00:02
Hi, we are given the two ions peroxidiculfate ion and the sulfate ion and we are asked to draw their low structure.
00:11
So the low structures are the diagrams drawn to show the bonding between the atoms of the molecules as well as the lone pair of electrons present on them.
00:22
So first of all, the low structure of peroxide sulfate ion is both the sulfur atoms are bonded by a double bond.
00:31
Then there are three oxygen atoms out of which one is bonded by us double bond and two others are bonded by a single bond.
00:41
After that we will complete their octet.
00:44
So there are already four electrons around this sulfur atom.
00:48
So we will add four other electrons as lone pair of electrons.
00:53
Here we need to add six more electrons.
00:57
Here four.
00:57
The single bonded electron carry the negative charge.
01:01
Now coming to the sulfate ion, there is only one sulfur atom with four oxygen atoms around it.
01:10
Out of these, two are double -bounded and two are single -bounded.
01:14
Similarly here, we will complete its octet by adding lone pairs.
01:19
The single -bonded oxygen atom carry the negative charge.
01:23
Now, next we are asked to calculate the formal charge.
01:27
The formula to calculate the formal charge is number of valence, total, number of valence electrons minus number of non -bonding electrons.
01:40
Non -bonding electrons are the electrons present as loan pair minus half of bonding electrons.
01:46
Bonding electrons are those that are present in bonds.
01:50
So for a single bond, there are two bonding electrons.
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For a double bond, there are four bonding electrons.
01:57
Now let's start by calculating the formal charge of this sulfur atom.
02:01
This is referred as s1 and this is referred as s2 to avoid confusion...