- Carbon dioxide (CO
_{2}) in the atmosphere acts as a greenhouse gas by absorbing infrared radiation at a wavelength of 15µm. What is the frequency of this radiation (Hz)? What is the energy of a single photon of this radiation (J)? What is the energy of a mole of photons at this wavelength (J mole^{-1})? - Ozone (O
_{3}) in the stratosphere filters out ultraviolet radiation by absorbing light at a wavelength of 250 nm. What is the frequency of this radiation (Hz)? What is the energy of a single photon of this radiation (J)? What is the energy of a mole of photons at this wavelength (J mole^{-1})? - What is the wavelength (nm), frequency (Hz), energy per photon (J) and energy per mole of photons (J mole
^{-1}) of the radiation produced by the transition of an electron in hydrogen- from the n=2 to n=1 level
- from the n=3 to n=1 level
- from the n=5 to n=1 level
- from the n=10 to n=1 level
- from the n=100 to n=1 level

- Make a table of the possible quantum numbers for a hydrogen electron that has been excited to a,
- 2s orbital
- 4p orbital
- 5d orbital
- 6f orbital

- Draw diagrams of the following orbitals,
- 1s
- 2p
_{x} - 2p
_{y} - 2p
_{z}

Please send comments or suggestions to svanbram@science.widener.edu

Scott Van Bramer

Department of Chemistry

Widener University

Chester, PA 19013

*© copyright 1996, S.E. Van Bramer*

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Last Updated: Saturday, May 18, 1996