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Solution of energy transfer for orbital electron

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How much energy will an electron in orbit about a hydrogen atom lose in a transition from orbit # 2 to orbit # 4, where orbits are counted from the closest outward? If this lost energy is carried away by a photon, what will be its wavelength?

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you can work out the energy (in eV) difference between two energy levels (Hydrogen atom) defined by principal quantum numbers, n1, n2 by the equation

E = -13.6 (1/n1^2- 1/n2^2) eV

Thus for level n1 = 2, n2 = 4

E = -13.6 (1/2^2 - 1/4^2) = -13.6(0.25 - 0.0625) = -2.55 ...

Solution Summary

Itis shown how to determine How much energy an electron in orbit about a hydrogen atom loses in a transition from orbit # 2 to orbit # 4, where orbits are counted from the closest outward? Considering that this energy is carried away by a photon, the photons wavelength is deduced?

$2.19