Part B What is the energy (in eV ) of a photon, E photon , that is emitted when
ID: 1047633 • Letter: P
Question
Part B
What is the energy (in eV) of a photon, Ephoton, that is emitted when an electron in hydrogen undergoes a transition from the n=4 to the n=2 energy level?
Part C - Use the energy in eV you calculated above this question.
What is the energy of a photon in Joules (J) emitted when an electron in hydrogen undergoes a transition from the n=4 to the n=2 energy level? Report your answer to three significant figures.
Part D - Now that you have the energy of the photon in Joules, use the equation above to:
Calculate the wavelength (in nm) of this transition. Report your answer to three significant figures.
Part F
If an electron moves from the n=2 to the n=4 energy level, energy is absorbed by the atom. Explain this.
Essay answers are limited to about 500 words (3800 characters maximum, including spaces).
Ephoton = Light is a form of electromagnetic radiation. The color (wavelength, ) of light is related to its photon energy, Ephoton, by the equation below ea Planck's constant ( h )-6.626x10-34 Js, Speed of light ( c ) 3.0x108 m/s, wavelength, ( ) measured in meters, m. Experimental evidence has shown that atoms emit different colors of light when their electrons travel from a higher to a lower energy level. Atoms absorbe light when electrons transition from a lower to a higher energy level. The energy of each photon emitted or absorbed is equal to the absolute value of the energy change of the electron Ephotons|Explanation / Answer
From Rydburg's Equation , 1/ = R[(1/ni2) – (1/nf2)]
Where R = Rydburg's constant = 10.96 x106 m-1
= wavelength = ?
ni = 2
nf = 4
Plug the values we get
1/ = 10.96 x106 x[(1/22) – (1/42)]
= 2.055x106
= 4.87x10-7 m
So Energy , E = hc/
Where
h = plank's constant = 6.625x 10-34 Js
c = speed of light = 3x 108 m/s
Plug the values we get E = (6.625x 10-34 Jsx3x 108 m/s) / (4.87x10-7 m)
= 4.08x10-19 J
Do the remaining in the similar manner