asked by @jds1 •
almost 2 years ago •
Chemistry
• 5 pts

What is the wavelength of a photon emitted from a hydrogen atom when an electron drops from the n=6 to the n=1 level? Hint: use the Rydberg formula.

```
109.351 nm
67.8999 nm
222.453 nm
0.0937901 nm
93.76 nm
131.226 nm
```

Please select all the following statements that are true concerning absorption and emission spectra. An emission spectrum is created when a sample of excited gas emits particular frequencies of light. By looking at each spectrum, we can see that the electrons move between discrete energy levels, resulting in specific wavelengths associated with each transition. An absorption spectrum is created when a sample of excited gas emits particular frequencies of light. If the energy of the electron is increasing, then there must be an emission of light energy. Conversely, if the energy of the electron is decreasing, then there must be an absorption of light energy. For a particular chemical, its absorption and emission spectra show the same discrete line patterns.

Hey! In this problem, we will be using the **Rydberg Formula** to solve for the missing wavelength.
1/λ = R(1/nf^2 - 1/ni^2).

We know that the R constant for this problem is 1.097 x 10^7 m^-1. Then we know that our initial n (ni) is n=6 as mentioned in the problem. We are then going to n=1 (this is our nf). So we have everything to plug in to solve for our wavelength (λ).

When we plug everything in carefully on the calculator, we get

1/λ = 1.067 x 10^7 m^-1.

When we solve for λ, we get 9.4 x 10^-8 m. But, the answer is needed in nm, not m, so we must convert. We multiply this number that we got by 10^9 nm/ 1 m, and we obtain **93.76 nm**, which in this case is the 5th answer choice. Hope that helped!

answered by @sabrina •
almost 2 years ago

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