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The following values are the only energy levels of a hypothetical one-electron atom:
E₆ = -2×10⁻¹⁹J E₅ = -7×10⁻¹⁹J
E₄ = -11 ×10⁻¹⁹J E₃ = -15 ×10⁻¹⁹J
E₂ = -17 ×10⁻¹⁹J E₁ = -20×10⁻¹⁹J
(a) If the electron were in the n = 3 level, what would be the highest frequency (and minimum wavelength) of radiation that could be emitted?

Respuesta :

  • "n=3 to n=2 to n=1" will be the range for both the maximum and the minimum frequency.
  • In this electronic setup, there won't be any energy development from n=3 to n=1 since all electronic stages below n=3 contain energy that is almost equal.

What is Emission Radiation?

  • When the excited electron transitions back to a lower electron orbital, emission takes place.
  • The radiation that is emitted is known as luminescence. At energies equal to or lower than the energy corresponding to the absorbed radiation, luminescence can be seen.
  • After initial absorption, one of two pathways can lead to emission.
  • Alpha particles, beta particles, and gamma rays are the three most prevalent forms of radiation.
  • It can be created artificially or by unstable atoms that experience radioactive decay.
  • From its source, radiation spreads outward as energetic waves or particles. Radiation comes in a variety of forms, each with its own characteristics and impacts.

Learn more about radiation here:

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