An equation resembling the Balmer-Rydberg equation shown below, where Z is the atomic number, can be used to describe the orbital energies of single-electron atoms or ions, such as Li⁺. 

What wavelength of light in nanometers is released when the electron in Li⁺ falls from n = 4 to n = 2?

Radiation with a wavelength of 92.315 nm is emitted by a hydrogen atom. What are the initial and final n values that correspond to this emission?

For the Balmer series (n_f = 2), what are the wavelengths in nm of the emission lines for n _i = 6, 7, 8?

For the Lyman series (n_f = 1), what are the wavelengths in nm of the emission lines for n _i = 5, 6, 7?

For the following electronic transitions in a hydrogen atom, find the frequency of the light emitted:

a. n = 3 → n = 2
b. n = 6 → n = 4
c. n = 4 → n = 1
d. n = 5 → n = 2

Three wavelengths are observed from an atomic emission spectrum of hydrogen. They are 97.23 nm, 102.6 nm, and 94.96 nm. What is their corresponding electronic transition?

What is the energy in Joules needed to excite a hydrogen atom via an electronic transition from n = 1 to n =3 principal energy level?