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In Bohr series of lines of hydrogen spectrum, the third line from the red end corresponds to which one of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen? A)3→2 B)5→2 C)4→1 D)2→5?
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Answer:
The third line from the red end of the hydrogen spectrum corresponds to the transition of the electron from the 4th energy level to the 2nd energy level. Therefore, the correct option is C) 4→1.
Explanation:
The Bohr model of the hydrogen atom involves the electron revolving around the nucleus in circular orbits of definite energy levels. When an electron jumps from a higher energy level to a lower energy level, it emits a photon of energy equal to the difference between the two energy levels. This emitted energy produces a spectral line in the spectrum of hydrogen.
The different energy levels of hydrogen are represented by integer values of 'n', where n = 1 represents the ground state and n = 2, 3, 4, 5, etc. represent the excited states. The third line from the red end of the spectrum of hydrogen corresponds to the transition of the electron from the 4th energy level to the 2nd energy level. This transition is known as the Balmer series and is represented by the following equation:
1/λ = R [1/22 - 1/n2]
where λ is the wavelength of the emitted photon, R is the Rydberg constant, and n is the energy level of the electron. Plugging in the values of n = 4 and n = 2, we get:
1/λ = R [1/22 - 1/42]
1/λ = R [3/16 × 1/4]
1/λ = R [3/64]
1/λ = 3R/64
This equation corresponds to the third line from the red end of the hydrogen spectrum, which is produced by the transition of the electron from the 4th energy level to the 2nd energy level.
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In Bohr series of lines of hydrogen spectrum, the third line from the red end corresponds to which one of the following inter-orbit jumps of the electron for Bohr orbits in an atom of hydrogen? A)3→2 B)5→2 C)4→1 D)2→5?
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