Chemistry - BHAJAN GYAN EDUCATION

1. Atomic and Molecular Structure
Atomic structure refers to the composition and arrangement of subatomic particles within an atom. An atom consists of a nucleus, which contains protons and neutrons, and electrons that orbit the nucleus in defined energy levels or electron shells. The protons have a positive charge, neutrons are neutral, and electrons have a negative charge. The number of protons in the nucleus defines the atomic number of an element and determines its chemical properties. The arrangement of electrons in various shells and subshells follows the principles of quantum mechanics, which explain the distribution and behavior of electrons around the nucleus.

Bohr Theory of Hydrogen atom

10:22
Spectrum of H atom

10:43
Sommerfeld Extension of Bohr Theory

19:55
Particle and wave nature of electron

04:58
De-Broglie equation

19:25
Aufbau principle

17:57
Compton effect

04:05
Schrodinger wave equation

12:36
Laplacian and Hamiltonian operator

18:07
Linear Combination of atomic orbitals

18:53
Molecular orbitals of diatomic molecules

07:48
Energy level diagrams of homonuclear and heteronuclear diatomics

28:23
Pi-molecular orbitals of butadiene

15:56
Pi-molecular orbitals of Benzene

12:22
Pi-molecular orbitals of Aromaticity

28:14
Crystal field theory and the energy level diagrams for transition metal ions and their magnetic properties

56:36
Band structure of solids and the role of doping on band structures.

25:53

2. Spectroscopic Techniques and Applications
Definition:- Spectroscopic techniques are analytical methods used to measure and interpret the interaction between matter and electromagnetic radiation. These techniques are pivotal in identifying, quantifying, and studying the chemical composition, structure, and physical properties of substances. In the context of engineering chemistry, spectroscopy provides critical insights into the molecular and atomic characteristics of materials, aiding in the development, optimization, and quality control of engineering processes and products. Applications in Engineering Chemistry:- 1. Material Characterization 2. Chemical Analysis 3. Quality Control 4. Surface Analysis 5. Environmental Monitoring

Principles of Electronic spectroscopy

23:21
Selection Rules of Electronic Spectroscopy

12:30
Fluorescence spectroscopy along with their applications

13:20
Principles of Vibrational and rotational spectroscopy of diatomic molecules

26:58
Selection rules of Vibrational spectroscopy of diatomic molecules

07:51
Selection rules of Rotational spectroscopy of diatomic molecules

10:11
Application of Vibrational and rotational spectroscopy of Diatomic molecules

14:57
Introduction of Nuclear Magnetic Resonance

12:59
Nuclear Magnetic Resonance up to Spin-Spin coupling

13:30
Introduction of Magnetic Resonance Imaging

05:39

3. Intermolecular Forces and Potential Energy Surfaces
Intermolecular Forces: Intermolecular forces are the attractive and repulsive forces between molecules that influence the physical properties of substances, such as boiling and melting points, vapor pressure, and solubility. These forces include hydrogen bonds, Van der Waals forces (dipole-dipole interactions, London dispersion forces), and ion-dipole interactions. Potential Energy Surfaces: Potential energy surfaces represent the variation of potential energy of a system, particularly molecules, as a function of the positions of its atoms. These surfaces illustrate how energy changes during chemical reactions and molecular interactions, helping to understand reaction mechanisms and molecular dynamics.

4. Use of Free Energy in Chemical Equilibria
The use of free energy in chemical equilibria refers to its role in determining whether a chemical reaction can occur spontaneously under given conditions. It helps engineers predict and control reactions by assessing the balance between the energy available to do work (free energy) and the conditions that influence reaction directionality, such as temperature and pressure.

Ideal Solution

29:29
Non-Ideal Solutions

29:34
Thermodynamic functions: energy, entropy and free energy

13:02
Free energy and emf

17:52
Cell potentials

05:17
The Nernst Equation and Applications

11:27
Acid – Base

13:13
Oxidation – Reduction

07:03
Solubility Equilibria

08:15
Thermodynamic properties of ideal solutions

59:31
Introduction to Electrochemical Corrosion and its Mechanism

14:24
Use of free energy considerations in metallurgy through Ellingham diagrams.

32:14

5. Periodic Properties
In engineering chemistry, periodic properties refer to the recurring trends observed in the chemical and physical characteristics of elements as they are arranged in the periodic table. These properties, which vary in a predictable manner across different periods (rows) and groups (columns) of the periodic table, include atomic radius, ionization energy, electron affinity, electronegativity, and metallic and non-metallic behavior. Understanding these periodic properties is crucial for engineers and chemists as they influence the reactivity, bonding, and overall behavior of elements in various chemical processes and applications.

Effective nuclear charge

11:18
Penetration of Orbitals

08:21
Variations of s, p, d and f Orbital Energies of atoms in the periodic table

14:46
Electronic Configurations

10:19
Atomic and Ionic Sizes

17:21
Ionization Energies

15:05
Electron Affinity and Electronegativity

08:41
Polarizability

08:01
oxidation states

18:21
Coordination Numbers and Geometries

15:06
Principle of Hard acid and Base, Soft acid and Base

14:27

6. Stereochemistry
In engineering chemistry, stereochemistry refers to the branch of chemistry that focuses on the spatial arrangement of atoms within molecules and the effects of this arrangement on the chemical and physical properties of substances. It deals with the three-dimensional structure of molecules and how this structure influences their interactions, reactivity, and behavior in various chemical processes. Stereochemistry is crucial in understanding and designing chemical reactions, synthesizing new compounds, and optimizing industrial processes, as the spatial orientation of molecules can significantly impact their effectiveness and function.

Course Content

Bohr Theory of Hydrogen atom

Spectrum of H atom

Sommerfeld Extension of Bohr Theory

Particle and wave nature of electron

De-Broglie equation

Aufbau principle

Compton effect

Schrodinger wave equation

Laplacian and Hamiltonian operator

Linear Combination of atomic orbitals

Molecular orbitals of diatomic molecules

Energy level diagrams of homonuclear and heteronuclear diatomics

Pi-molecular orbitals of butadiene

Pi-molecular orbitals of Benzene

Pi-molecular orbitals of Aromaticity

Crystal field theory and the energy level diagrams for transition metal ions and their magnetic properties

Band structure of solids and the role of doping on band structures.

Principles of Electronic spectroscopy

Selection Rules of Electronic Spectroscopy

Fluorescence spectroscopy along with their applications

Principles of Vibrational and rotational spectroscopy of diatomic molecules

Selection rules of Vibrational spectroscopy of diatomic molecules

Selection rules of Rotational spectroscopy of diatomic molecules

Application of Vibrational and rotational spectroscopy of Diatomic molecules

Introduction of Nuclear Magnetic Resonance

Nuclear Magnetic Resonance up to Spin-Spin coupling

Introduction of Magnetic Resonance Imaging

Ideal gas equation

Ionic Interaction

Dipolar Interactions

Vander Waals Interactions

Real gas equation

Equations of State of Real gases and Critical phenomena

Potential energy surfaces of H3

Potential energy surfaces of HCN

Ideal Solution

Non-Ideal Solutions

Thermodynamic functions: energy, entropy and free energy

Free energy and emf

Cell potentials

The Nernst Equation and Applications

Acid – Base

Oxidation – Reduction

Solubility Equilibria

Thermodynamic properties of ideal solutions

Introduction to Electrochemical Corrosion and its Mechanism

Use of free energy considerations in metallurgy through Ellingham diagrams.

Effective nuclear charge

Penetration of Orbitals

Variations of s, p, d and f Orbital Energies of atoms in the periodic table

Electronic Configurations

Atomic and Ionic Sizes

Ionization Energies

Electron Affinity and Electronegativity

Polarizability

oxidation states

Coordination Numbers and Geometries

Principle of Hard acid and Base, Soft acid and Base

Representations of 3-dimensional structures

Structural isomers and Stereoisomers

Configurations

Symmetry

Chirality

Enantiomers AND Diastereomers

Student Ratings & Reviews

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