Draw the Lewis structure(s) for each of the molecules and...

Draw the Lewis structure(s) for each of the molecules and molecular ions listed below. Follow the procedures given in the Summary at the end of the study assignment. Include the formal charges in the Lewis structures. Look for equivalent resonance structures and write the number of equivalent structures. Molecule | Number of valence electrons | Bond skeleton | Remaining electrons | Lewis structures with formal charges | Resonance structures? How many? CF4 | | | | | NH3 | | | | | OCl2 | | | | | PO4^3- | | | | | NH4^+ | | | | | C2H6 | | | | |

Transcript

00:01 For this problem we are drawing several different structures lewis structures.

00:06 So the first one we need to draw is c f4 each carbon brings in four valence electrons each fluorine brings in seven and there are four of them.

00:19 So that would be four plus twenty eight so we have 32 electrons valence electrons that we're working with here the next thing we need to do is draw the bond skeleton so that's going to be your central atom surrounded by the other things that are attached to it then we need to know how many remaining electrons there are so we have used two four six eight so that means we have 24 electrons that are left.

00:45 The next thing we need to do is draw the structure with all of its electrons so that's going to look like this and so each fluorine needs to have a total of eight electrons around it so we're going to go ahead and put all of those on there and then the last thing asks if there are any resonance structures in this case, there aren't any because there aren't any atoms that are different from each other next we have nh 3 so nh 3 each end brings in 5 each h brings in 1 that's 3 so that's a total of 8 electrons.

01:33 We will have our end surrounded by the three h's that leaves us we've used two four six so we have two electrons left to place and they are going to go on our central atom so that it also has eight electrons and ammonia does not have any resonance structures.

01:52 So we'll do that for that and this for this so there are none for those.

01:58 Okay next we have ocl 2 so ocl 2 each o brings in 6 each cl brings in 7 there are two of them so that's 14.

02:11 So we have 20 total electrons.

02:13 Oh is in the center with the cl's around it...

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