00:01
Okay, so we're asked to illustrate the formation of a single, double, and triple -provalent bond using loose structures.
00:09
So let's start with a single bond.
00:12
So let's look at our atom fluorine.
00:17
And let's say that it wants to bond with another flooring.
00:21
So we have two fluorings with valence electrons 7, so that makes a total of 14 valence electrons.
00:32
Okay, let's see.
00:35
So let's draw out our valence electrons for each flooring.
00:39
So we have one, two, three, four, five, six, seven, and then one, two, three, four, five, six, seven.
00:46
So as you can see, based on the structure, like one of these, or this electron can be shared with this electron here to form a bond or specifically a single bond in order for both to have a noble gas configuration.
01:04
So it would look something like this.
01:07
If those two bonds form, we'd have a dash like that, and then our remaining lone pairs.
01:14
Now let's see how a double bond forms.
01:16
So let's take our element oxygen, which has six valence electrons, and let's say it wants to bond with another oxygen.
01:30
So that makes it to have like 12 valence electrons since it's six times two.
01:35
Okay, let's draw them out separately...