Consider an electron transitioning between two orbits in a hydrogen atom. If the wavelength of the energy emitted is 4055 nm, what is the difference in energy between the orbits? Express your answer as a positive number using scientific notation in the following format: 1.25e16 (3 significant figures) or 1.25e-16 (3SF w/a negative exponent).
Several scientists contributed to our understanding of the energy emissions resulting from electron transitions in the hydrogen atom. The four emission series are named as the Lyman series, the Balmer series, the Paschen series, and the Bracket series in their honor.
Consider an electron transitioning between two orbits in a hydrogen atom. If the wavelength of the energy emitted is 4055 nm, what is the difference in energy between the orbits? Express your answer as a positive number using scientific notation in the following format: 1.25e16 (3 significant figures) or 1.25e-16 (3SF w/a negative exponent).
Given : Wavelength of the energy emitted = 4055 nm
Since 1 nm = 10-9 m
Hence wavelength of the energy emitted in m = 4055 X 10-9 m
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