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July 31, 2014

July 31, 2014

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

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.

- college-- chemistry -
**Dr Russ**, Monday, February 16, 2009 at 3:50ama) 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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