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

**$\overline{){\mathbf{\u2206}}{\mathbf{E}}{\mathbf{=}}{\mathbf{-}}{{\mathbf{R}}}_{{\mathbf{H}}}\mathbf{(}\frac{\mathbf{1}}{{\mathbf{n}}_{\mathbf{final}}^{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{n}}_{\mathbf{initial}}^{\mathbf{2}}}\mathbf{)}}$**

ΔE = energy related to the transition, J/atom

R_{H} = Rydberg constant, 2.178x10^{-18} J

n_{i} = initial principal energy level

n_{f} = final principal energy level

Calculate **ΔE**:

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

What professor is this problem relevant for?

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

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 Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.