Network Covalent Atomic Solids Explain why graphite can conduct electricity, but diamond does no

step 1 We need to determine why graphite is capable of conducting electricity and why diamond cannot. B

Network Covalent Atomic Solids Explain why graphite can...

Key Concepts

Covalent Network Solids

Covalent network solids are materials characterized by a continuous network of covalent bonds extending throughout the structure. This type of bonding yields materials that are typically hard and have high melting points, and the arrangement of bonds influences properties such as electrical conductivity.

Delocalized Electrons

Delocalized electrons are electrons that are not confined to a single bond or atom but can move freely over a large part of the structure. Their mobility is essential for electrical conductivity, as seen in materials where these electrons can carry charge across the structure.

Atomic Hybridization

Atomic hybridization involves the mixing of atomic orbitals to form new hybrid orbitals, which determine the geometry and bonding characteristics of a material. For example, sp² hybridization in some forms of carbon leads to a planar structure with free electrons, while sp³ hybridization results in a three-dimensional structure where electrons are more localized.

Crystal Lattice Structure

The crystal lattice structure describes the geometric arrangement of atoms in a solid. In some materials, such as layered solids, this structure allows for pathways that enable electron mobility and electrical conduction, whereas in other tightly bonded three-dimensional networks, electrons remain fixed in their bonds.

Electrical Conductivity

Electrical conductivity in solids is largely determined by the presence and mobility of electrons. Materials with delocalized electrons can conduct electricity well because these electrons can move easily under an applied electric field. In contrast, materials with electrons tightly bound in a three-dimensional network structure tend to be insulators.

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