00:01
Okay, so let's begin by drawing the lewis dot structures for each of these molecules.
00:05
So that way we can get a better idea of the central molecule, how many alone pairs it has, and how many other molecules it has on it.
00:14
So first off, we have tri -iodide.
00:21
So we have three iodine molecules plus one extra electron.
00:32
So one of those iodine molecules is going to bond to our central one.
00:35
The other one's going to bond to our central one.
00:37
And we'll put that extra electron on our central atom.
00:45
So that's going to give us, it's going to give us two bonds and three lone pairs.
01:04
So those three lone pairs will form a triangle around the middle of our iodine, while the other two iodine atoms will be on opposite sides.
01:25
So this molecule will be linear.
01:29
Next let's look at silicon tetrachloride.
01:34
We've got our central silicon atom, which has four molecules, there are four electrons, just like that, and it's going to be surrounded by chlorines, each of which has seven electrons.
01:56
So they connect the dots, and it's just like, and silicon is just like carbon...