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Modern Physics: Section 12-3
“Energy Level Diagrams”Time : 41 minutes, 09 seconds
OPEN YOUR PHYSICS REFERENCE TABLES TO THE “ENERGY LEVEL DIAGRAMS” PAGE NOW
HYDROGEN IS SHOWN ON THE LEFT, MERCURY IS SHOWN ON THE RIGHT
NOTE: In the video the transition from n=5 to n=2 in the hydrogen atom the emitted photon is stated to be in the Balmer Series and GREEN in color. While this transition is listed on some charts and diagrams on the Internet as GREEN, the calculations agree with a BLUE photon based upon the Physics Reference Tables. This disagreement between charts from different sources is trivial and you should not worry too much about the discrepancy.
1. Explain what the two diagrams “Hydrogen” and “Mercury” are showing on your Physics Reference Tables
2. In chemistry we generally orient an electron shell diagram from left to right. On the “Energy Level Diagrams”
Chart in the Physics Reference Tables, the energy levels are oriented from ______to
______.
3. If an electron jumps from any lower energy level to infinity, the electron is “lost” and the atom
has been ______(it has become an ion by losing an electron).
4. The energy levels closer to the nucleus (at the bottom of the chart) are ______energy
levels. The energy levels further away from the nucleus (higher on the chart) are ______
energy.
5. If an electron jumps from the n=1 energy level to the n=2 energy level it must absorb
______eV of energy. (Just subtract the two numbers, forget the negative signs)
6. If an electron jumps from the n=1 energy level to the n=3 energy level it must absorb
______eV of energy. (Just subtract the two numbers, forget the negative signs)
7. If an electron jumps from the n=1 energy level to the n=4 energy level it must absorb
______eV of energy. (Just subtract the two numbers, forget the negative signs)
8. If an electron jumps from the n=1 energy level to the n=5 energy level it must absorb
______eV of energy. (Just subtract the two numbers, forget the negative signs)
9. Show the difference in electron volts between each pair of energy levels below with an arrow going up.
Show 1 to 2, 1 to 3, 1 to 4 and 1 to 5. Then show 2 to 3, 2 to 4 and 2 to 5
You will have to do some of the math on your own. There should be 7 labeled arrows when you finish.
n = ∞ ------Ionization
n = 5 ------
n = 4 ------
n = 3 ------
n = 2 ------
n = 1 ------Ground State
10. In order for an electron to be able to jump from one energy level to a higher energy level,
The electron must absorb a photon with exactly the correct amount of energy (the difference between the two
Energy Levels) For example, to jump from the n=1 energy level to the n=2 energy level, the photon must
have exactly ______eV
11. The energy levels at the bottom ( ______to the nucleus) are
______energy levels.
12. The energy levels at the top ( ______from the nucleus) are
______energy levels.
13. Which direction ( up or down ) on the “Energy Level Diagram” shows energy being absorbed?
After an electron absorbs energy and jumps to a higher energy level, the electron (or the atom) is said to
be ______, or in the excited ______.
14. Which direction ( up or down ) on the “Energy Level Diagram” shows energy being emitted?
Electrons ______or “give off” energy when they ______
From a higher to a lower energy level.
15. Many types of energy can be ( absorbed , emitted ) by the electrons in atoms. Electrons can
absorb ______, ______or a photon of light.
16. The only type of energy that can be ( absorbed , emitted ) by the electrons in atoms is photons of light.
SUMMARY:
17. Electrons can absorb several different types of energy. They can absorb ______,
______or ______. When an electron absorbs energy,
It ______from a lower to a ______energy level
And we say that the electron (or the atom it belongs to) is ______. On our
Diagrams an electron absorbs energy when it goes up the diagram.
18. Electrons can only emit one type of energy, that is ______,
When an electron emits a photon of ______
It ______from a ______to a
______energy level.
And we say that the electron (or the atom it belongs to) is back in the ______
State. On our diagrams, electrons emit light when they go ______the diagram.
The Hydrogen Atom
19. In the hydrogen atom, when an electron falls to the 1st energy level from any higher energy level, it gives off
______light. Draw three arrows on the diagram below showing electrons falling from
higher energy levels down to n = 1. What scientist are these ultraviolet rays named after? ______
20. In the hydrogen atom, when an electron falls to the 2nd energy level from any higher energy level, it gives off
______light. Draw four arrows on the diagram below showing electrons falling from
higher energy levels down to n = 2. What scientist are these visible light rays named after? ______
21. In the hydrogen atom, when an electron falls to the 3rd energy level from any higher energy level, it gives off
______light. Draw three arrows on the diagram below showing electrons falling from
higher energy levels down to n = 3. What scientist are these infrared rays named after? ______
Label the type of light and the name of the scientist above each section of arrows on the diagram below.
n = ∞ ------Ionization
n = 6 ------
n = 5 ------
n = 4 ------
n = 3 ------
n = 2 ------
n = 1 ------Ground State
Calculating the Energy of Emitted Photons to Figure Out the Type of Light
22. An electron falls from the n=5 energy level to the n=1 energy level of a hydrogen atom.
Because we are falling to the 1st energy level, we know that this photon of light will be in the
______series and it will be ______light.
a. Calculate the change in energy in eVb. Convert the electron volts to Joules
c. Calculate the frequency of the photond. Identify the type of light using the calculated frequency
by going to the chart “The Electromagnetic Spectrum”
e. When an electron falls from the n=5 to the n=1 energy level, it emits a photon of
______light
23. An electron falls from the n=4 energy level to the n=2 energy level of a hydrogen atom.
Because we are falling to the 2nd energy level, we know that this photon of light will be in the
______series and it will be ______light.
a. Calculate the change in energy in eVb. Convert the electron volts to Joules
c. Calculate the frequency of the photond. Identify the type of light using the calculated frequency
by going to the chart “The Electromagnetic Spectrum”
e. When an electron falls from the n=4 to the n=2 energy level, it emits a photon of
______light and the color is ______
24. An electron falls from the n=6 energy level to the n=3 energy level of a hydrogen atom.
Because we are falling to the 3rd energy level, we know that this photon of light will be in the
______series and it will be ______light.
a. Calculate the change in energy in eVb. Convert the electron volts to Joules
c. Calculate the frequency of the photond. Identify the type of light using the calculated frequency
by going to the chart “The Electromagnetic Spectrum”
e. When an electron falls from the n=6 to the n=3 energy level, it emits a photon of
______light
Now Identify the Type of Emitted Light on Your Own (This example is not shown in the video)
25. An electron falls from the n=3 energy level to the n=2 energy level of a hydrogen atom.
Because we are falling to the 2nd energy level, we know that this photon of light will be in the
______series and it will be ______light.
a. Calculate the change in energy in eVb. Convert the electron volts to Joules
c. Calculate the frequency of the photond. Identify the type of light using the calculated frequency
by going to the chart “The Electromagnetic Spectrum”
e. When an electron falls from the n=3 to the n=2 energy level, it emits a photon of
______light and the color is ______
Problems Based on the Mercury Diagram
26. An electron falls from the f energy level to the b energy level of a mercury atom.
a. Calculate the change in energy in eVb. Convert the electron volts to Joules
c. Calculate the frequency of the photond. Identify the type of light using the calculated frequency
by going to the chart “The Electromagnetic Spectrum”
e. When an electron falls from the f to the b energy level, it emits a photon of
______light and the color is ______
Referring Again to the Hydrogen Atom Diagram
27. In order to ionize an electron from the n=1 energy level (to infinity) how many electron
volts of energy would be required? ______
28. In order to ionize an electron from the n=3 energy level (to infinity) how many electron
volts of energy would be required? ______
29. An electron in a hydrogen atom absorbs a photon and transitions from n=2 to n=5.
How many electron volts was the photon? ______
30. An electron in a hydrogen atom absorbs a photon and transitions from n=4 to n=6.
How many electron volts was the photon? ______
31. An electron in a hydrogen atom falls from n=6 to n=1 and emits a photon of light.
How many electron volts is the photon? ______
32. Look on the front of the Reference Tables. How much is Planck’s Constant? ______