Chemical energetics: describe question

When $\ce{NaCl}$ dissolves in water, the enthalpy change of solution, $\Delta H_ ext{sol}$, is +3.9 kJ mol$^{-1}$. The enthalpy change of hydration of $\ce{Na+}$ is $-406$ kJ mol$^{-1}$ and that of $\ce{Cl-}$ is $-364$ kJ mol$^{-1}$. The lattice energy of $\ce{NaCl}$ is $-776$ kJ mol$^{-1}$.

Describe, in words, an energy cycle that links $\Delta H_ ext{sol}$ to the lattice energy and the enthalpy changes of hydration of the two ions. In your description, define enthalpy change of solution and explain how the numerical values given are related in the cycle.