Structure Of Atom

The section covers the structure of atoms and the discovery of sub-atomic particles, outlining various atomic models and quantum mechanical properties.

Discovery Of Sub-Atomic Particles

This section outlines the historical discovery of sub-atomic particles, including electrons, protons, and neutrons, and explores the experiments that led to our current understanding of atomic structure.

Discovery Of Electron

The discovery of the electron transformed the understanding of atomic structure, revealing that atoms are composed of subatomic particles.

Charge To Mass Ratio Of Electron

This section discusses the historical measurement of the charge-to-mass ratio of the electron, providing insights into its fundamental properties discovered through experiments.

Charge On The Electron

The charge on the electron, determined by R.A. Millikan's oil drop experiment, is crucial for understanding atomic structure.

Discovery Of Protons And Neutrons

The section outlines the discovery of protons and neutrons and their significance in atomic structure.

Atomic Models

This section discusses atomic models that emerged from the discovery of sub-atomic particles, focusing on their implications for atom stability and molecular formation.

Thomson Model Of Atom

The Thomson model, proposed in 1898, describes the atom as a uniformly charged sphere with embedded electrons, akin to a plum pudding.

Rutherford Nuclear Model Of Atom

The Rutherford Nuclear Model introduces a revised understanding of atomic structure, proposing that atoms consist of a dense nucleus surrounded by electrons in orbit.

Atomic Number And Mass Number

The section discusses atomic number and mass number, their definitions, and their significance in identifying elements and isotopes.

Isobars And Isotopes

This section discusses isobars and isotopes, highlighting their definitions, characteristics, and significance in atomic structure.

Drawbacks Of Rutherford Model

The Rutherford model, while revolutionary in demonstrating nuclear structure, fails to explain atomic stability and electron distribution.

Developments Leading To The Bohr’s Model Of Atom

This section outlines the key developments that led Niels Bohr to formulate his model of the atom, particularly focusing on the dual nature of electromagnetic radiation and experimental results regarding atomic spectra.

Wave Nature Of Electromagnetic Radiation

This section explores the wave nature of electromagnetic radiation, emphasizing its properties, the electromagnetic spectrum, and the foundational concepts introduced by Maxwell and Planck.

Particle Nature Of Electromagnetic Radiation: Planck’s Quantum Theory

This section explores the particle nature of electromagnetic radiation, focusing on Planck’s Quantum Theory and its explanations for phenomena such as black-body radiation and the photoelectric effect.

Evidence For The Quantized Electronic Energy Levels: Atomic Spectra

This section discusses the quantized electronic energy levels of atoms, focusing on atomic spectra as evidence for these levels.

Bohr’s Model For Hydrogen Atom

Bohr's Model offers a groundbreaking explanation for the structure of the hydrogen atom, employing quantization to describe electron orbits and energy levels.

Explanation Of Line Spectrum Of Hydrogen

The line spectrum of hydrogen can be explained using Bohr's model, which describes quantized energy levels for the electron.

Limitations Of Ohr’s Model

Bohr's atomic model is an important advancement in atomic theory, but it has significant limitations in explaining complex atomic behavior.

Towards Quantum Mechanical Model Of The Atom

The section discusses the failures of Bohr's atomic model and introduces the quantum mechanical model, which incorporates the dual nature of matter and the Heisenberg uncertainty principle.

Dual Behaviour Of Matter

The dual behaviour of matter encompasses both particle and wave-like characteristics of subatomic particles, significantly impacting our understanding of atomic structure.

Heisenberg’s Uncertainty Principle

The Heisenberg Uncertainty Principle posits that it is impossible to know both the exact position and momentum of an electron simultaneously.

Electronic Configuration Of Atoms

This section discusses the electron distribution in atomic orbitals, known as electronic configuration, highlighting its significance in determining chemical behavior.

Quantum Mechanical Model Of Atom

The Quantum Mechanical Model describes the atomic structure as a complex system where electrons exist in probabilistic atomic orbitals rather than fixed orbits, built on the principles of quantum mechanics.

Orbitals And Quantum Numbers

This section introduces orbitals and quantum numbers, crucial for understanding the electronic structure of atoms.

Shapes Of Atomic Orbitals

This section discusses the shapes of atomic orbitals and their implications for electron distribution in atoms.

Energies Of Orbitals

This section discusses the energy levels associated with different atomic orbitals in hydrogen and multi-electron atoms.

Filling Of Orbitals In Atom

The filling of electrons in an atom's orbitals occurs according to the Aufbau principle, influenced by the Pauli exclusion principle and Hund's rule.

Stability Of Completely Filled And Half Filled Subshells

The stability of atoms is influenced by the electronic configuration, particularly in regard to completely filled and half-filled subshells.

Summary

This section covers the atomic theory's evolution, focusing on subatomic particles and the atomic models proposed by notable scientists.

Exercises

This section provides various exercises related to atomic structure, covering concepts from atomic particles to quantum numbers and electron configurations.