00:02
We're going to start with a, which is n2 with a plus charge.
00:08
First thing we need to do is add up how many valence electrons are going to be able to go into our image.
00:13
Now, valence electrons for our main group elements can just be found by labeling 1 through 8 on the periodic table for each column.
00:23
So a nitrogen has five valence electrons, and there's two of those.
00:31
And then a plus one charge means an electron has been removed.
00:37
This ends up being 10 minus 1, which is nine electrons to work with.
00:43
All right.
00:43
Next, we can go ahead and start our image.
00:45
We've got two nitrogen bound together.
00:48
Now, each bond counts as two electrons.
00:52
So that drops us down to seven left.
00:55
Each nitrogen wants to have eight electrons total.
00:58
Each one currently thinks that owns two, right? each nitrogen thinks that owns both those electrons.
01:03
So each one needs six more.
01:06
So one, two, three, four, five, six, seven.
01:14
Now, we're not going to be able to get to a full octet for both nitrogens.
01:20
Just because we have got a free radical here.
01:23
A free radical is when you have an odd number of electrons.
01:27
But we can try to help as much as we can by making double bonds.
01:31
So we can take our first loan pair and move it to being big.
01:36
Between the two nitrogen's.
01:39
And then we can do it again with this guy.
01:43
And that gives us something that looks like this.
01:52
Still got two over there, got one over there.
01:56
And when you finish a lewis structure, you wanna show the charge.
01:59
So it'd be in square brackets with a plus sign.
02:03
So there's our first one.
02:06
Next, we have got xe, xenon, seven.
02:14
So this would be xenon heptophoride with a minus one charge.
02:20
So we need to add up our valance electrons.
02:24
Xenon is a noble gas, so it has eight valence.
02:30
Fluorine has seven, and there's seven of those.
02:36
And then the minus one charge means an electron has been added to the system.
02:42
So this is going to give us a very large total of 58 electrons going into our image.
02:52
Now normally, these complexes really don't go above a single atom having six bonds, but technically as you get really low on the periodic table, you can have more than six.
03:05
This isn't common, but i believe this is what this one is looking for.
03:10
We're going to put a xenon in the middle and then surround it by seven florines.
03:24
Oh, come on, little pen.
03:27
Florine, flooring, flooring.
03:34
Drawing those bonds, that's seven bonds.
03:36
Seven times two is 14.
03:39
Which means we are down to 44 electrons.
03:45
Next, we need to fill the octets of the outer atoms, these fluorines.
03:48
They all currently think they own two electrons, so they need six more.
03:52
So for each one of these, we're going to add six more electrons.
04:06
Okay.
04:08
Six electrons times seven atoms is 42.
04:13
We've got two electrons left.
04:16
Those are going to go on the xenon.
04:18
Anywhere you like as long as they're on that xenon.
04:20
Okay, we'll put it in square brackets with the charge outside.
04:28
There you have it.
04:29
It's a big molecule...