Final answer:
The lattice energy of NaF is 910 kJ/mol, which is indicative of strong ionic bonds between the sodium and fluoride ions. This value should be considered in the context of the direction of energy flow—whether the lattice is being formed or broken apart—and it reflects the stability of the ionic compound.
Step-by-step explanation:
The lattice energy of an ionic compound is a measure of the strength of the bonds holding the ions together in the crystal lattice structure.
To determine the lattice energy of sodium fluoride (NaF), we can refer to empirical data and trends observed from similar ionic compounds.
According to Coulomb's Law, the force and thus the energy is related to the charge on the ions and inversely related to the distance between them.
Therefore, compounds with larger charges will have stronger attractions and higher lattice energies.
In comparing NaF with other ionic compounds, it is important to consider both ion charges and the interionic distances.
NaF has a calculated lattice energy of 910 kJ/mol, which is a high value indicating a strong ionic bond between sodium (Na+) and fluoride (F-) ions.
This is significantly less than the value for magnesium oxide (MgO), which has a lattice energy of 3795 kJ/mol due to magnesium's +2 charge.
It is also important to note the definitions of lattice energy, which can be considered as either endothermic (positive) when separating the ionic compound into gaseous ions or exothermic (negative) when forming the lattice from gaseous ions.
However, in any case, a larger magnitude of lattice energy indicates a more stable ionic compound.