Electrons jump around within an atom as they either gain or lose energy. When an electron is hit by a photon of light for example, it absorbs the energy the photon was carrying and moves to a higher energy state. Then, at some point, these higher energy electrons give up their “extra” energy in the form of a photon of light, and fall back down to their original energy level. The light that has suddenly been produced rushes away from the electron and c an be seen as light or color. This property of electrons, and the energy they absorb or give off, can be put to an every day use. In todays lab, students will study the electromagnetic spectrum and understand how electrons absorb or lose energy. Students will perform a flame test to show how energy is released as various colors.
Firework video: https://www.youtube.com/watch?v=WDGxepzOiLE Metal flame emission explanation: https://www.jove.com/science-education/11162/metal-flame-emission Flamer test lab results: cesium chloride (blue), barium chloride (green), cupric chloride (blue green), strontium chloride (red), potassium chloride (purple), lithium chloride (red), sodium chloride (yellow), calcium chloride (orange)