 So let's do this one First, the complex ion pictured has a square planar geometry name the complex ion pictured and then draw the structures of the two geometric isomers of this complex Okay, and in fact I have the models built already so we can look at that too Okay, so naming this thing Right first we put the ligands and we got to put them in alphabetical order and they're all negatively charged If you if you don't know bromines are negatively charged cyanogrups or negatively charged of cyanide So this is going and we've got to put them in alphabetical order. So this is going to be called die-bromo die-cyano Then we put the Metal atom, but it's a negatively charged ion So it's going to be the nickel-8, and we have to figure out its oxidation state Well, this is negative one times two so negative two negative one times two so negative two so negative two Negative two so that's overall negative four right negative four so to get a negative two This must be positive Right, so so the name of this compound is die-bromo die-cyano nickel-8 two Okay, and now it wants us to draw the geometric isomers Okay, so remember the geometric isomers are going to be at the same Atoms connected to the same other atoms, but they're going to be arranged differently Okay, and it already told us it's in a square planar arrangement But the nickel in the middle so We'll draw the cis Complex first remember cis same side So this is the cis With the two groups being on the same side. Okay, so we're doing so let's do the trans isomers now So what is it going to look like it's going to have the nickel in the middle still, but instead of having the Same group on the same side. We're going to have different groups on the same side the same groups opposite of each other so this geometric isomer is called the trans isomers So that's when the same groups are opposite of each other Okay, so let's just look at what these two look like and instead of their square planar Right, so there's the cis Hopefully you can see the square planar arrangement. Okay, we've seen a few of these now Hopefully you can see the cis right same side ligands same ligands on the same side Let's compare that to the trans right the same ligands are on opposite sides of each other same ligands are on opposite sides of each other and Want to ask are these the same compound? No, they're not why because to inter-convert from one to another What would I have to do? I'd actually have to break a covalent bond and Reattach it so break two of them in this case Then I would get the same Okay, so they're actually different compounds even though They have the same molecular formula and the same atoms are bonded to the same Okay, any questions on this one? Okay wonderful