#Bohr's atomic theory series#

Discovering Water: James Watt, Henry Cavendish and the Nineteenth Century Water Controversy. Garden City, NY: Doubleday, 1964.įrayn, M. The Fly in the Cathedral: How a Small Group of Cambridge Scientists Won the Race to Split the Atom.

#Bohr's atomic theory series#

“ On the Constitution of Atoms and Molecules.” Philosophical Magazine Series 6 26 (July 1913): 1-15.Ĭathcart, B. On the Constitution of Atoms and Molecules. Niels Bohr: His Life and Work as Seen by His Friends and Colleagues. Suspended in Language: Niels Bohr’s Life, Discoveries, and the Century He Shaped. 6.1, “Waves and Electromagnetic Energy.”

Electrons change orbits by radiating or absorbing photons.

Electrons in stable orbits do not radiate.

Orbital angular momentum is quantized hence only certain orbits are possible.

c.The average radius of the hydrogen atom. b.The minimum radius of the hydrogen atom. a.The maximum radius of the hydrogen atom.

Electrons follow circular orbits around a nucleus In his calculations, Bohr came across a number now called the 'Bohr radius'.

Explanation of blackbody radiation and atomic spectra.

Majority of the mass is found in the nucleus.

Conclusions from the gold foil experiment.

Electrons are distributed uniformly throughout the atom.

He defines the different isotopes of hydrogen. He details Bohr’s postulates for the hydrogen atom and discusses how the Planck-Einstein relationship applies to electron transitions. Sadoway talks about the principles of modern chemistry and how that led to the understanding of the structure of the atom. Periodic Table and Table of Constants Lecture Summary Line spectra the Bohr model uses of emission and absorption spectra 6.3, “Atomic Spectra and Models of the Atom.” 6.2, “The Quantization of Energy.”īlackbody radiation the photoelectric effect The electron radioactivity the atomic model

Understand Bohr’s quantization condition.Īrchived Lecture Notes #1 (PDF), Sections 1-3.

Understand Rutherford’s “nuclear” model.

Understand Thomson’s “plum pudding” model.

Learning ObjectivesĪfter completing this session, you should be able to: Bohr's model calculated the following energies for an electron in the shell, n : E ( n) 1 n 2 13. Sadoway discusses the atomic spectra of hydrogen ( Session 4). Bohr's model of hydrogen is based on the nonclassical assumption that electrons travel in specific shells, or orbits, around the nucleus.

Lanthanum (La), magnesium (Mg), chlorine (Cl), titanium (Ti), helium (He), hydrogen (H)īefore starting this session, you should be familiar with: Thomson, proton, electrical charge, amber, alpha particle, beta particle, ionization, conservation of mass, Johannes Geiger, Ernest Marsden, coulomb, Niels Bohr, Bohr model of hydrogen, energy quantization, orbital angular momentum, Planck-Einstein relationship, joule, Newtonian force, Coulombic force, Max Planck, photon, energy, frequency, Planck’s constant, isotope, Henry Cavendish, Harold Urey, Ernest Rutherford, blackbody radiation Lanthanides, actinides, electron, mass, J. Thomson’s plum pudding model, Rutherford’s model of the nucleus, Bohr’s model of the hydrogen atom, Rutherford-Geiger-Marsden experiment, Planck-Einstein relationship, isotopes of hydrogen