D. The Balmer Series

1. When Balmer found his famous series for hydrogen in 1886, he was limited experimentally to wavelengths in the visible and near ultraviolet regions from 250 nm to 700 nm, so all the lines in his series lie in that region.

Based on the entries in Table 2 and the transitions on your energy level diagram, what common characteristic do the lines in the Balmer series have?

What would be the longest possible wavelength for a line in the Balmer series?
λ = ___________nm

What would be the shortest possible wavelength that a line in the Balmer series could have? Hint: What is the largest possible value of ΔE to be associated with a line in the Balmer series?

λ = ___________nm

The Ionization Energy of Hydrogen

1. In the normal hydrogen atom the electron is in its lowest energy state, which is called the ground state of the atom. The maximum electronic energy that an electron in a hydrogen atom can have is 0 kJ/mole, at which point it would essentially be removed from the atom and it would become a H+ ion. How much energy in kilojoules per mole does it take to ionize a hydrogen atom?

______________ kJ/mole

The ionization energy of hydrogen is often expressed in units other than kJ/mole. What would it be in joules per atom? in electron volts per atom? (1 ev = 1.602 x 10-19 J)

______________J/atom; _____________ ev/atom