To answer your question, let's break down each step to calculate energies using the Rydberg equation:

1. Identify the atomic number (Z) for Hydrogen.

- For Hydrogen, Z = 1.

2. Determine n_i and n_f:

a. If calculating energy of light emitted by an electron dropping from higher level 'n' to lower level 'm', then use:

n_i > m

n_i is the initial (higher) state.

b. Conversely, if calculating energy absorbed as an electron jumps up from lower level 'm' to a higher level 'n', then:

n_f > m

n_f is the final (lower) state.

3. Plug in values into the Rydberg equation for Hydrogen:

E = -13.6 eV * '1/n_i^2 - 1/(n_f)^2'

4. Solve for energy 'E'.

For example, if we want to calculate the energy of light emitted when an electron drops from n=3 to n=1 in a hydrogen atom (which is not actually possible with the Bohr model since it predicts that electrons can only transition between specific discrete levels), then:

- Z = 1

- m = 2 (since we're dropping two levels, so this corresponds to going from n_i = 4 down to n_f = 3)

- n_f would be equal to 'm', but in the equation it's written as 'n_f' which is actually referring to our initial state when calculating energy emitted.

So plugging these values into the Rydberg equation:

E = -13.6 eV * '1/(4)^2 - 1/9^2'

= -3.36e-19 J

= (-3.36e-18) J

Therefore, the energy of light emitted would be approximately (-3.36 x 10^-18) Joules.

Please note that this example is simplified as it assumes certain conditions (like only considering two levels and using a specific set of numbers without explanation), but following these steps should give you an idea on how to apply the Rydberg equation in general for calculating energies related to hydrogen atom transitions.

Bohr model of hydrogen atom