Problem: Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 3 to n = 1 energy level, based on the Bohr theory. Use the equation En = -2.18 x 10 -18 J [(1/nf2)-(1/ni2)]a. 2.92 x 1015 s-1b. 3.56 x 1014 s-1c. 2.92 x 1014 s-1d. 1.17 x 1015 s-1

FREE Expert Solution
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FREE Expert Solution

We will calculate the frequency of the light emitted by a hydrogen atom from the energy using the following equation:

E = energy, J/photon
h = Planck' s constant = 6.626x10-34 J
s
ν = frequency


Let’s first calculate the energy of the hydrogen atom using the given Bohr Equation:

ni = initial energy level
nf = final energy level

93% (114 ratings)
Problem Details

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 3 to n = 1 energy level, based on the Bohr theory. Use the equation En = -2.18 x 10 -18 J [(1/nf2)-(1/ni2)]

a. 2.92 x 1015 s-1

b. 3.56 x 1014 s-1

c. 2.92 x 1014 s-1

d. 1.17 x 1015 s-1

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