00:01
Hello, so we're here to answer the question that asks to write the leo structure for six different resonance forms of the sulfate ion in so4 -2 negative.
00:20
So let's see how we will get the structure.
00:23
So first, let's do the level structure for the molecule and then we will get to the resonance structures.
00:32
So first we will basically we'll put the sulfate.
00:37
In the middle and then we'll add the oxygens around the sulfur atom and we'll have one bond, one sigma bond between all of this and to satisfy the rest of the electrons, the variance electrons so each oxygen will have three pairs of electrons and to calculate the formal charge each of these oxygens will have a one negative charge.
01:17
On them and the sulfur atom will have two positive charges which will give us two negative formal charges on the molecule but there's a better low structure for this if we it's the formal charge is the same but you will reduce the number of charges so basically takes take these electrons and put them and do another bond between this sulfur and this oxygen to look like this.
02:11
So here, now this oxygen has a zero formal charge, has no negative charges now.
02:24
These oxygians has, each one has a negative one charge, and the sulfur now has only one positive charge which will still give us a form of charge of two negative.
02:37
This structure is electronically better than this one, but we still can make it better...