Explain the large difference in the melting point of the compound of formula MgO and P4O104

Answer 1

The large difference in the melting points of MgO and P4O10 can be attributed to their differing chemical compositions and structures.

MgO, magnesium oxide, is a simple ionic compound composed of magnesium cations (Mg2+) and oxide anions (O2-). Due to the strong ionic bonds between the cations and anions, MgO has a high melting point of around 2,852 degrees Celsius. This high melting point is characteristic of many ionic compounds that have strong electrostatic interactions between their constituent ions.

On the other hand, P4O10, tetraphosphorus decaoxide, is a covalent compound composed of phosphorus atoms covalently bonded to oxygen atoms in a large polyatomic structure. Covalent compounds typically have lower melting points compared to ionic compounds because the intermolecular forces holding the molecules together are weaker than the ionic bonds present in ionic compounds. P4O10 has a lower melting point of around 340 degrees Celsius due to the weaker forces holding its molecules together.

In summary, the large difference in the melting points of MgO and P4O10 can be attributed to the difference in their chemical compositions, structures, and the type of bonding present in each compound. MgO has a high melting point due to its strong ionic bonds, while P4O10 has a lower melting point due to its covalent bonding and weaker intermolecular forces.