I am not sure how to do this???? For hydrogen-like atoms, the energy level for a
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I am not sure how to do this????
For hydrogen-like atoms, the energy level for a given quantum number n is En = z2/n2(-13.6 eV) This is Equation 30.26 in the OpenStax textbook. Doubly-ionized lithium is a hydrogen-like atom. The Balmer series of hydrogen comprises those transitions which end at n = 2. Which energy level (value of n) in doubly-ionized lithium has the same energy as the n = 2 level of hydrogen? Consider the hydrogen transition n = 5 to n = 2, which gives off a photon of wavelength 434 nm. We wish to find a transition in doubly-ionized lithium which will produce a photon of the same wavelength. The final n value will be the same as your answer above. What would the initial n value of this transition (in lithium) be?Explanation / Answer
9/x^2 = 1/2^2, n = 6
(1/2^2 - 1/5^2) = 9 (1/6^2 - 1/x^2), n = 15
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