Answer the following questions to the best of your ability.
You will receive a grade for completing this
page but your score will only be used for information about
what you may have learned from playing the game. Incomplete
papers will earn a grade that reflects the degree of
incompleteness. Complete papers will receive a 100. You may use
a calculator. All necessary formulas and constants have been
provided. Show all work!
What is the frequency in hertz (Hz)
of light that has an energy per photon of 2.12 ×
10^{-18} J?
What is the wavelength in meters
(m) of light that has a frequency of 4.57 ×
10^{14} Hz?
How many joules (J) equals the
energy of 13.062 eV?
How many electron volts (eV) is
equal to 1.82 × 10^{-19} J?
What is the wavelength of light that
has an energy per photon of 10.205 eV?
How many nanometers (nm) is equal
to 4.34 × 10^{-7} m?
In one or more complete sentences describe what happens
when an electron moves from a higher energy level to a lower
energy level.
In one or more complete sentences describe what is
required for an electron to move from a lower energy level to
a higher energy level.
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Draw a picture showing emission
of light due to a transition between energy levels 5 and
2 using the energy-level diagram shown at left. Draw and
label the electron and the photon in your picture.
Draw a picture showing
absorption of light that causes and transition between energy
levels 3 and 1 using the energy-level diagram shown at left.
Draw and label the electron and the photon in your
picture.
How much energy (in electron volts,
eV) is released or absorbed when an electron moves from
energy level 2 to energy level 5? Energy level 2 is at -3.402
eV and energy level 5 is at -0.544 eV.
What is the relationship between the color of a line in
an atomic emission spectrum and what is happening inside the
atoms?