Which of the following factors tends to increase the melting point of a solid?

The melting point of a solid is significantly influenced by the type of bonds present in the material.

Ionic bonding typically results in the formation of strong electrostatic attractions between cations and anions. This strong interaction requires substantial energy to overcome, thus leading to higher melting points in ionic compounds. For example, sodium chloride (table salt) has a high melting point due to the extensive lattice structure created by these ionic bonds.

Covalent bonding, particularly in network solids (like diamond or quartz), involves atoms sharing electrons in a way that creates a stable, rigid structure. The strong covalent bonds hold the atoms in place tightly, necessitating high levels of energy to break these bonds during the melting process, again leading to a higher melting point.

Hydrogen bonding is another inter-molecular force that can increase melting points, especially observed in water, where hydrogen bonds create a network that holds molecules together more tightly than in substances without such bonding. While hydrogen bonds are generally weaker than ionic or covalent bonds, in certain contexts (like the solid-state of water), they can significantly increase the melting point when compared to substances with weaker intermolecular forces.

Since each of these types of bonding—ionic, covalent, and hydrogen—contributes to increasing