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 n_{final }= 3

$\overline{)\frac{\mathbf{1}}{\mathbf{\lambda}}{\mathbf{=}}{{\mathbf{RZ}}}^{{\mathbf{2}}}\left(\frac{\mathbf{1}}{{{\mathbf{n}}^{\mathbf{2}}}_{\mathbf{final}}}\mathbf{-}\frac{\mathbf{1}}{{{\mathbf{n}}^{\mathbf{2}}}_{\mathbf{initial}}}\right)}$

λ = wavelength, m

R = Rydberg constant = 1.097x10^{7} m^{-1}

Z = atomic number of the element

n_{initial }= initial energy level

n_{final} = final energy level

**Calculate the initial**** energy level**** ****(n _{initial}):**

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 .

Frequently Asked Questions

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 Equation concept. You can view video lessons to learn Bohr Equation. Or if you need more Bohr Equation practice, you can also practice Bohr Equation 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.