Pure elemental silicon and germanium serve as the foundation of modern solid-state electronics due to their intermediate electrical conductivity. What atomic characteristic distinguishes these Group IV elements as semiconductors?
- AThey contain only one weakly held outer electron that drifts freely between atomic nuclei.
- They have exactly four valence electrons in their outermost shell, creating a stable covalent lattice under normal conditions.Answer
- CThey feature a full valence shell of eight electrons that completely blocks electrical charge movement.
- DThey maintain a permanent net positive charge that actively opposes the flow of conventional current.
Answer
Pure silicon and germanium are classified as semiconductors because their atoms possess four valence electrons in their outermost shell, forming covalent bonds that yield intermediate electrical conductivity.
Semiconductors such as silicon () and germanium () belong to Group IV of the periodic table and have four valence electrons in their outer shell. In crystalline form, each atom shares these four electrons with adjacent atoms via covalent bonds, resulting in electrical conductivity that lies midway between conductors (which typically have to loosely held valence electrons) and insulators (which typically have to tightly held valence electrons).
Step-by-Step Solution
Key Concept
Semiconductor atomic structure and valence electrons
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