Which of the following correctly describes the bonding in graphite?

In graphite, the structure comprises layers of carbon atoms arranged in a two-dimensional hexagonal lattice. Within each layer, the carbon atoms are bonded together by strong covalent bonds, which creates a robust framework. However, the layers themselves are not strongly bonded to each other. Instead, they are held together by relatively weak van der Waals forces, allowing the layers to slide past one another easily. This characteristic is what gives graphite its lubricating properties and makes it useful as a lubricant and as the "lead" in pencils.

The other options do not accurately reflect the bonding in graphite. For instance, claiming that there are strong covalent bonds throughout would ignore the distinct nature of the interlayer interactions, which are indeed much weaker. Suggesting metallic bonds is misleading as well, since graphite does not exhibit the properties typically associated with metals, such as electrical conductivity due to free-moving electrons between layers. While discussing simple molecular bonding does not fit either, as graphite's structure is more complex than that, involving a continuous network of carbons rather than discrete molecules. Thus, the option describing the weak interlayer forces is the most accurate representation of graphite's bonding characteristics.