Name: Date: ______ Electromagnetic Radiation Worksheet E = hv

```Name: _________________
Date: _______
E = hv
This formula shows the relationship between the energy (E, measured in joules) and
frequency (v, measured in 1/s or s-1) of light. Energy is directly proportional to frequency.
h is called Planck’s Constant, and equals 6.626*10-34J*s.
c = λv
This formula shows the relationship between the frequency (v) and the wavelength (λ,
pronounced lambda) of light. Frequency is inversely proportional to wavelength. c is the
speed of light, and equals 3.00*108m/s.
1. What is the energy of a photon with a frequency of 7.23*1014s-1
2. If a photon carries 1.2*10-19J of energy, what is its frequency?
3. What type of light is the photon in question 2? (Use the electromagnetic spectrum on
the back.)
4. What is the wavelength of electromagnetic radiation with a frequency of 4.6*1014s-1?
5. What color is the light in question 4?
6. Use the emission model for hydrogen on the back of this sheet to fill in the following
table with the wavelength of light (in nanometers) that would be released by an electron
falling from the initial level to the final level.
Final Energy Level
3
Initial Energy
Level
2
1
6
x
5
x
4
3
x
2
x
x
Bohr Model for Hydrogen Atom
(measurement in nanometers)
n
n
n
n
n
=
=
=
=
=
6
5
4
3
2
n=1
UV = Ultraviolet
IR = Infrared
1282
656 434
1094
1875
IR
486
410
Visible
122 97
103
UV
Electromagnetic Spectrum
(measurement in meters)
104 103 102 101 100 10–1 10–2 10–3 10–4 10–5 10–6 10–7 10–8 10–9 10–1010–1110–12 10–13
X rays
Microwaves
Infrared
Ultraviolet
Gamma
rays
waves
Shorter Wavelength
Longer Wavelength
Visible Light
Red
Orange
Yellow
Green
Blue
Violet
7.0 ! 10 –7 6.5 ! 10 –7 5.9 ! 10 –7 5.7 ! 10–7 4.9 ! 10 –7 4.2 ! 10 –7 4.0 ! 10–7
NCDPI Reference Tables for Chemistry (2012)
Page 8
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