Which compound has the highest lattice energy?
a) CaO
b) LiF
c) MgO
d) NaF
I am guessing B because Lithium has the lowest energy level?
OK but because Li is smaller size.
To determine which compound has the highest lattice energy, we need to understand what influences lattice energy. Lattice energy is the energy released when gaseous ions come together to form a solid ionic compound. It depends on two factors: the charge of the ions and the distance between them.
The general trend is that lattice energy increases with increasing ion charge and decreasing ion size. Higher charges result in stronger attractions between ions, while smaller ions allow for closer proximity and stronger interactions.
Now, let's analyze the given compounds (CaO, LiF, MgO, NaF) to find the one with the highest lattice energy:
a) CaO: Calcium (Ca) has a 2+ charge, and oxygen (O) has a 2- charge. The charges are balanced, but both ions are relatively larger in size compared to other options.
b) LiF: Lithium (Li) has a 1+ charge, and fluorine (F) has a 1- charge. This combination involves smaller ions than in option "a," which generally leads to stronger attractions.
c) MgO: Magnesium (Mg) has a 2+ charge, and oxygen (O) has a 2- charge. Similar to option "a," this combination involves larger ions.
d) NaF: Sodium (Na) has a 1+ charge, and fluorine (F) has a 1- charge. Once again, smaller ions are involved, which promotes stronger interactions.
Based on the analysis, the compound with the highest lattice energy is LiF (option b). Therefore, your guess is correct. Lithium fluoride (LiF) has the highest lattice energy due to its combination of smaller ion size and appropriate charges.