The wavelength of the spectral lines in the hydrogen atom's emission and absorption spectra are predicted by:
Correct answer: D. Bohr's model
- A. Rutherford's model
- B. Maxwell's model
- C. Dalton's mode
- D. Bohr's model
Explanation
Bohr's model of the hydrogen atom, proposed by Niels Bohr in 1913, successfully explained the observed spectral lines in the hydrogen atom's emission and absorption spectra. It introduced the concept of quantized energy levels for electrons in atoms and postulated that electrons occupy specific orbits around the nucleus. When an electron transitions between these orbits, it emits or absorbs energy in discrete packets called quanta or photons. The energy of these photons is directly related to the difference in energy between the initial and final electron orbits.The wavelength of the spectral lines in the hydrogen atom's emission and absorption spectra can be calculated using the equation:1/λ = R_H * (1/n_final^2 - 1/n_initial^2)where λ is the wavelength of the spectral line, R_H is the Rydberg constant specific to hydrogen, and n_final and n_initial are the principal quantum numbers of the final and initial electron orbits, respectively.
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About Atomic Spectra
Atoms emit or absorb light at specific wavelengths because electrons occupy quantized energy levels and change levels by absorbing or releasing photons. The topic covers emission and absorption spectra, spectral series, hydrogen’s line spectrum, energy-level transitions, and the relation between wavelength, frequency and photon energy.
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