# 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

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 ###### 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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Bohr and Balmer Equations concept. If you need more Bohr and Balmer Equations practice, you can also practice Bohr and Balmer Equations practice problems.

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Based on our data, we think this problem is relevant for Professor Sandusky's class at URI.