Question

Question: Compare the hybridization of Si atoms in Si(s) with that of C atoms in graphite (see Fig. 21.26). If silicon were to adopt the graphite structure, would its electrical conductivity be high or low?

Short answer

The electrical conductivity of Si atom will be high.

Step-by-step solution

Step 1:

In outer most Shell both the atoms Si and C have 4 valence electrons. Silicon form 4 single bond which are $\mathrm{\sigma }-\mathrm{bonds}$ so the hybridization of Si is ${\mathrm{sp}}^3$ and C form 3 $\mathrm{\sigma }-\mathrm{bonds}$ and the electron is free so the hybridization of C is ${\mathrm{sp}}^2$, due to its hybridization it is a Hexagonal Planer Structure.

Step 2:

From the 4 $\mathrm{\sigma }-\mathrm{bonds}$of Si, 1 bond will break when the Si atom were to adopt the graphite structure. Due to the presence of 1 free electrons with each of the Si atom, it’s conductivity increases so the electrical conductivity of Si atom will be high.