Valence electrons of carbon, silicon, and germanium — check the count used in semiconductor bonding Carbon (C), silicon (Si), and germanium (Ge) each have the same number of valence electrons that participate in covalent bonding in crystals. The statement “they have 5 valence electrons” is being evaluated. Decide whether this claim is accurate.

Introduction / Context:
Semiconductor materials rely on valence electrons to form covalent bonds in a crystal lattice. Knowing how many valence electrons elements like carbon, silicon, and germanium possess is essential for understanding intrinsic semiconductors and how doping creates n-type and p-type materials.

Given Data / Assumptions:

• Carbon (group 14), silicon (group 14), and germanium (group 14) are tetravalent in the periodic table.
• Valence electrons determine bonding and the ease of creating charge carriers via doping.
• Room-temperature solid-state behavior is considered.

Concept / Approach:
Group 14 elements have 4 valence electrons. In the diamond or zinc-blende lattice, each atom forms four covalent bonds with neighbors, using those 4 valence electrons. This is true for C, Si, and Ge. Therefore, saying they have 5 valence electrons is incorrect; elements with 5 valence electrons belong to group 15 (e.g., phosphorus, arsenic, antimony), which serve as donor dopants in silicon.

Step-by-Step Solution:

Verification / Alternative check:
Introductory semiconductor texts list silicon’s electron configuration as [Ne]3s^2 3p^2 → 4 valence electrons; germanium [Ar]3d^10 4s^2 4p^2; carbon 2s^2 2p^2.

Why Other Options Are Wrong:

Common Pitfalls:
Confusing valence count (4) with donor dopants (5) used to create n-type material. The base element’s valence does not become 5 due to temperature.

Final Answer:
Incorrect