Talk:High School Chemistry/Electrons and Light

Quiz

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Points for an incorrect answer:
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1 In 1900s, scientists found out that different elements made different colored-flames. What can be observed from this?

	This never happened.
	The arrangement of electrons determine the different colored-flames.
	It depends on the electron's atomic mass.
	Protons and neutrons both cause these different colors.

2 Complete the measurements.

1. v:

2. λ:

3 What is the speed of light?

4 Fill out the information.

As wavelength increases, frequency . As frequency increases, wavelength .

5 Which description fits the description for harmful wavelengths/frequencies?

	High frequency, short wavelength
	Short wavelength, high frequency
	Long wavelength, high frequency
	Short wavelength, short frequency

6 Fill out the information.

The visible spectrum goes from nanometers to nanometers.

7 Complete the formulas.

1. The mathematical relationship between energy and frequency:

2. The mathematical relationship between wavelength and frequency:

3. What is Planck's constant? .

8 Max Planck states that energy is quantized, and not continuous. Electromagnetic rays travel in waves and are made out of _____. Atoms can gain or lose energy in small amounts known as _____. Electrons have to ______ energy in order to move up through the orbits and ______ energy in order to move down through the orbits.

	quanta, photons, release, absorb
	photons, quanta, lose, absorb
	photons, quanta, absorb, lose
	photons, quanta, release, absorb

9 Complete the blanks with the correct information.

Electrons to the nucleus are the lowest in energy

10 Who found out that light is made up of photons?

	Albert Einstein
	Mannhoauf Einzwegol
	Adolf Friedrich Johann Butenandt
	Carl Bosch

11 Who stated that merely the act of observing an electron changes its position and velocity?

	Albert Einstein
	Werner Heisenberg
	J. J. Thomson
	Carl Bosch

12 Which rule requires you to fill up your lowest energy level before moving up to the next energy level?

	Aufbau
	Hund's rule
	Paul exclusion principle