Which statement describes graphite's bonding arrangement?

Which statement describes graphite's bonding arrangement?

• A. Layers of carbon atoms with strong interlayer bonds
• B. Layers of carbon atoms in hexagonal rings held together by weaker forces with delocalized electrons
• C. Carbon atoms arranged in a simple lattice with localized electrons
• D. Each carbon atom forms ionic bonds

Answer: (B)

Graphite is made of layers of carbon atoms arranged in hexagonal rings. Within each layer, the carbon atoms are held together by strong covalent bonds, forming a two-dimensional network. Between these layers, the forces are weak van der Waals forces, so the layers can slide over one another. The electrons in each layer are delocalized, which allows electricity to flow along the plane. The statement that best describes this is the one that says layers of carbon atoms in hexagonal rings are held together by weaker forces with delocalized electrons. It captures the strong in-layer bonds, the weak interlayer attraction, and the presence of delocalized electrons that enable conductivity. The other ideas don’t fit graphite: having strong bonds between layers would prevent the layers from sliding; a simple lattice with localized electrons isn’t accurate for graphite’s delocalized electrons within the planes; and carbon–carbon bonding in graphite is covalent, not ionic.

Graphite is made of layers of carbon atoms arranged in hexagonal rings. Within each layer, the carbon atoms are held together by strong covalent bonds, forming a two-dimensional network. Between these layers, the forces are weak van der Waals forces, so the layers can slide over one another. The electrons in each layer are delocalized, which allows electricity to flow along the plane.

The statement that best describes this is the one that says layers of carbon atoms in hexagonal rings are held together by weaker forces with delocalized electrons. It captures the strong in-layer bonds, the weak interlayer attraction, and the presence of delocalized electrons that enable conductivity.

The other ideas don’t fit graphite: having strong bonds between layers would prevent the layers from sliding; a simple lattice with localized electrons isn’t accurate for graphite’s delocalized electrons within the planes; and carbon–carbon bonding in graphite is covalent, not ionic.