00:01
To determine the molecular shape, hybridization, and the axe formula for this molecule, we need to focus on the central carbon here, and first we need to draw the lewis structure.
00:20
To draw the lewis structure, we need to count the number of valence electrons.
00:23
There are three carbons at four valence electrons each, and six hydrogens at one valence electron each, given us 18 valence electrons.
00:31
So if we bond the three carbons in a chain, each bond being two electrons, we would have used up four.
00:39
So we would be down to 14 valence electrons.
00:43
We'll then bond three hydrogens to this carbon, this three right here, one to the central carbon, and two to the peripheral carbon.
00:54
So that's a total of one, two, three, four, five, six bonds.
01:00
At two bonds each, we've used, i'm sorry, two electrons.
01:03
Each we've used up 12 additional valence electrons and we've got two left and everything every carbon has an octet except for these two right here so i guess only that one has an octet.
01:16
The hydrogens don't need an octet, they just need one bond.
01:20
So with the two electrons we have left we're going to make a double bond right here...