Although the isotopes of hydrogen are the only neutral one-electron bound atomic

Question

Although the isotopes of hydrogen are the only neutral one-electron bound atomic systems, one-electron ions do exist and are important, particularly in the physics of stellar atmospheres, where the high temperatures can lead to multiple ionization of atoms. We saw in Chapter 1 of QPI that Bohr’s semi-classical model of the hydrogen atom led to the correct expression for the allowed energy levels of one-electron ions, in spite of the model’s inadequacies.

(a) Following Bohr’s model, derive an expression for the allowed energy levels of an electron bound to a nucleus of charge +Ze. At each stage, state explicitly any laws, postulates or assumptions you employ. Express your answer in terms of the energy E1 of the first Bohr orbit in hydrogen.

(b) Singly-ionized helium is referred to by spectroscopists as He II. Use your result from part (a) to calculate the ground-state energy of He II. Compare this with the ground-state energy of an electron in neutral helium (He I; see Figure 3.35 in QPI). What is the reason for the difference?

Explanation / Answer

Hmmmm...maybe I am beinga bit thick but how does the answer given above answer the question? I can see nothing in th elink directly correlated to Bohr's model?

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