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How can you calculate the frequency of a photon emitted by hydrogen atom given the energy level transition that happens?
Wiki User
∙ 14y ago
To calculate the frequency of the light emitted when an electron in a hydrogen atom makes a transition, simply use change in E = (-2.18*10^-18 J)[1/(nf)^2 - 1/(ni)^2]. Then convert the energy E to frequency using f = E/h where h is Planck's constant 6.626*10^-34 J*s.
Wiki User
∙ 9y ago
Wiki User
∙ 14y agoClassic quantum mechanics-type question. Energy levels are in discrete amounts and only absorb and emit photons of equal energy to the energy absorbed or emitted!
What this means is that the photon energy is equal to the energy level transition that occurs.
So all we need to do here is convert energy into frequency. That's not so bad.
f = E/h so E = fh (where E is your energy in eV, f is the frequency and h is, of course, Planck's constant).
I can't give you a numerical answer since the energy wasn't given but that's how you do it. It's probably helpful to do the same equation with units in place, also.
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