Explain the question and the answer

The question asks to identify the enthalpy change ($\Delta H$) values corresponding to three specific energy changes involved in the formation of sodium chloride ($\text{NaCl}$). These values are typically part of a Born-Haber cycle, which is used to calculate lattice energy.

• Heat of formation: This is the enthalpy change when one mole of a compound is formed from its constituent elements in their standard states. For $\text{NaCl}$, this is the formation from solid sodium ($\text{Na}_{(\text{s})}$) and chlorine gas ($\text{Cl}_{2(\text{g})}$). The value $\boxed{\text{-410}}$ represents the overall energy released when $\text{NaCl}$ is formed.

• Atomization energy: This is the enthalpy change required to produce one mole of gaseous atoms from an element in its standard state. For chlorine, it's the energy needed to break the $\text{Cl-Cl}$ bond in $\text{Cl}_{2(\text{g})}$ to form individual gaseous chlorine atoms ($\text{Cl}_{(\text{g})}$). The value $\boxed{\text{+121}}$ is positive because energy is absorbed to break bonds.

• Sublimation energy: This is the enthalpy change required to convert one mole of a solid directly into a gas. For sodium, it's the energy needed to change solid sodium ($\text{Na}_{(\text{s})}$) into gaseous sodium atoms ($\text{Na}_{(\text{g})}$). The value $\boxed{\text{+108}}$ is positive because energy is absorbed to overcome intermolecular forces and change state.