Lecture

Atomic Structure: Bohr Model

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Description

This lecture introduces the concept of atomistic structure, focusing on the Bohr model. It covers the historical development of atomic theory, from Democritus to John Dalton, and explains the key features of the Bohr model, such as quantized energy levels and spectral lines. The lecture also discusses the limitations of the Bohr model and contrasts it with the Schrödinger model, emphasizing the transition from classical to quantum mechanics in describing atomic behavior. Furthermore, it delves into the significance of electron orbitals, isotopes, and the dual nature of electrons as particles and waves, providing a comprehensive overview of atomic structure.

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Ontological neighbourhood

Physics

Atomic physics: Topics in atomic physics

Related concepts (32)

Bohr model

In atomic physics, the Bohr model or Rutherford–Bohr model of the atom, presented by Niels Bohr and Ernest Rutherford in 1913, consists of a small, dense nucleus surrounded by orbiting electrons. It is analogous to the structure of the Solar System, but with attraction provided by electrostatic force rather than gravity, and with the electron energies quantized (assuming only discrete values).

Atomic physics

Atomic physics is the field of physics that studies atoms as an isolated system of electrons and an atomic nucleus. Atomic physics typically refers to the study of atomic structure and the interaction between atoms. It is primarily concerned with the way in which electrons are arranged around the nucleus and the processes by which these arrangements change. This comprises ions, neutral atoms and, unless otherwise stated, it can be assumed that the term atom includes ions.

Bohr radius

The Bohr radius (a0) is a physical constant, approximately equal to the most probable distance between the nucleus and the electron in a hydrogen atom in its ground state. It is named after Niels Bohr, due to its role in the Bohr model of an atom. Its value is The Bohr radius is defined as where is the permittivity of free space, is the reduced Planck constant, is the mass of an electron, is the elementary charge, is the speed of light in vacuum, and is the fine-structure constant.

Atomic theory

Atomic theory is the scientific theory that matter is composed of particles called atoms. The concept that matter is composed of discrete particles is an ancient idea, but gained scientific credence in the 18th and 19th centuries when scientists found it could explain the behaviors of gases and how chemical elements reacted with each other. By the end of the 19th century, atomic theory had gained widespread acceptance in the scientific community. The term "atom" comes from the Greek word atomos, which means "uncuttable".

Isotope geochemistry

Isotope geochemistry is an aspect of geology based upon the study of natural variations in the relative abundances of isotopes of various elements. Variations in isotopic abundance are measured by isotope ratio mass spectrometry, and can reveal information about the ages and origins of rock, air or water bodies, or processes of mixing between them. Stable isotope geochemistry is largely concerned with isotopic variations arising from mass-dependent isotope fractionation, whereas radiogenic isotope geochemistry is concerned with the products of natural radioactivity.

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