In the pobr3 molecule the p atom is the central atom draw a...

'In the POBr3 molecule; the P atom is the central atom Draw a Lewis diagram of POBr3 for which all formal charges are equal to zero. How many double bonds are there in the structure that you have drawn? number of double bonds Draw a Lewis diagram in which the octet rule is satisfied on all atoms What are the formal charges on the following atoms in the structure that you have drawn? Br Based on formal charge; which is the best Lewis structure for the molecule?'

Transcript

00:01 All right, so we're told that we have the molecule p -o -b -r -3.

00:05 Phosphorus is a central atom, and first we want to draw a lewis structure in which there's no non -zero formal charges.

00:12 So we have phosphorus in the center, and we know that we're going to have at least one bond to each of these species, br, br, and br, like that.

00:25 So bromine tends to typically form one bond.

00:28 So if we were to put the other three loan pairs on it to satisfy its octet rule, now it has seven electrons.

00:35 So each of these bromines has a formal charge of zero.

00:39 Now, phosphorus wants to have five electrons, and right here it has only four.

00:45 So this way it has a formal charge.

00:48 So that means if we were to draw another bond to the oxygen, because we don't want to mess with bromine.

00:52 Bromine tends to form one bond each.

00:55 Now phosphorus has a formal charge of zero.

00:57 And then this oxygen has two bonds, so it would need two loan pairs in order to satisfy the octet rule.

01:04 And that way it has two from the bond and four loan, a total of six electrons belonging to it.

01:09 So a zero formal charge.

01:11 This is an example of an expanded octet, which is possible for the central phosphorus because it's in the third or below period.

01:19 So it has deorbital's available for expanded octet bonding, meaning more than four bonds around it...

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