Q1)
Calculate the energy of an electron in the n =
2 level of a hydrogen atom.
Energy = _______Joules
Q2)
What would be the wavelength of radiation emitted from a hydrogen atom when an electron moves from the n = 2 to n = 1energy level? In what region of the spectrum does this radiation lie?
Wavelength = ________nm
Region = _________(ultraviolet or visible or infrared)
1)
Energy in eV in nth level is given by:
En = -13.6/n^2
for n=2,
E = -13.6/2^2 eV
E = -13.6/4 eV
E = -3.4 eV
E = -3.4*1.602*10^-19 J
E = 5.45*10^-19 J
Answer: 5.45*10^-19 J
2)
Here photon will be emitted
1/lambda = R* (1/nf^2 - 1/ni^2)
R is Rydberg constant. R = 1.097*10^7
1/lambda = R* (1/nf^2 - 1/ni^2)
1/lambda = 1.097*10^7* (1/1^2 - 1/2^2)
lambda = 1.215*10^-7 m
lambda = 122 nm
Answer: 122 nm
this wavelength is less than wavelength of violet rays
So, this is ultraviolet
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