Problem: An atomic emission spectrum of hydrogen shows the following three wavelengths: 1875 nm, 1282 nm, and 1093 nm. Assign these wavelengths to transitions in the hydrogen atom.For nm = 1282 { m nm}.

🤓 Based on our data, we think this question is relevant for Professor Wambsgans' class at DREXEL.

FREE Expert Solution

We’re being asked to assign 1282 nm to transitions in the hydrogen atom.

We can see that the three wavelengths correspond to Paschen/Bohr series with nfinal = 3


1λ=RZ21n2final-1n2initial

λ = wavelength, m
R = Rydberg constant = 1.097x107 m-1 
Z = atomic number of the element
ninitial = initial energy level
nfinal = final energy level


Calculate the initial energy level (ninitial):

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Problem Details

An atomic emission spectrum of hydrogen shows the following three wavelengths: 1875 nm, 1282 nm, and 1093 nm. Assign these wavelengths to transitions in the hydrogen atom.

For nm = 1282 .

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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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Wambsgans' class at DREXEL.