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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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?
Solution Preview
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 ...
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