Question

Consider the following compounds: cao, cas, and mgo. answer the following questions based on expected periodic trends:

(a) which is expected to have the shortest ionic bonds?
(b) which is expected to have the highest lattice energy?
(c) which is expected to have the lowest melting point?

Answer 1

MgO is expected to have the shortest ionic bond, LiF is expected to have the highest lattice energy, and CaO is expected to have the lowest melting point.

Step-by-step explanation:

a) The compound expected to have the shortest ionic bond is MgO. This is because both Mg²+ and O²- have high charges and small radii, resulting in a stronger ionic bond.

b) The compound expected to have the highest lattice energy is LiF. This is because Li⁺ and F⁻ have high charges, resulting in a stronger electrostatic attraction in the lattice.

c) The compound expected to have the lowest melting point is CaO. This is because CaO has a higher lattice energy than the other compounds mentioned, making it more difficult for the ions to move freely and therefore increasing the melting point.