00:01
That involves the sharing of electron pairs between atoms, and these electron pairs are known as bonding pairs.
00:05
Here we're writing out some lower structures, so what we need to concern ourselves with is the valence electron count on each of the atom, and the valence electron count corresponds to the group number of that atom.
00:16
So for example, we've got oxygen, that's group six, so it will have six valence electrons.
00:21
So we can jump into these examples here.
00:23
So firstly, we have clf, so we have chlorine and fluorine, where we have a single bond, so we've used up one, each.
00:31
So we know that chlorine and fluorine, both halogens, so they have seven valence electrons.
00:36
So then each species needs three more lone pairs and that accounts for all of their electrons, where we have 14 available electrons, where we have a complete octet.
00:47
Next we have h2se.
00:51
So we have s -e, one into two hydrogens.
00:56
So we're using four electrons in bonding pairs, and then selenium has two lone pairs because it is group six.
01:03
And so then, then, therefore, we have eight electrons available where selenium has a full octet and hydrogen has a complete duet.
01:14
Next we have bf4 minus...