Calculate the energy of light emitted as an electron relaxes from the n = 5 to the n = 3 energy level of a hydrogen atom
Answers
Answered by
1
The n = 5 to n = 3 electron transition is part of the Paschen series.
To calculate the energy that corresponds to this specific electron transition you'll have to use the Rydberg equation
E=RE⋅(1n2final−1n2initial), where
RE - the Rydberg constant, equal to 2.78⋅10−18J;
nfinal - the final energy level of the transition;
ninitial - the initial energy level of the transition.
Plug your values into the above equation and solve for E
E=2.178⋅10−18J⋅(132−152)=1.55⋅10−19J
To determine the frequency of the light emitted in this transition, use the relationship that exists between energy, frequency, and Planck's constant
E=h⋅ν, where
h - Planck's constant, equal to 6.626⋅10−34J s
ν - the frequency of the emitted photon.
Solving for ν will give you
ν=Eh=1.55⋅10−19J6.626⋅10−34Js=2.34⋅1015s−1
Hope it's help you
To calculate the energy that corresponds to this specific electron transition you'll have to use the Rydberg equation
E=RE⋅(1n2final−1n2initial), where
RE - the Rydberg constant, equal to 2.78⋅10−18J;
nfinal - the final energy level of the transition;
ninitial - the initial energy level of the transition.
Plug your values into the above equation and solve for E
E=2.178⋅10−18J⋅(132−152)=1.55⋅10−19J
To determine the frequency of the light emitted in this transition, use the relationship that exists between energy, frequency, and Planck's constant
E=h⋅ν, where
h - Planck's constant, equal to 6.626⋅10−34J s
ν - the frequency of the emitted photon.
Solving for ν will give you
ν=Eh=1.55⋅10−19J6.626⋅10−34Js=2.34⋅1015s−1
Hope it's help you
Similar questions