Nature of covalent bonding in semiconductors Electron-pair bonding in a crystal lattice occurs when atoms do which of the following?

Introduction / Context:
Covalent bonding underpins the structure of semiconductor crystals. Understanding how atoms bond helps explain band formation, carrier generation, and the operation of diodes and transistors.

Given Data / Assumptions:

• Group IV semiconductor lattice (e.g., silicon).
• Stable, periodic crystal with sp³ hybridization.

Concept / Approach:
In covalent bonds, neighboring atoms share pairs of electrons to complete their outer shells. In silicon, each atom shares one electron with each of four neighbors, forming four electron-pair bonds. At finite temperature, breaking some bonds generates mobile carriers (electrons and holes).

Step-by-Step Solution:
Recognize covalent bond definition: shared electron pairs between atoms.Apply to semiconductors: four shared pairs per atom in the tetrahedral lattice.Infer: electron-pair bonding equals sharing electrons.Therefore, the correct description is “share electrons.”

Verification / Alternative check:
Band theory derivations begin with covalent bonding and result in valence and conduction bands separated by a bandgap appropriate to shared-electron systems.

Why Other Options Are Wrong:
Lack electrons/holes: describes defect states, not the bonding mechanism.Share holes: holes are the absence of electrons; the bond itself is electron sharing.

Common Pitfalls:
Thinking of holes as physical particles in bonds; bonds involve electrons, while holes are mobile vacancies influencing conduction.

Final Answer:
share electrons