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## Hydrogen Atom Game Pre-test

 Speed Formula c = λf Planck’s Formula E = hf Speed of Light (c) 3.00 × 108 m/s Planck’s Constant (h) 6.626 × 10-34 J· s 1 electron volt (eV) = 1.602 × 10-19 J 1 m = 1 × 109 nm 1 m = 1 × 106 µm

1. What is the frequency of light that has an energy per photon of 1.94 × 10-18 J?
1. What is the wavelength of light that has a frequency of 1.38 × 1014 Hz?
2. How many joules (J) equals the
energy of 5.34 eV?
3. How many electron volts (eV) is
equal to 1.63 × 10-18 J?

1. What is the wavelength of light that has an energy per photon of 2.858 eV?
2. How many nanometers (nm) is equal
to 6.57 × 10-7 m?
3. In one or more complete sentences describe what happens when an electron moves from a higher energy level to a lower energy level.

1. 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 1. 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. 1. 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.

1. 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.
2. What is the relationship between the color of a line in an atomic emission spectrum and what is happening inside the atoms?
Examples for the calculations required in this game
Rules for Referees
Score Sheet
Backs of Playing Cards
Playing Cards Page 1
Playing Cards Page 2
Playing Cards Page 3
Playing Cards Page 4
Hydrogen Atom Energy Level Diagram Playing Board
Emission and Absorption Spectra page
Post-test
Last updated: Apr 29, 2010        Home