Light and Energy

How the structure of electrons relates to the function of emitting

energy as light

Light Bulbs…which uses less energy?

Let’s look at it in another way…

Let’s follow the sun!

All elements absorb a certain

amount of energy and release that

energy as specific

“fingerprints” of light

Energy is emitted because electrons “jump” and then “fall”

The amount electrons jump is

“quantized” and therefore

we can measure energy

produced by the color of

light.

Today we will:

• Determine the difference between continuous, absorption and emission spectra.

• Observe the spectral fingeprints of various types of light.

• Calculate the energy associated with different wavelengths of light.

• Explain how the excitation of electrons and their fall back to their original state allows us to see light.

Tool: Spectroscope

If you are really stuck…

• Try to look in the spectroscope. If you get really stuck, google image what the spectral fingerprint of what you are looking at SHOULD look like.

• Look again with the spectroscope and see if you can see what was expected.