Question

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.

Answer 1

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.