Bohr-Rutherford Model

Emission Spectrum

Bohr heated hydrogen and looked at the colours released. He then separated that light using a prism (spectroscope).

Bohr determined that the lines in the visible spectrum were the result of energy being released when an electron drops to level .

Going to would be UV light, and would be IR.

Bohr mathematically calculated this, but could not verify it at the time.

• The UV spectrum is called the Lyman series (anything down to 1)
• The visible spectrum is called the Balmer series (anything down to 2)
• The IR spectrum is called the Paschen series (anything down to 3)

Absorption Spectrum

If we direct white light through some sample hydrogen, the spectra should be complementary.

The absorption spectrum is just the opposite of the emission spectrum. That is, it is caused by electrons jumping from . For example, an electron jumping from to would create absorb the same amount of energy as green light, removing it from the spectrum.