# Problem: Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by n = 1, by n = 2.

🤓 Based on our data, we think this question is relevant for Professor Yang's class at UT.

###### FREE Expert Solution

We can determine Δ E first using the Bohr Equation shown below:

$\overline{){\mathbf{∆}}{\mathbf{E}}{\mathbf{=}}{\mathbf{-}}{{\mathbf{R}}}_{{\mathbf{H}}}\mathbf{\left(}\frac{\mathbf{1}}{{\mathbf{n}}_{\mathbf{final}}^{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{n}}_{\mathbf{initial}}^{\mathbf{2}}}\mathbf{\right)}}$

ΔE = energy related to the transition, J/atom
RH = Rydberg constant, 2.178x10-18 J
ni = initial principal energy level
nf = final principal energy level

Calculate ΔE:

###### Problem Details

Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by n = 1, by n = 2.

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 Periodic Trends: Ionization Energy concept. You can view video lessons to learn Periodic Trends: Ionization Energy. Or if you need more Periodic Trends: Ionization Energy practice, you can also practice Periodic Trends: Ionization Energy practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Yang's class at UT.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.