Study Guide to Atomic Theory & Quantum Mechanics
DISCLAIMER: This Guide is not meant to be exhaustive. That is, I have
tried to summarize the essential points of the lectures on this topic. The
presence of a topic here does not guarantee a related question on an exam, nor
are exam topics limited to what appears in this Guide. As with any Chemistry
class, you are responsible for ALL of the assigned readings, problems and
lecture material. Lectures will often contain information not covered or given
less emphasis in the text.
Text
Reading
Chapter
12 (pages 510-573)
What
should you learn from this section of the course?
We have worked our way through the "history" of the development of
quantum mechanics. You should know what each famous chemist/physicist did. You
need not know any more detail than I presented, but you may find more in the
text or the reserve reading. The Bohr model is not correct, but provides a
chance to see just how quantum theory works. You should be comfortable with all
of its details and the experimental application to the hydrogen atom (the
Rydberg experiment you performed in the lab). Finally, we have developed the
particle in a box model problem. You must be able to follow what we did and
understand the implications. For hydrogen, we did not complete any derivation.
We took the results from the Schroedinger equation and used them to examine
hydrogen and hydrogen-like ions in detail. Finally, we examined the
implications of many electrons in an atom by looking at periodic properties such
as ionization energy and electron affinity. It is important for you to observe
and rationalize periodic trends in any property.
General
The Bohr Atom
The Schroedinger Equation
Many Electron Atoms
Recommended
Chapter 15 Problems
Light: 23, 25, 27,
29. Bohr Model: 31, 33, 35. Wave
Mechanics 37, 41, 43, 45, 47.
Orbitals: 49, 51, 54, 55, 57.
Many Electron Atoms: 61, 65, 67,
73, 77. The Periodic Table: 79, 81, 83, 85, 87, 91, 93, 95, 97, 107. Mixed Concepts: 109,
111, 113, 121, 125, 131
Additional
Problems
1. The emission spectrum of the hydrogen atom has a line in the infrared at 18,900 Angstrom. Calculate the energy in Joules of a photon with this wavelength. Assign this transition by identifying the principal quantum numbers of the initial and final energy levels that are involved.
2. Calculate the wavelength at which the series of lines to
which the 18,900 Angstrom line belongs will have its series limit. What is the physical significance of this series
limit? NOTE: A series of spectral lines in emission is characterized by a
common value of nfinal -- i.e. the
quantum number of the level at which the transition terminates. The series limit for a series
of emission lines is the wavelength that would correspond to the transition ninitial = ∞ to nfinal.
3. Explain why both the electron affinity and the ionization energy of Cl are greater than the corresponding quantities for S.
4. Electrons may be ejected from the surface of Mo by photons of 274 nm or less. What is the work function of Mo? What is the maximum kinetic energy of electrons ejected from Mo by 100 nm photons? What is the speed of the electrons ejected by 100 nm photons?
5. Calculate the energy required to remove the electron from the ground states of the following ions: He+, Li2+ and Be3+.
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