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 already know about the topics covered on this
pre-test. 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 of light that
has an energy per photon of 1.94 × 10-18
J?
What is the wavelength of light
that has a frequency of 1.38 × 1014
Hz?
How many joules (J) equals the
energy of 5.34 eV?
How many electron volts (eV) is
equal to 1.63 × 10-18 J?
What is the wavelength of light that
has an energy per photon of 2.858 eV?
How many nanometers (nm) is equal
to 6.57 × 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.
turn page
over
page break
Draw a picture showing emission
of light due to a transition between energy levels 6 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 4 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 1 to energy level 6? Energy level 1 is at
-13.606 eV and energy level 6 is at -0.378 eV.
What is the relationship between the color of a line in
an atomic emission spectrum and what is happening inside the
atoms?
