Question

how does Bohr's theory explain the origin of hydrogen spectra? Name the different spectral lines with labelled diagram?​

Answer 1

Answer:

The spectral lines of the atomic emission spectrum of hydrogen are explained by Bohr's hypothesis.

Explanation:

• The electron energy of an atom does not change in the ground state.
• When an atom absorbs one or more energy quanta, the electron jumps from the ground state orbit to an excited state orbit.
• The variable n is used to identify the energy level.
• The first excited state is n = 2, the ground state is n = 1, and so on.
• The energy difference between the two energy levels is equal to the energy received by the atom.  
• When the atom relaxes and returns to a low energy state, it emits energy equal to the energy difference between the two orbitals.
• According to the equation E ≈ hv, the change in energy E emits light at a specific frequency.
• The discovery that the electron orbitals are not evenly spaced is explained by the Bohr model.
• As the energy moves away from the core, the distance between the planes becomes smaller and smaller.
• Using the wavelengths of the spectral lines, Bohr was able to calculate the energy that a hydrogen electron would have at each of its permissible energy levels.

Different spectral lines:

• He found that the four visible spectral lines correlate with the transition from higher energy levels to lower energy levels (n = 2). It is called the Balmer series.
• The Lyman series refers to transitions that end in the ground state (n = 1), but the energy emitted is so high that all spectral lines are in the ultraviolet part of the spectrum.
• Both the Paschen series and Brackett series transitions produce spectral lines in the infrared region because the energy is too low.

Hence, Bohr's theory explains the origin of the hydrogen atom. The four spectral lines are the Balmer series, Lyman series, Passhen series, and Bracket series.

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