If the atom looked like a solar system, how could line spectra be explained? Line spectra are what you get when you excite gases with a high voltage. Gases emit light at only a few sharply-defined frequencies, and the frequencies are different for different gases. These emission spectra, then, are made up of a few well-defined lines.
In 1885 Johann Jakob Balmer showed that the wavelengths of light in the hydrogen spectrum could be predicted by the following equation:
Balmer series: |
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= R | ( |
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- |
|
) | where n = 3, 4, 5, ... |
R is known as the Rydberg constant, R = 1.097 x 107 m-1
The first three wavelengths in the Balmer series are:
n = 3, l = 656 nm
n = 4, l = 486 nm
n = 5, l = 434 nm
Gases will also selectively absorb light at these same frequencies. You can see this if you expose a gas to a continuous spectrum of light. The absorption spectra will be very similar to a continuous spectrum, except for a few dark lines corresponding to the frequencies absorbed by the gas.