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

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 .

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}):**

Bohr and Balmer Equations

Bohr and Balmer Equations

Bohr and Balmer Equations

Bohr and Balmer Equations