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What wavelength should the astrophysicist look for to detect a transition of an electron from the n equals 7 to the n equals 3 level?
Wiki User
∙ 10y ago
,
Use Rydberg's Equation to solve for this problem, which is as follows:
1/wavelength = R((1/n2x )-(1/ny2 ))
Where R is Rydberg's constant, 1.0974 * 107 m-1
And where nx is the lower energy state (n=1), and ny is the higher energy state (n=3).
So, plugging in those values gives us the following calculations to be made:
1/(12)=1, and 1/(32)= 1/9, so (1) - (1/9) = 8/9.
So, we get:
1/wavelength = (1.0974* 107 m-1)(8/9)
=
1/wavelength = (.9754666667 m-1)
=
wavelength = 1/(.9754666667 m-1)
=
Wavelength = 1.025150355 * 10-7 m
And, since wavelength is typically given in nanometers (1 nm = 1 * 10-9 m) when looking at hydrogren emission spectra, convert the 10-7to 10-9 by moving the decimal back two more places.
So,
The wavelength expected for light composed of photons produced by an n=3 to n=1 transition in a hydrogen atom is:
102.5150355 nm
or, to three significant figures,
103 nm
Hope I helped!
I am an engineering student at the University of Arizona.
Wiki User
∙ 8y ago
Wiki User
∙ 14y agoWhat wavelength should the astrophysicist look for to detect a transition of an electron from the to the level?
Wiki User
∙ 12y ago1.00*10^-6 m
Wiki User
∙ 13y agoIn what atom? Need a Z number.
Wiki User
∙ 10y ago1.00*10^-6
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