An electron in an unexcited hydrogen atom acquired an energy of 12.1 eV. To what energy level did it jump? How many spectral lines may be emitted in the course of its transition to lower energy levels? Calculate the corresponding wavelengths.

An electron in an unexcited hydrogen atom acquired an energy of 12.1 e

1.	An electron in an unexcited hydrogen atom acquired an energy of 12.1 eV. To what energy level did it jump? How many spectral lines may be emitted in the course of its transition to lower energy levels? Calculate the corresponding wavelengths.
Answer» Solution :From the formula `epsi=hcR(1/1^(2)-1/n^(2))=13.6(1-1/n^(2))`, We obtain the number of the excited LEVEL: n= 3. Direct transitions from the THIRD level to the first, or second, and from the second to the first level are possible. We obtain three spectral lines.

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An electron in an unexcited hydrogen atom acquired an energy of 12.1 eV. To what energy level did it jump? How many spectral lines may be emitted in the course of its transition to lower energy levels? Calculate the corresponding wavelengths.

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