Calculating energy level from wavelength


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> 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.
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By using $E = h\nu$


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


How do I use this value to solve the qus? 




All you need are two equations and two constants (speed of light and Planck constant):
\begin{eqnarray}
\mathrm{E} & = & h\nu\\
h & = & \mathrm{6.62606957 \cdot 10^{−34} J\cdot s}\\
\mathrm{c} & = & \lambda\nu\\
\mathrm{c} & = & 299792458\ \mathrm{m\cdot s}^{-1}\\
\end{eqnarray}


Using these data, the energy of a photon with $\lambda = 350\ \mathrm{nm}$ calculates to:


$$\mathrm{E} = \frac{6.62606957 \cdot 10^{-34} \cdot 2.99792458 \cdot 10^8}{350 \cdot 10^{-9}} \cdot \frac{\mathrm{J \cdot s \cdot m}}{\mathrm{s \cdot m}} = 0.05676 \cdot 10^{-17} \mathrm{J} = 5.676 \cdot 10^{-19} \mathrm{J}$$


This is the energy difference to the higher level.


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