Final answer:
Without hybridization, a silicon atom with a 3s²3p² valence electron configuration can form two covalent bonds using the two unpaired electrons in the 3p orbitals. However, silicon typically undergoes sp³ hybridization to form a tetrahedral structure with four bonds, as seen in various silicon compounds like SiH4 and SiO4²-.
Step-by-step explanation:
Bonding Capacity Without Hybridization
The valence electron configuration of an atom determines its bonding capacity, that is, how many covalent bonds it can form without hybridization. Silicon (Si) with a valence electron configuration of 3s²3p² has four valence electrons. Two electrons occupy the 3s orbital and two electrons are in the 3p orbitals. Without hybridization, the two unpaired electrons in the 3p orbitals can form two bonds. However, to form four bonds and complete the octet, silicon typically undergoes sp³ hybridization, allowing four equal sp³ hybrid orbitals to form.
Exploring this further with examples, (CH3)3SiH, SiO4²-, Si₂H₆, Si(OH)4, and SiF6²- all feature silicon with sp³ or sp³d² hybridization, supporting structures such as tetrahedral and octahedral arrangements. However, without invoking hybridization, we would expect silicon to make fewer bonds, as it would be limited to the unpaired electrons in its p orbitals.