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Quiz 6 Introduction to Quantum Theory

Wave and particle properties of electromagnetic radiation.

Wave and particle duality of waves and particles.

A brief history on the development of quantum theory.
 Describe the nature of electromagnetic radiation
 Give names for the various ranges of the electromagnetic radiation spectrum
 Give the range of wavelengths in the visible region
 Evaluate wavelength from frequency
speed of light = 3.00e8 m s^{1}
= wavelength * frequency
in symbols commonly used
c = l n
 Evaluate frequency from wavelength
 Apply Planck's equation E = h n
to evaluate energy of photon
 Apply Einstein's interpretation for the photoelectric experiment
for problem solving.
Magnetic Spectra
 spectra, absorption spectra, emission spectra, line spectra,
continuous spectra
 hydrogen spectra, Raydberg equation, Raydberg constant,
The Bohr Atom
 Bohr assumption
 Energy level of the hydrogen atom
 Transitions for light emission and absorption
 Balmer series
 Explain rules of quantum numbers.
 Apply quantum number rules to work out the atomic orbitals.
 Describe the properties of atomic orbitals.
 Give the shape of 1s, 2s, 3s, 2p, 3p, and 3d atomic orbitals.
 Describe Pauli exclusion principle.
 Describe Zeeman effect.
 Describe the electron densities of various atomic orbitals.
 Plot the radial electron density for 1s, 2s, 3s, 2p, and 3d atomic
orbitals.
 Construct the periodic table of elements from atomic orbitals.
To review
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