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**Problem**: What is the wavelength (in nm) of light emitted from a hydrogen atom when an electron falls from the n = 5 to n = 2 energy level?a. 780b. 656c. 486d. 434e. 308

###### FREE Expert Solution

We’re being asked to calculate for the wavelength of light emitted by an electron to transition from n=5 to n = 2.

We’re going to use the **Balmer Equation** which relates wavelengths to a photon’s electronic transitions.

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

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 ****wavelength of light emitted ****(****λ):**

###### Problem Details

What is the wavelength (in nm) of light emitted from a hydrogen atom when an electron falls from the n = 5 to n = 2 energy level?

a. 780

b. 656

c. 486

d. 434

e. 308

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 .

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