    Equivalence Point in Titration
    03:06

Spontaneous vs Nonspontaneous Reactions

  • Guided course
    Spontaneity of Processes Example
    03:05
  • Guided course
    Spontaneity of Processes
    04:20

Entropy

  • Guided course
    Second Law of Thermodynamics Example
    00:48
  • Guided course
    Entropy and Physical Changes
    02:35
  • Guided course
    Standard Molar Entropy Example
    01:17

Gibbs Free Energy

  • Guided course
    Spontaneity of Reactions
    03:38
  • Guided course
    ΔG and Spontaneity Example
    01:23
  • Guided course
    Spontaneity and Temperature Example
    02:42

Gibbs Free Energy Calculations

  • Guided course
    The Gibbs Free Energy Formula
    00:44
  • Guided course
    Standard Gibbs Free Energy and Temperature
    00:32
  • Guided course
    The Gibbs Free Energy Formula Example
    01:29

Gibbs Free Energy And Equilibrium

  • Guided course
    ∆G° and K Example
    01:13
  • Guided course
    ∆G° and K
    01:19
  • Guided course
    ∆G, ∆G° and Q
    01:03

Intro to Electrochemical Cells

  • Guided course
    Electrochemical Cells Example
    01:01
  • Guided course
    Cell Potential and Spontaneity
    02:32
  • Guided course
    Electrochemical Cells
    02:46

Galvanic Cell

  • Guided course
    Galvanic Cell Components
    03:55
  • Guided course
    Galvanic Cell and Spontaneity
    03:04
  • Guided course
    Galvanic Cell Components Example
    02:22

Electrolytic Cell

  • Guided course
    Electrolytic Cell Example
    00:45
  • Guided course
    The Electrolytic Cell
    01:21
  • Guided course
    Electrolytic Cells and Spontaneity Example
    01:24

Cell Potential: Standard

  • Guided course
    Standard Cell Potential
    01:27
  • Guided course
    Standard Cell Potential and Spontaneity
    01:46
  • Guided course
    Standard Cell Potential Example
    01:34

Cell Potential: The Nernst Equation

  • Guided course
    The Reaction Quotient
    01:01
  • Guided course
    The Nernst Equation Example
    04:38
  • Guided course
    The Nernst Equation
    01:17

Cell Potential and Gibbs Free Energy

  • Guided course
    Faraday's Constant in Electrochemistry Example
    02:11
  • Guided course
    Cell Potential and Gibbs Free Energy Example
    03:18
  • Guided course
    Faraday's Constant in Electrochemistry
    01:40

Cell Potential and Equilibrium

  • Guided course
    Cell Potential and Equilibrium
    02:38
  • Guided course
    Cell Potential and Equilibrium Example
    02:17

Cell Potential: G and K

  • Guided course
    Relationship between ∆E°, ∆G°, and K
    02:43
  • Guided course
    Relationship between ∆E°, ∆G°, and K Example
    02:57

Cell Notation

  • Guided course
    Cell Notation
    06:23
  • Guided course
    Cell Notation Example
    01:49

Main Group Elements: Periodic Trends

  • Guided course
    Main Group Elements: Periodic Trends Example
    00:59
  • Guided course
    Periodic Trends
    01:55

Coordination Complexes

  • Guided course
    Coordination Complexes Example
    00:43
  • Guided course
    Coordination Complexes I and II
    02:28

Ligands

  • Guided course
    Ligands Example
    01:12
  • Guided course
    Ligand Reaction
    01:53
  • Guided course
    Ligands Example
    00:40

Complex Ions

  • Guided course
    Complex Ions Example
    00:57
  • Guided course
    Complex Ion Formation
    02:09

Coordination Complexes

  • Guided course
    Coordination Complexes Example
    00:43
  • Guided course
    Coordination Complexes I and II
    02:28

Classification of Ligands

  • Guided course
    Classification of Ligands Example
    01:42
  • Guided course
    Classification of Ligands Example
    01:48
  • Guided course
    Chelating Agents
    01:21

Coordination Numbers & Geometry

  • Guided course
    Coordination Numbers and Geometry Example
    00:30
  • Guided course
    Coordination Numbers
    00:27
  • Guided course
    Molecular Geometry of Coordination Complexes
    02:40

Naming Coordination Compounds

  • Guided course
    Ligand Naming
    02:03
  • Guided course
    Naming Coordination Compounds Example
    04:11
  • Guided course
    Complex Ion Naming
    01:28

Writing Formulas of Coordination Compounds

  • Guided course
    Writing Formulas of Coordination Compounds Example
    03:37
  • Guided course
    Writing Formulas
    00:46

Isomerism in Coordination Complexes

  • Guided course
    Isomerism in Coordination Complexes Example
    2:14
  • Guided course
    Structural Isomers
    3:22
  • Guided course
    Geometric Isomers
    02:02

Intro to Crystal Field Theory

  • Guided course
    Example
    00:59
  • Guided course
    For tetrahedral complexes, the greatest ligand-metal interactions occur in between the axes.
    02:37
  • Guided course
    For octahedral complexes, the greatest ligand-metal interactions occur on or along the axes.
    02:01

Crystal Field Theory: Octahedral Complexes

  • Guided course
    Example
    00:43
  • Guided course
    The crystal field splitting pattern for octahedral complexes has the d orbitals on or along the axes as having the higher energy.
    03:04

Crystal Field Theory: Tetrahedral Complexes

  • Guided course
    The crystal field splitting pattern for tetrahedral complexes has the d orbitals in between the axes as having the higher energy.
    01:38
  • Guided course
    Example
    01:11

Crystal Field Theory: Square Planar Complexes

  • Guided course
    Square planar complexes show the most complex splitting pattern.
    02:07
  • Guided course
    Example
    01:17

Crystal Field Theory Summary

  • Guided course
    Example
    02:46
  • Guided course
    The greatest ligand-orbital interactions result in the greatest increase in energy.
    03:01

Magnetic Properties of Complex Ions

  • Guided course
    Low-Spin Complexes are associated with large Δ values and High-Spin Complexes are associated with small Δ values.
    04:23
  • Guided course
    Finding tetrahedral and square planar geometries helps to determine the low vs high spin of complexes.
    01:43
  • Guided course
    Example
    02:14

Strong-Field vs Weak-Field Ligands

  • Guided course
    Example
    02:09
  • Guided course
    Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.
    02:40

Magnetic Properties of Complex Ions: Octahedral Complexes

  • Guided course
    For octahedral complexes, Weak-Field Ligands create High-spin complexes and Strong-Field Ligands create Low-spin complexes.
    01:28
  • Guided course
    Example
    02:52