Let's understand why Silicon (Si) from Group 14 is a semiconductor:---Step 1: Locate Silicon (Si) in the Periodic Table. You'll find it in Group 14, Period 3.---Step 2: Recall the electron configuration for elements in Group 14. They typically have 4 valence electrons (electrons in the outermost shell).---Step 3: In a pure Silicon crystal, each Silicon atom shares its 4 valence electrons with 4 neighbouring Silicon atoms, forming strong covalent bonds. This creates a stable structure where electrons are mostly 'locked in'.---Step 4: At very low temperatures, these electrons are not free to move, making pure Silicon behave like an insulator.---Step 5: When you add a little energy (like heat or light), some of these electrons gain enough energy to break free from their bonds and start moving.---Step 6: These free electrons can then carry electric current, making Silicon a semiconductor, meaning its conductivity is 'in-between' a conductor and an insulator.---Answer: Silicon from Group 14 is a semiconductor because its 4 valence electrons allow it to form bonds that can be broken with a small amount of energy, enabling controlled electrical conduction.