I am resubmitting because my answer is different from my original answer. I had

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I am resubmitting because my answer is different from my original answer. I had to send it a second time because the answers were hard to read. please write clearly. thanks so much

1. The emission spectrum of hydrogen can be divided up into series, which represent particular electronic transitions in the H atom from higher energy levels to the same lower energy level. For instance, the Paschen series consists of transitions from energy levels with n > 3 to the n 3 energy level. a. What transition in the Paschen series would result in the emission of a photon with a wavelength of 1875 nm? (Hint: What energy level does the electron end up in? What do you know about transitions in the H atom?) b. The Lyman series consist of transitions from energy levels with n > 1 to the n = 1 energy level. If an electron starts in the n-6 energy level initially, how does the wavelength of the photon emitted in the Paschen series compare to the wavelength of the photon emitted in the Lyman series? Explain your answer

Explanation / Answer

a. it is n=4 to n=3 transition.

wavenumber(1/l) = 109737(1/n1^2 - 1/n2^2)   (n2>n1)

rydberg constant = 109737 cm-1

wavenumber = 1/ wavelength(l)

   l = wavelength = 1875*10^-7 cm

    n1 = 3 (paschen series) , n2 = x

(1/(1875*10^-7)) = 109737((1/3^2)-(1/x^2))

x = 4

so that, it is n=4 to n=3 transition.

b.

wavenumber(1/l) = 109737(1/n1^2 - 1/n2^2)   (n2>n1)

rydberg constant = 109737 cm-1

wavenumber = 1/ wavelength(l)

   l = wavelength = 1875*10^-7 cm

    n1 = 1 (lyman series) , n2 = 6

(1/(l)) = 109737((1/3^2)-(1/6^2))

l = 1.09*10^-4 cm = 1090 nm

compared to paschen series, lyman series wavelength is less,

means energy associated with the lyman series transion is high.

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