Atomic spectra of hydrogen atom series#

Cambridge, MA: Harvard University Press, 1963. New York, NY: Cambridge University Press, 1996. Cecilia Payne-Gaposchkin: An Autobiography and Other Recollections. This lecture gives more details about the atomic spectra of hydrogen along with matter/energy interactions involving atomic hydrogen. Lecture Slides (PDF - 1.3MB) Lecture Summary Line spectra the Bohr model uses of emission and absorption spectra (c) doc b Bohrs model of hydrogen assumes that electrons can only exist in certain specific electronic energy levels. 6.3, “Atomic Spectra and Models of the Atom.” The principal quantum number is an integer n that corresponds to the gross energy states of the atom.

The solutions to the Schrödinger equation are catalogued in terms of certain quantum numbers of the particular electron state. Describe the ground state of the gas phase atom.Īrchived Lecture Notes #1 (PDF), Sections 3, 5 The hydrogen atom is composed of a single proton and a single electron.Explain trends in ionization energy across the periodic table.

Atomic spectra of hydrogen atom series#

Calculate the energy of an electron in the ground state of hydrogen. Four more series of lines were discovered in the emission spectrum of hydrogen by searching the infrared spectrum at longer wave-lengths and the ultraviolet.

Explain why the radius of the electron orbital takes multiple values that are discrete, quantized, and non-linear.

Describe how the atomic spectra of hydrogen is produced. The atomic hydrogen emission spectrum is the spectrum of electromagnetic radiation emitted by the hydrogen atom when its electrons make transitions between.

Learning ObjectivesĪfter completing this session, you should be able to: Sadoway discusses the shell model and quantum numbers ( Session 5).

Session 3: Atomic Models: Rutherford & Bohr.

Matter/Energy Interactions: Atomic SpectraĪtomic spectra of hydrogen, matter/energy interactions involving atomic hydrogen, planetary model, Bohr’s postulates, quantum condition, ionization energy, electron orbital transitionsĪngstrom, Avogadro’s number, prism, refraction, wavelength, nanometer, Johann Balmer, wavenumber, Michael Faraday, cathode, anode, electron-volt, Bohr radius, ground state, ionization energy, energy level, conservation of energy, atomic spectra, Cecilia Payne, Ernest Rutherford, joule, coulomb, Max Planck, Planck’s constant, emission spectra, spectrograph, electrode, photon, volt, radiationĬhemical analysis, analyzing composition of stars, televisionīefore starting this session, you should be familiar with: