Different elements emit unique atomic line spectra colors when burned, due to electrons gaining and losing discrete energy levels and releasing photons of specific frequencies. Lithium burns with an orangish-yellow hue, demonstrating flame tests can distinguish elements based on their colored flames. Questions ask why chemicals have different colored flames, why heating is needed before light emission, and how metals create the color in salts.

1. Flame Test Lab

2. Background Chemists began studying colored flames in the 18 th century and soon used "flame tests" to distinguish between some elements. Different elements burn with different colored flames. Although some of the flames you will be seeing will appear similar in color, their light can be resolved (separated) with a prism into distinctly different bands of colors on the electromagnetic spectrum (ROYGBIV). These bands of colors are called atomic line spectra , and they are UNIQUE to each element.

3. October sunset tinged with Autumn maple leaves Lithium (Li) Solid Orangish yellow with a hint of tangerine Lithium (Li) Solution Color Metal

4. Questions Why do different chemicals emit different colors of light? Why do you think the chemicals have to be heated in the flame first before the colored light is emitted? The salt used for this experiment contained metals and niitrogen, how do we know the metals create the color?

5. More Questions What happens to an electron when energy is added? What is released when an electron loses energy? What determines the frequency (color) of photons?