Provide an example of the lattice energy and enthalpy of formation in the Born-Haber cycle.

An example of the lattice energy and enthalpy of formation in the Born-Haber cycle is the formation of sodium chloride.

In the Born-Haber cycle, the enthalpy of formation of sodium chloride is calculated by adding the enthalpies of several steps. First, the enthalpy of sublimation of sodium is added, which is the energy required to convert solid sodium into gaseous sodium atoms. Then, the enthalpy of ionization of sodium is added, which is the energy required to remove an electron from a sodium atom to form a sodium ion. Next, the enthalpy of electron affinity of chlorine is added, which is the energy released when a chlorine atom gains an electron to form a chloride ion. Finally, the lattice energy of sodium chloride is subtracted, which is the energy released when sodium and chloride ions come together to form a solid crystal lattice.

The lattice energy of sodium chloride is a measure of the strength of the ionic bonds between the sodium and chloride ions in the crystal lattice. It is a large negative value, indicating that a large amount of energy is released when the ions come together to form the lattice. The lattice energy is influenced by factors such as the size of the ions, the charge on the ions, and the distance between the ions.

Overall, the Born-Haber cycle provides a way to calculate the enthalpy of formation of an ionic compound and understand the various factors that contribute to it.