00:01
So here we're asked to essentially determine whether there is not, whether there is not, whether there is or not a net dipole moment.
00:10
So we have a list of different compounds.
00:13
So our first compound is h3cbr.
00:17
And basically we can use intuitiveness to determine whether or not there would be a net dipole moment.
00:23
So first of all, carbon and hydrogen bonds are relatively non -polar.
00:27
So we can assume there's no net dipole there.
00:29
However, bromine typically is more electronegative than carbon, so we can draw our net dipole vector in this direction, since more electrons would be attracted to bromine.
00:43
So here, in part b, we have basically a similar compound, but in this case, we have a lithium atom.
00:51
And occasionally we can approximate basically the carbon lithium bond as an ionic bond, but in this case, we'll just assume it's a covalent bond.
00:59
So lithium is very un -electron -negative, so it's more technically electropositive.
01:05
So it disfavors the addition of more electrons.
01:10
So in this case, carbon would actually be more electronegative than lithium.
01:14
So the net dipole moment arrow would be in this direction...