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**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

###### 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**:

n_{i} = initial energy level

n_{f} = final energy level

###### 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 E_{n} = -2.18 x 10^{ -18} J [(1/n_{f}^{2})-(1/n_{i}^{2})]

a. 2.92 x 10^{15} s^{-1}

b. 3.56 x 10^{14} s^{-1}

c. 2.92 x 10^{14} s^{-1}

d. 1.17 x 10^{15} s^{-1}

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