Chapter 7 Lecture Problems
7.1 Schrodinger's Cat
7.2 The Nature of Light
- What is the frequency of light at 120 nm (a wavelength I frequently used for
experiments in graduate school)
- What is the wavelength of the radiation for proton NMR in our instrument (300
MHz)
- What wavelength of light corresponds to the energy of an O=O bond, 498 kJ/mol.
- 498 kJ/mol = 8.27 * 10-19 J/molecule
- This is the amount of energy that 1 photon must have to break the bond in
an O=O atom. Since the energy of a photon is related to it's frequency as:
- E = h v (v is the greek nu and h is Planck's constant)
- v = 1.25 * 1015 Hz (Hz is frequency or s-1)
- c = [lambda] * v
- [lambda] = 2.40 * 10-7 meters or 240 nm
- What energy (kJ/mol) corresponds to the wavelength of light required to remove
an electron from a hydrogen atom (90 nm)
- 90 nm = 90*10-9 m
- Since c = [lambda] * v
- v = (3*108 m/sec)/(90*10-9 m)
- v = 3.33*1015 Hz
- Since E=h v
- E = (33.3*1015 Hz) * (6.626*10-34 J sec/photon)
- E = 2.21*10-18 J/photon
- Multiply by Avogadro's number to get J/mol
- E = (2.21*10-18 J/photon) * (6.02*1023 photon/mol)
- E = 1.33*106 J/mol
- E = 1330 kJ/mol
7.3 Atomic Spectroscopy and the Bohr Model
7.4 The Wave Nature of Matter: the de Broglie Wavelength, the Uncertainty Principle, and Indeterminancy
7.5 Quantum Mechanics and the Atom
7.6 The Shapes of Atomic Orbitals
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Department of Chemistry
Widener University
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Last Updated Friday, May 25, 2001 2:10:36 PM