Carbon, silicon, and germanium have four vale | vedclass

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(D) Carbon $(C)$, Silicon $(Si)$, and Germanium $(Ge)$ all belong to Group $14$ of the periodic table and have $4$ valence electrons.At room temperatu

Vedclass · Accepted Answer

The number of free electrons for conduction is significant only in $Si$ and $Ge$ but small in $C$.

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(D) Carbon $(C)$, Silicon $(Si)$, and Germanium $(Ge)$ all belong to Group $14$ of the periodic table and have $4$ valence electrons.At room temperature, the energy band gap $(E_g)$ for Carbon (diamond) is approximately $5.4 	ext{ eV}$, which is very large, making it an insulator.For Silicon, $E_g \approx 1.1 	ext{ eV}$, and for Germanium, $E_g \approx 0.7 	ext{ eV}$.Because these band gaps are relatively small, thermal energy at room temperature is sufficient to excite a significant number of electrons from the valence band to the conduction band in $Si$ and $Ge$, making them semiconductors.In contrast, the large band gap of Carbon prevents significant electron excitation at room temperature, resulting in a negligible number of free conduction electrons.Therefore, the number of free conduction electrons is significant in $Si$ and $Ge$ but small in $C$.

Carbon, silicon, and germanium have four valence electrons each. At room temperature, which one of the following statements is most appropriate?

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