00:02
Hi there.
00:03
In this question, we actually have two questions.
00:06
One about the shape, the molecular shape of h3o plus the molecular geometry, and the other question about the bond angle, an h -to -o -h bond angle in this.
00:19
To answer each of these questions, we need a lewis structure.
00:22
So let's start out by determining the number of valence electrons we have to work with.
00:27
There are three hydrogens, and hydrogens in group 1a of the periodic table, so each hydrogen has one valence electron.
00:36
We also have an oxygen.
00:38
Oxygen is in group 6a of the periodic table, so it has six valence electrons.
00:43
And then finally we have one unit of positive charge.
00:46
That means we have lost one electron, so we need to subtract one.
00:50
This gives us a total of eight valence electrons.
00:57
And since lewis structures show balance electrons as dots, it means that our structure will end up needing exactly eight dots.
01:09
Okay, let's go ahead and put this together.
01:12
We have oxygen.
01:14
It's bonded to three hydrogens.
01:18
We know that we need a bond to hold each of these hydrogens to the oxygen, and a bond requires a pair of shared electrons.
01:27
That takes up six of our electrons.
01:30
Each of the hydrogens now has two electrons, which is all that hydrogen needs, because it only has that first energy level.
01:37
So our remaining two electrons will go on the oxygen to complete its octet.
01:43
This is our completed lewis structure.
01:47
And from this lewis structure, looking at the oxygen, we see that the oxygen has three atoms bonded to it.
01:53
So the oxygen is our central atom.
01:56
It has three atoms bonded to it...