3. Calculate the wavelength, frequency, and energy of a photon emitted by the following
transitions in a hydrogen atom: (Show your work to receive full credit)
6--->5
A)Wavelength(in nm)
B)Frequency (in s^-1)
C) Energy of photon (in J)
Here photon will be emitted
E = R* (1/nf^2 - 1/ni^2)
R is Rydberg constant. R = 2.18*10^-18 J
E = R* (1/nf^2 - 1/ni^2)
E = 2.18*10^-18* (1/5^2 - 1/6^2)
E = 2.664*10^-20 J
Given:
E = 2.664*10^-20 J
use:
E = h*f
2.664*10^-20 J =(6.626*10^-34 J.s)*f
f = 4.021*10^13 Hz
Given:
E = 2.664*10^-20 J
use:
E = h*c/lambda
2.664*10^-20J =(6.626*10^-34 J.s)*(3.0*10^8 m/s)/lambda
lambda = 7.462*10^-6 m
lambda = 7462 nm
Answer:
A) 7462 nm
B) 4.021*10^13 s-1
C) 2.664*10^-20 J
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