Provide the complex ion structure and geometry when a Co 3+ ion combines with 3 ethylenediamines.

Alright. So from the little bit of hints that I gave to you, let's approach this question. So we know that we have cobalt 3 ion and it's connecting to 3 ethylenediamines. Remember, in terms of abbreviation that's just e n. Alright. Now, we're going to say, that the structure would be what? It would be cobalt connected to 3 ethylenediamines. The overall charge would be plus 3 coming from the cobalt 3 and no charge contribution from the ethylenediamines because they are l ligands. They have no charge. So overall, the complex ion should have a plus 3 charge overall. So brackets and then 3 plus on the outside. Alright. Now, we have to draw this. Remember, ethylenediamine is a bidentate ligand and they form rings when they combine with the transition metal to make the complex ion structure. So we have our cobalt in the center. Now, I told you that these 3 ethylenediamines is equivalent to 6 ligands, 6 monodentate ligands. So that if we have 6 ligands that gives us an octahedral shape. So remember, octahedral, we'd have these 2 bonds on the plane of the paper. We'd have these 2 bonds that go into the plane of the paper. Then we'd have these 2 bonds that point up out of the plane of the paper. And all we gotta do now is just draw these 3 Ethylenediamines. So, remember Ethylenediamine we have NH2 connected to a CH2, So that's one part of it done. Same thing here. So that's one part of it done. Same thing here, n h 2 connected to a c h 2, c h 2 connected to an NH 2. And then n h 2 Connected to a CH2. Connected to another CH2. Connected to an NH2. Okay. I'm drawing it as best as I can. So we'd get something like this. So as we can see that each, bidentate ligand helps to make a cyclic structure for a complex ion. And then brackets and then the charge on the outside. So you get something like this as the geometry for a complex ion. So, just keep in mind when it comes to complex ion structures, the charge of your ligands are important and the charge of your transition metal is important. Them all contributing together gives us the overall charge of our complex ion. Also, remember the rules that we established when it comes to the geometry of these complex ion structures. If you have a coordination number of 2, which equals 2 2 ligands, then you're linear. If you have 6 ligands, then you're octahedral. When you have a coordination number of 4, then you can be either tetrahedral or square planar. It's all based on the electron configuration of your transition metal. Keep these in mind when you're writing either the complex ion structure or its geometry.