Can someone please help me solve this?

The Lyman series in the hydrogen atom consists of transitions to the n=1 level that take place in the ultraviolet part of the spectrum. Calculate the wavelength of the light emitted due to the lowest energy transition of this series between n=2 and n=1levels.
I know this is set up so that you have 1/wavelength=1.097x10^-2m^-1[(1/n1^2)-(1/n2^2)], but I'm not sure how to plug in the numbers. Help!

Question

Can someone please help me solve this?

The Lyman series in the hydrogen atom consists of transitions to the n=1 level that take place in the ultraviolet part of the spectrum. Calculate the wavelength of the light emitted due to the lowest energy transition of this series between n=2 and n=1levels. 
I know this is set up so that you have 1/wavelength=1.097x10^-2m^-1[(1/n1^2)-(1/n2^2)], but I'm not sure how to plug in the numbers. Help!

jfraser · Answer

plug in n=1 for n1 and n=2 for n2 and solve for 1/wavelength, then invert it