The energy levels for a Bohr atom are shown below. -0.54eV -0.85eV -1.51eV -3.40eV -13.6eV   An electron absorbs a photon of wavelength 4008 nm. What transition did the electron make? (h = 6.626 x 10-34, 1 eV = 1.6 x 10-19 J)   from 5 to 4   from 4 to 2   from 4 to 5   from 2 to 4

Principles of Physics: A Calculus-Based Text
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Chapter11: Gravity, Planetary Orbits, And The Hydrogen Atom
Section11.5: Atomic Spectra And The Bohr Theory Of Hydrogen
Problem 11.4QQ
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The energy levels for a Bohr atom are shown below.

-0.54eV

-0.85eV

-1.51eV

-3.40eV

-13.6eV

 

An electron absorbs a photon of wavelength 4008 nm. What transition did the electron make? (h = 6.626 x 10-34, 1 eV = 1.6 x 10-19 J)

 
from 5 to 4
 
from 4 to 2
 
from 4 to 5
 
from 2 to 4
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