True/False (Bonding): In a purely covalent (valence) crystal, the bonding between atoms is accomplished by sharing valence electrons.

Introduction / Context:Crystalline solids are stabilized by different bonding mechanisms: ionic, covalent, metallic, Van der Waals, or mixed. A “valence crystal” typically refers to a covalent crystal where each atom shares electrons with neighbors to fill valence shells, leading to directional bonds and characteristic properties.

Given Data / Assumptions:

• Ideal covalent solids (e.g., diamond, silicon, germanium).
• Atoms form tetrahedral or other directional bonds by sharing electrons.
• No significant ionic character for the idealized statement.

Concept / Approach:Covalent bonding arises when atoms with comparable electronegativities share pairs of electrons to achieve closed-shell configurations. In diamond (sp^3 hybridization), each carbon atom shares four electrons with neighbors, yielding a strong, directional network. This contrasts with ionic crystals (electron transfer) and metals (delocalized electron sea).

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