# Calculating energy level from wavelength

The transition of an electron from a higher level to a lower level results in the emission of a photon of wavelength $350.0\ \mathrm{nm}$. If the energy of the higher level is $-3.24\times10^{-19}\ \mathrm J$, calculate the energy of the lower level.

By using $E = h\nu$

I find $E = 5.679\times10^{-28}\ \mathrm J$

How do I use this value to solve the qus?

Using these data, the energy of a photon with $\lambda = 350\ \mathrm{nm}$ calculates to:
$$\mathrm{E} = \frac{6.62606957 \cdot 10^{-34} \cdot 2.99792458 \cdot 10^8}{350 \cdot 10^{-9}} \cdot \frac{\mathrm{J \cdot s \cdot m}}{\mathrm{s \cdot m}} = 0.05676 \cdot 10^{-17} \mathrm{J} = 5.676 \cdot 10^{-19} \mathrm{J}$$
• @Kenny Almost, you're calculating the energy of a photon with $\lambda$ = 350 nm. This is the difference to the other level for which the energy was given. – Klaus-Dieter Warzecha Nov 17 '14 at 18:04