Explain an electron in the hydrogen atom makes a transition

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An electron in the hydrogen atom makes a transition from an energy state of principle quantum number n to the n=1 state. If the photon emitted has a wavelength of 95nm, what is the value of n?

On this problem I tried using the equation 1/wavelength = R (1/n^2 - 1/n^2)
= 1/ (9.5x10^8m) = 1.097x10^7 m^-1 (1/1 - 1/n^2)
Not sure if im using the wrong equation, or if im getting tripped up in the math, but I am not getting the answer I am looking for.

One of the lines in the Lyman series of the emission spectrum for hydrogen results when an excited electron in the n=2 level returns to ground state. What is the energy in kJ of the photon emitted when this transition occurs.

So far I have:

E = Ef - Ei
E = hv = -2.18 x 10^-18J(1/1 - 1/4)
= -2.18x10^-18J (.75)
= -1.635 x 10^18 J x 1kJ/1000J =

Reference no: EM13515833

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