1. How many possibilities exist for emission spectral lines when a hydrogen atom's electron in the n = 4 quantum level of a Bohr atom drops to the ground state (i.e. n = 1)? Use a diagram to illustrate each of the possible transitions responsible for the spectral lines.

2. Use the Rydberg equation to calculate the wavelength in nm of the light emitted when the electron in a hydrogen atom undergoes a transition from n= 6 to n = 2. Consult figure in your textbook to determine the color of light emitted.

3. Calculate the energy in units of Joules for each photon of light in the spectral line in question #2, above = / , h= Planck's constant = 6.626 x 10-34 J.s