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ne of the lines in the hydrogen emission atom spectrum has a wavelength of 486.1 nm. if this electron ends in the n=2 energy level, what energy level did it start in?

User Clark Bao
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Final answer:

The question pertains to the Hydrogen Emission Spectrum in physics. The electron in question moved to the n=2 energy level, emitting a light wavelength of 486.1 nm. Using the Rydberg formula, it was likely at the n=4 energy level originally.

Step-by-step explanation:

The question you asked relates to the hydrogen emission spectrum, a key concept in quantum physics. The electron you mentioned changes its energy level from a higher to a lower state, in this case, to the n=2 level. The excess energy results in the emission of light, with a wavelength related to the difference in energy levels. We use the Rydberg formula to calculate these energy levels:

Rydberg Formula: 1/λ = R*(1/n12 - 1/n22) where R is the Rydberg constant ≈ 1.097 x 107 m-1. From the formula, solve for n1, where n2 = 2 and λ = 486.1 nm.

Performing the calculations, the electron likely originated in the n=4 energy level.

Learn more about Hydrogen Emission Spectrum

User John Hanley
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