Posted by **shylo** on Monday, February 16, 2009 at 3:26am.

I got stuck on this problem and I cannot figure out what to do or explain this problem. Please help me with this problem.

The emission lines of one-electron atoms and ions can all be fit to the equation describing the spectrum of the hydrogen atom:

E= -(2.18X10^-18J)Z^2(1/n^2final-1/n^2initial) where Z is the atomic number.

a) calculate the energy (in J) of one photon associated with the transition of the electron in He^+2 from n=2 to n=1.

b) As the value of Z increases, does the wavelength of the photon associated with the transition from n=2 to n=1 increase or decrease? Explain.

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