# Wavelength of a photon

Kennedy111

## Homework Statement

Calculate the shortest wavelength photon that is emitted in the hydrogen atom.

Energy when n = 1 = -13.6 eV

E = hc/λ
λ = hc/E

## The Attempt at a Solution

Well as far as I understand, when the electron is in the n = 1 energy level it has it's lowest energy, which is -13.6 eV. I believe this is where the shortest wavelength will be...
λ = hc/E
= (4.14 x 10^-15 eV*s)(3.00 x 10^8 m/s) / -13.6 eV
= approx 9.13 x 10^-8 m

Was my method correct? I would really just like a second opinion. Thank you!

Homework Helper
The method is correct, but the photon energy is positive: 13.6 eV, the same the electron loses when it becomes bounded to the hydrogen atom. You divided by -13.6 eV, then ignored the sign, which is wrong.

ehild

apelling
Are n't photons produced when an electron jumps between energy levels not stay on one level? The shortest wavelength photon will be the one with least energy produced by an electron transition of the smallest energy. If the electron is to end up at n=1, the shortest wavelength photon comes from a jump from n=2 to n=1 (-3.4eV to -13.6eV).

apelling
Sorry I have just realized my mistake. Shortest wavelength comes from the largest energy not the smallest.