college chemistry
posted by shylo .
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 oneelectron 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^2final1/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.

a) you need to plug the values into the equation to find E, where Z is the atomic number of helium.
b) if Z increases what happens to E? A larger value for Z will give a larger value for E. What is the relationship between E and wavelength? You also need this for your other posting.
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