Borek said:In what context is it said? In the ground state I would expect s2p2, but perhaps they aim at the hybridized sp3 (not that it physically exists).
256bits said:silicon - 4 valence electrons
Shells would have 1 electron in each before pairing
I would think your testbook is of the opinion silicon has arrangement
[Ne] s1 p1 p1 p1
The electron configuration of silicon is 1s2 2s2 2p6 3s2 3p2. This means that silicon has 14 electrons total, with two in the first energy level, eight in the second energy level, and four in the third energy level.
Silicon has two unpaired electrons. This is because in its electron configuration, the last two electrons are in the 3p sublevel, and there are only two available spaces in this sublevel for electrons to occupy.
Silicon's unpaired electrons make it a semiconductor, meaning it can conduct electricity under certain conditions. This is because the unpaired electrons can move between atoms, allowing for the flow of electric current.
The number of unpaired electrons in silicon affects its ability to bond with other elements and form compounds. Silicon can bond with up to four other atoms, making it a versatile element in creating various materials, such as computer chips and solar panels.
No, silicon cannot have more than two unpaired electrons. This is due to its electron configuration, which only allows for two electrons in the 3p sublevel. Any additional electrons would have to occupy a higher energy level, making it less stable and less likely to occur in nature.