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This question is really confusing me. Okay here it is:
What is the energy of an electron in the second principal energy level of a He+ ion>
Answer is:
B) -2.18E-18 J
We use the equation given in the passage:
En= -Rh( (Z^2)/(n^2))
Rh is the Rydberg Constant equaling 2.18E-18 J. n= principal quantum number.
My question here is why is Z=2 in this equation? My reasoning is that since He+ is an ion, it only has 1 electron, and its nuclear charge would be protons-electrons not in valence shell, therefore it would be 2-0 because there is still one electron and it is in the valence shell. Can someone help clear this up for me? Thanks a lot!
What is the energy of an electron in the second principal energy level of a He+ ion>
Answer is:
B) -2.18E-18 J
We use the equation given in the passage:
En= -Rh( (Z^2)/(n^2))
Rh is the Rydberg Constant equaling 2.18E-18 J. n= principal quantum number.
My question here is why is Z=2 in this equation? My reasoning is that since He+ is an ion, it only has 1 electron, and its nuclear charge would be protons-electrons not in valence shell, therefore it would be 2-0 because there is still one electron and it is in the valence shell. Can someone help clear this up for me? Thanks a lot!
