00:01
Hi, in this question we are given with 5 molecules and we are asked to find out their electron geometry.
00:06
We can say that in case of electron geometry, number of total electron pairs are calculated.
00:24
The first molecule given to us is carbon dioxide, that is co2.
00:30
We have carbon atom as a central atom, rounded by 2 oxygen atom, which is, double bonded with carbon.
00:37
Oxygen are having two lone pairs.
00:41
To find the electron geometry, we need to find the total electron pair around the central atom.
00:47
We have carbon as central atom and we can see around it we have two sigma bonds or we can say that bond pairs.
01:04
There is no lone pair on the carbon.
01:06
For two bond pairs we can say the hybrid the hybridization will be sp and if we talk about the geometry then we can say that carbon dioxide is having a linear geometry.
01:24
Now the second compound given to us is ammonia that is nh3.
01:29
We have nitrogen atom surrounded by three hydrogen atoms and there is one lone pair.
01:37
Here we can see we have three bond pairs and one lone pair.
01:49
Together they form four number.
01:53
For four we can say the hybridization is sp3 and if we talk about the electron geometry it will be tetrahedral.
02:06
Now we are given with third molecule that is phosphory.
02:11
Trichloride we can draw the structure as we have phosphorus as central atom around which there are three chlorine atoms.
02:24
Phosphorus is having one lone pair of electron around chlorine we are having three lone pair of electrons we can represent in this manner.
02:34
We need to consider the electron pairs around the central atom...