Instructor’s Notes for Assignment #93: The Photon Game
Steve Sogo, Laguna Beach High School ssogo@lbusd.org
Overview: This game is designed to help students understand the nature of quantum energy
states within an atom and their correlation to the production of discrete photons. In the game,
students work in pairs, using an energy well to simulate the quantum leaps made by electrons in
excited atoms. Colored pencils are used to record the colors of photons produced, based on the
energy difference between the initial and final quantum states of the electron.
Why do this activity?
In my teaching, I found that students enjoyed looking at atomic spectra, but their conceptual
understanding of how/why the various colors were produced was always disappointing. This
game enhances conceptual understanding in a user-friendly, enjoyable activity. Cooperation
between student pairs is required for “victory”.
Materials:
 One practice game board per student
 One version C game board and one version D game board per pair
 Set of colored pencils (Red, Orange, Yellow, Green, Blue, Violet, Black/Gray) needed
for each pair of students
 Calculators may be required
 Powerpoint slide show used by the instructor
Note: To obtain electronic copies of this lab, including instructor’s notes with color photos,
please Google “Steve Sogo Haiku”, which should take you to the “Chemistry with Mr. Sogo”
Haiku page. From here, click on the “ChemEd 2015” link displayed in the lower right corner of
the Haiku page (see picture below). This link will take you to a site where you will find
downloadable editable documents (MS Word format) including both student pages and
instructor’s notes. The instructor’s notes will provide links to relevant Youtube instructional
videos from the ACR92651 channel.
Assignment #93a: The Photon Game!!!
Key Concepts:
1. You will work with a partner in this game. Each of you will need to start with a game board
that represents the quantum energy levels in a particular atom (see next page for example!).
2. You will need a ¾” disk to represent an electron. In this game, the electron will be jumping
between various energy levels within each atom.
3. Take a look at the gameboard on the next page and notice that there are energy values written
on the board. Based on these energy values, try to complete the sentences below:
In any atom, the lowest energy level is labeled as n = ___. This corresponds to the innermost shell
of the atom. As n increases, energy approaches _____ kJ/mol. This means that an outer shell is
at a relatively high / low energy level compared to an inner shell. If an electron ever reaches the
energy level of zero kJ/mole, the electron has _____________ from the pull of the atom’s nucleus.
4. For an electron to climb higher in the energy well, it must ABSORB energy. This results in an
increase in POTENTIAL energy. Sources of energy in the PHOTON GAME include:



Bunsen burner
The Sun!
Energy-carrying photons (infrared, visible, and ultraviolet)
5. If an electron FALLS DOWN in the energy well, it will create a
PHOTON of a particular color. This is a conversion of potential
energy to light energy! The energy table shown on each game
board specifies the particular photon ENERGIES that are associated
with various COLORS.
Ex: This drop
of ____ kJ/mol
will create a
_________ colored photon.
6. Your instructor has a set of powerpoint slides which will specify possible changes
for the electron’s position on the game board. For example, a slide may say “jump to
level 4”. Alternatively, the slide may say something like “gain up to 500 kJ/mole of
energy”. You must move your electron within the energy well to follow the changes
that the slides specify.
e-
-600 kJ/mol
-820 kJ/mol
Fi
g
Color
ur
Orange
e
Yellow
3
Green
7. When your team has successfully produced ALL the colors of the rainbow (as well as ALL the
“colors” that lie above and below the visible spectrum, you are a WINNER in the photon game!
Your prize is a pair of photon-viewing glasses (one pair per person).
kJ/mole
191-210
211-230
231-250
#93b: The Photon Game!
Version P (for Practice)
0 kJ/mol
n=5
-100 kJ/mol
n=4
-250 kJ/mol
-430 kJ/mol
n=3
-650 kJ/mol
n=2
A PHOTON is produced
only when an electron
FALLS within the
energy well.
An electron must
reside on one of the
indicated levels (or on
the 0 kJ “freedom”
level. When an
electron jumps from
one level to another, it
is called a QUANTUM
LEAP.
Scoreboard
-910 kJ/mol
As you create
photons, shade in the
boxes here with
appropriate colors!!!!
n=1
Photon
Color
Energy
(kJ/mol)
Infrared
<170
Red
170-190
Orange
191-210
Yellow
211-230
Green
231-250
Blue
251-270
Violet
271-300
UV-A
301-370
UV-B
371-420
UV-C
421-1200
#93c: The Photon Game!
Version C
0 kJ/mol
n=6
-20 kJ/mol
n=5
-80 kJ/mol
n=4
-170 kJ/mol
-280 kJ/mol
A PHOTON is produced
only when an electron
FALLS within the
energy well.
An electron must
reside on one of the
indicated levels (or on
the 0 kJ “freedom”
level. When an
electron jumps from
one level to another, it
is called a QUANTUM
LEAP.
n=3
-460 kJ/mol
n=2
-800 kJ/mol
As you create
photons, shade in the
boxes here with
appropriate colors!!!!
n=1
Scoreboard
Photon
Color
Energy
(kJ/mol)
Infrared
<170
Red
170-190
Orange
191-210
Yellow
211-230
Green
231-250
Blue
251-270
Violet
271-300
UV-A
301-370
UV-B
371-420
UV-C
421-1200
#93d: The Photon Game!
Version D
0 kJ/mol
-20 kJ/mol
n=6
n=5
-60 kJ/mol
n=4
-120 kJ/mol
n=3
-310 kJ/mol
A PHOTON is produced
only when an electron
FALLS within the
energy well.
An electron must
reside on one of the
indicated levels (or on
the 0 kJ “freedom”
level. When an
electron jumps from
one level to another, it
is called a QUANTUM
LEAP.
-530 kJ/mol
n=2
Scoreboard
-1030 kJ/mol
As you create
photons, shade in the
boxes here with
appropriate colors!!!!
n=1
Photon
Color
Energy
(kJ/mol)
Infrared
<170
Red
170-190
Orange
191-210
Yellow
211-230
Green
231-250
Blue
251-270
Violet
271-300
UV-A
301-370
UV-B
371-420
UV-C
421-1200
Assignment #94: The Photon Game Questions
1. A particular atom (such as a helium atom) can emit only certain colors of photons. In other words,
helium atoms might be able to make R, Y, and V photons, but not O, G, or B photons. What is your
explanation for why helium atoms can only emit particular colors of photons?
2. You probably know that ultraviolet “rays” can be damaging to your skin (and eyes). Why do you
suppose UV light is so damaging to skin and eyes?
3. Label each of the following statements as TRUE or FALSE. Explain your reasoning in each case!
Photons can never be created or destroyed
An atom in its GROUND STATE cannot emit a photon
Photons can go through glass
Photons carry energy
Photons can be created only after an atom has GAINED energy
4. Describe the conditions under which each of the following can be a photon producer. Note: a
photon producer is different from a photon reflector. Consider invisible photons (IR and UV). . .
a) The sun
b) A light bulb
c) A TV remote control
d) A glow in the dark Frisbee
e) A hedgehog
5. In order to remember the relative energies of the various colors of the rainbow, an acronym known as
ROY G BIV is sometimes employed. Fill in the spaces in the table below.
Abbreviation
Color name
Wavelength
Energy
(high vs. low)
Long
Low
Short
High
R
O
Y
G
B
I
Indigo
V
6. Add in the “color” that belongs before R and the “color” that belongs after V in the table shown above.
𝐸𝑛 = −
Assignment #95: The Colors of the Rainbow
An introduction to the Balmer Series of photons
1312
𝑘𝐽/𝑚𝑜𝑙
𝑛2
1. Use the Bohr Model equation shown above to
calculate energy values for the first 8 shells of a
hydrogen atom.
Energy
8
-20.5 kJ/mole
E4 =
E3 =
E2 =
Increasing Energy
Shell #
E5 =
7
6
5
4
3
E1 =
2
1
Energy well for a hydrogen atom
2. Using the energy values that you calculated above, find the COLORS of photons produced
from the following electron transitions that could occur within a hydrogen atom:
Transition
Potential Energy Loss
Photon color emitted
31
1166 kJ/mole
Ultraviolet (UV-C)
63
42
3. The visible spectrum of a hydrogen atom consists of only four bright lines. The photons
emitted are red, teal green, and two closely spaced violet lines. Determine the electron
transitions that result in these 4 colors and explain why no other visible colors can be emitted.
Violet (1)
Violet (2)
Green (Teal)
Red
62
292 kJ/mol
Explanation: