Q: Graphite cannot be classified as ______.

Explanation:

Graphite’s Structure 

Graphite is a form of carbon where each carbon atom is bonded to three other carbon atoms in a flat, two-dimensional hexagonal lattice. These strong covalent bonds within each layer form a network solid, giving graphite its stability and structure. The layers are held together by weaker van der Waals forces, allowing them to slide over one another easily, which is why graphite feels slippery and is used as a lubricant.

Graphite can conduct electricity because the electrons in its structure are free to move within the layers. However, it does not consist of positive and negative ions; instead, it is composed entirely of carbon atoms bonded covalently. Ionic solids, on the other hand, are made up of positive and negative ions held together by strong electrostatic forces in a rigid lattice. Since graphite does not have this ionic bonding structure, it cannot be classified as an ionic solid.