Absorption and Emission Lines (Part 1)

In the last page, you examined the spectra of 7 stars. You probably noticed two features that all the spectra had in common. All the spectra have similar overall shapes, and all have peaks and valleys of different heights. These are the very same features astronomers use to classify stars.

The Hydrogen Atom

To begin to understand what the peaks and valleys mean, let’s take a close look at a hydrogen atom. A hydrogen atom has one proton and one electron. Its electron can only occupy certain energy levels; think of energy levels as unequally-spaced steps of a ladder. The higher up an electron is on the ladder, the more energy it has. Astronomers use the letter ‘n’ and a number to designate each energy level. The lowest energy level is called the ‘n=1’ level, the second lowest level ‘n=2’, the third ‘n=3’, and so on.

Electrons can move from one level to another, but the atom’s total energy must always be conserved. So, if an electron moves down from the 2nd energy level to the 1st (n=2 to n=1), then the atom conserves energy by emitting a photon of light. The emitted photon has an energy equal to the difference between the 2nd and 1st energy levels. An electron can only move up from the 1st to 2nd energy level if it gains the right amount of energy. The electron typically gains this energy if the atom absorbs a photon of light with the right energy.

When an electron in the n=1 energy level absorbs a photon to go to n=2, it emits a photon of the same energy to go back to n=1. Because a photon’s wavelength is determined by its energy, if you know the energy a photon has, you know its wavelength. To go up from n=1 to n=2, an electron must absorb a photon with an energy of 10.2 electron-Volts (1.63 x 10-18 Joules) – this photon has a wavelength of 1216 Ångstroms.

To go down from n=2 to n=1, the atom must emit a photon of 1216 Ångstroms.

Question 4. To go up in energy level from n=1 to n=2, what wavelength of light must a hydrogen atom absorb? How do you know?