Course Content
Atomic Structure
0/14
Notes and Worksheets
Lesson 1 | Electron Orbitals
35:21
Lesson 2 | Orbitals, Shells & Subshells
38:41
Lesson 3 | Spin Pair Repulsion and Aufbau
00:00
Lesson 4 | Writing Electronic Configuration
41:00
Lesson 5 | Past Paper Questions on Atomic Structure
00:00
Lesson 6 | Different ways to write E-configuration | Two Special Cases
41:32
Lesson 7 | Size of Atoms and Ions | Past Paper Practice
00:00
Lesson 8 | Past Paper Practice | Electronic Configuration
00:00
Lesson 9 | Ionization Energy Factors
37:30
Lesson 10 | Successive Ionization Energies | Past Paper Questions
37:30
Lesson 11 | 1st Ionization Energy | Down the Group | Across the Period
43:14
Lesson 12 | Past Papers on Ionization Energies
00:00
Lesson 13 | Past Papers on Ionization Energies
00:00
Chemical Bonding
1 - Ionic, Covalent, Metallic, Giant Covalent 2 - Sigma and Pi Covalent Bonds 3 - Coordinate Bonds 4 - Shapes of Molecules 5 - Intermolecular Forces
0/16
AS Chemical Bonding | Notes and Workbook
Complete Crash Course for Quick Revision
03:39:52
1 | Electronegativity and Bonding
38:03
2 | Ionic Bonding & Electronegativity | Properties of Ionic Lattices
34:53
3 | Covalent Bonds | Dot & Cross Diagrams | VSEPR | Shapes of Molecules
36:15
3 | VSEPR | Shapes of Molecules
38:34
4 | Shapes of Molecules | Past Papers Solved
40:10
5 | Dative Covalent (Coordinate) Bond
30:34
6 | Intermolecular Forces | Permanent Dipoles
37:37
7 | Intermolecular Forces | Hydrogen Bonds
36:57
8 | Intermolecular Forces | Instantaneous Dipole – Induced Dipole (Van der Waals)
41:28
9 | Intermolecular Forces | Past Papers Solved
19:02
10 | Sigma and Pi Bonding
40:49
11 | Sigma and Pi Bonding | Past Papers Solved
03:08
12 | Hybridization | sp3 sp2 sp
00:00
13 | Hybridization | sp3 sp2 sp
41:42
Energetics
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Chemical Energetics | Notes and Worksheets
1 | Introduction
40:43
2 | Catalysts | Bond Energy Calculations
41:16
3 | Bond Energy | Past Paper Solved
44:28
4 | Definitions of Enthalpy Change of Reaction, Formation & Combustion
00:00
5 | Energetics Definitions | Enthalpy of Neutralization | Hess Law Intro
43:23
6 | Drawing Hess law with Past Paper Questions
41:04
7 | Finding Enthalpy Changes using Hess law Formulas
38:03
8 | Q= mcΔt questions
30:14
Inorganic Chemistry
Physical and Chemical properties of the following topics will be covered in these lectures: Chemical Periodicity, Group 2, Group 17 and Nitrogen and Sulfur
0/10
Notes and Worksheets
1 | Chemical Periodicity | Physical Properties
38:40
2 | Chemical Periodicity | Oxides and Chlorides
44:15
3 | Chemical Periodicity | Chlorides | Flame Tests | Past Paper Questions
44:35
4 | Group 2 | Metals | Reactivity | Decomposition | Uses
42:39
5 | Group 17 | Physical Properties | Reducing and Oxidizing Agents
44:47
6 | Group 17 | Hydrogen Halides | Redox | Uses | Tests
47:21
7 | Nitrogen & Sulfur | Haber Process | Contact Process
39:57
8 | Past Paper Questions on Inorganic Chemistry
47:04
9 | Past Paper Questions on Inorganic Chemistry
42:33
Infrared spectroscopy
0/1
Interpreting Infrared Spectroscopy
15:45
Mass spectrometry
0/2
Lesson 1 | Mass Spectroscopy | Past Paper Questions
01:05:11
Lesson 2 | Mass Spectroscopy | Find Relative Atomic Mass | Past Paper Questions
Organic Chemistry
0/24
Organic Chemistry | Notes & Workbook
AS 9701 Organic Chemistry Part 0 | Introduction | Formulas
31:34
AS 9701 Organic Chemistry Part 1 | Structural Formulas, Skeletal Formulas, Condensed Formulas
42:37
AS 9701 Organic Chemistry Part 2 | Formulas and IUPAC Nomenclature for Organic Chemistry
01:25:22
AS 9701 Organic Chemistry Part 3 | IUPAC Nomenclature & Introduction to Isomers
42:31
AS 9701 Organic Chemistry Part 4 | Structural and Stereo Isomers
01:32:03
AS 9701 Organic Chemistry Part 5 | Structural and Stereo Isomers | Optical Isomers
39:16
AS 9701 Organic Chemistry Part 6 | Isomers and Past Paper Questions
42:07
AS 9701 Organic Chemistry Part 7 | Introduction to Alkanes and Mechanisms
36:22
AS 9701 Organic Chemistry Part 8 | Alkanes | Free Radical Substitution
37:59
AS 9701 Organic Chemistry Part 9 | Alkenes | Cracking | Electrophilic Addition
32:35
AS 9701 Organic Chemistry Part 10 | Alkenes | Electrophilic Addition | Markovnikov’s Rule
44:41
AS 9701 Organic Chemistry Part 11 | Alkenes | Electrophilic Addition | Mild & Strong Oxidation
29:36
AS 9701 Organic Chemistry Part 12 | Alkanes & Alkenes | Past Paper Questions
38:31
AS 9701 Organic Chemistry Part 13 | Halogenoalkanes | Nucleophilic Substitution
32:14
AS 9701 Organic Chemistry Part 14 | Halogenoalkanes | Nucleophilic Substitution
34:03
AS 9701 Organic Chemistry Part 15 | Halogenoalkanes | Elimination
32:59
AS 9701 Organic Chemistry Part 16 | Alcohols | Oxidation of Primary, Secondary, Tertiary Alcohols
35:35
AS 9701 Organic Chemistry Part 17 | Alcohols | Reduction of Carboxylic Acids, Aldehydes, Ketones
35:40
AS 9701 Organic Chemistry Part 18 | Carbonyl | Aldehyde & Ketones | Nucleophilic Addition | 2,4 DNPH
35:49
AS 9701 Organic Chemistry Part 19 | Carboxylic Acids
36:40
AS 9701 Organic Chemistry Part 20 | Past Paper Questions
34:32
AS 9701 Organic Chemistry Part 21 | Past Paper Questions
28:42
AS 9701 Organic Chemistry Part 22 | Past Paper Questions
38:43
AS Organic Chemistry Past Papers (200 Questions Solved)
0/1
AS Organic Past Papers Practice
36:22
Chemical Equilibria
Chemical Equilibria Outline Introduction to Chemical Equilibria Definition of chemical equilibrium Characteristics of a system in equilibrium Dynamic nature of equilibrium The Equilibrium Constant (Kc) Derivation and expression of the equilibrium constant Calculation of Kc for homogeneous and heterogeneous equilibria Units of Kc and their significance Factors Affecting Equilibrium Le Chatelier's Principle Effect of changes in concentration, temperature, and pressure on equilibrium Effect of catalysts on equilibrium position Applications of Equilibrium Principles Industrial processes (Haber Process, Contact Process) Biological systems and biochemical equilibria Environmental equilibria (acid rain, ocean acidification) Calculation of Equilibrium Concentrations Using the ICE (Initial, Change, Equilibrium) table method Solving equilibrium problems involving Kc Relationship Between Kp and Kc Definition of Kp (equilibrium constant for gaseous systems) Conversion between Kc and Kp Impact of partial pressure on equilibrium
0/5
AS Chemistry | Chemical Equilibria Part 1 | Introduction to Equilibria
45:43
AS Chemistry | Chemical Equilibria Part 2 | Le Chatelier Principle – Past Papers Solved
42:27
AS Chemistry | Chemical Equilibria Part 3 | Equilibrium Constant Kc
41:18
AS Chemistry | Chemical Equilibria Part 4 | Equilibrium Constant Kc | Past Papers Solved
39:34
AS Chemistry | Chemical Equilibria Part 5 | Equilibrium Constant Kp
00:10
AS Chemistry | Complete Video Course | Notes | Worksheet
About Lesson

Chemical Equilibria Overview

In chemistry, a chemical equilibrium is a state in which the concentrations of reactants and products remain constant over time. This happens when the rates of the forward and reverse reactions are equal. This equilibrium state can be represented using the equilibrium constant (K), which is a ratio of the concentrations of the products to the reactants, each raised to the power of their respective coefficients from the balanced chemical equation.

Key Concepts:

  1. Dynamic Equilibrium: Chemical equilibria are dynamic, meaning that while the concentrations of reactants and products remain constant, the reactions continue to occur in both directions at the same rate.

  2. Equilibrium Constant (K): The equilibrium constant is a numerical value that indicates the ratio of product concentrations to reactant concentrations at equilibrium. For a general reaction aA+bB↔cC+dDaA + bB leftrightarrow cC + dD, the equilibrium constant expression is:

[ K = frac{[C]c[D]d}{[A]a[B]b} ]

Here, [A][A], [B][B], [C][C], and [D][D] represent the concentrations of the respective species.

  1. Le Chatelier’s Principle: This principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to partially counteract the change and restore a new equilibrium.

  2. Reaction Quotient (Q): The reaction quotient has the same form as the equilibrium constant expression but is used to determine the direction in which a reaction will proceed to reach equilibrium. If Q<KQ < K, the reaction will proceed in the forward direction; if Q>KQ > K, the reaction will proceed in the reverse direction.

Example Reaction: Consider the synthesis of ammonia (NH₃) via the Haber process:

N2(g)+3H2(g)↔2NH3(g)N_2(g) + 3H_2(g) leftrightarrow 2NH_3(g)

The equilibrium constant expression for this reaction is:

[ K = frac{[NH_3]2}{[N_2][H_2]3} ]

Importance of Equilibria: Understanding chemical equilibria is crucial in industrial processes, biological systems, and environmental science, as it helps in predicting the concentrations of reactants and products under different conditions and optimizing reactions for maximum yield.

 

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