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### Atomic Spectra

Posted: Wed Oct 17, 2018 10:25 pm
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!

### Re: Atomic Spectra

Posted: Wed Oct 17, 2018 10:39 pm
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!

### Re: Atomic Spectra

Posted: Wed Oct 17, 2018 11:20 pm
Just to reiterate, when the energy difference is smaller, wavelength is larger, and frequency is lower.

### Re: Atomic Spectra

Posted: Thu Oct 18, 2018 3:25 pm
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.

### Re: Atomic Spectra

Posted: Sat Oct 20, 2018 9:09 pm
You can use the formula to calculate the different energy and thus compare. Concrete number is the answer. Hope this will help.