Can someone explain why the transition from n = 4 to n = 2 emits radiation of longer wavelength than the transition from n = 5 to n = 1?
Thank you!
Atomic Spectra
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Re: Atomic Spectra
I think this is because a smaller amount of energy is emitted when an electron goes from n=4 to n=2 compared to going from n=5 to n=1 since the energy difference is smaller. This energy can be represented by E=hv, from which the equation E=(ch)/wavelength, or wavelength=(ch)/E, can be derived. From the latter equation, we can see that as E decreases, the wavelength increases. Therefore, an electron going from n=4 to n=2 will emit radiation of a longer wavelength then that of an electron going from n=5 to n=1.
Hope this helps!
Hope this helps!
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Re: Atomic Spectra
Just to reiterate, when the energy difference is smaller, wavelength is larger, and frequency is lower.
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Re: Atomic Spectra
Since energy is directly proportional to frequency, its inversely related to wavelength (c = wavelength x freq and E = planks constant (h) x freq ==> derive (E = hc/wavelength) by plugging in for freq). There is a greater change in energy from n =5 to n = 1 than n = 4 to n = 2, so the transition from 5 to 1 gives off a smaller wavelength than the one from 4 to 2. Does that make sense? It's really just thinking about the equations and how the variables relate to each other.
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Re: Atomic Spectra
You can use the formula to calculate the different energy and thus compare. Concrete number is the answer. Hope this will help.
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