Rydberg equation for the hydrogen atom, which looks like this

Here

• λe is the wavelength of the emitted photon (in a vacuum)
• R is the Rydberg constant, equal to 1.097⋅107 m−1
• n1 represents the principal quantum number of the orbital that is lower in energy
• n2 represents the principal quantum number of the orbital that is higher in energy

In your case, you have

This implies that the Rydberg equation will take the form

which, in your case, will get you

Rearrange to solve for the wavelength

Plug in the value you have for R to get

Now, in order to find the energy that corresponds to this transition, calculate the frequency, ν, of a photon that is emitted when this transition takes place by using the fact that wavelength and frequency have an inverse relationship described by this equation

Here

• ν is the frequency of the photon
• c is the speed of light in a vacuum, usually given as 3⋅108 m s−1

Rearrange to solve for the frequency and plug in your value to find

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