 Okay so the first question we wanted to do or we were asked is let's figure out what the complete Lewis structure showing all atoms, valence, electrons, and all formal charges for the following species. So the first one sodium fluorohydride that we're looking at. So sodium, what is it? Always. It's just that positive and so it's going to be just the cationic portion. The structural portion of this molecule is the BH4 or the borohydride portion. So the sodium ion is just going to be a spectator ion. So it's going to be just the counter ion to the thing that we're looking at. So what do we know about boron? Right? Yeah so normally it will want to have three, right? But since we have a sodium plus on there, what must BH4 have on minus charge? Okay so it looks like this BH4 minus. Okay so if you're building things like how I taught you how to build things, putting all your valence electrons first, so Lewis structure wise we wanted to say well boron has three valence, right? How many does hydrogen have? One. Okay if I give hydrogen another electron, the way we've been doing it, can it make a bond? What do you need to make a bond? A half filled orbital. Remember guys we talked about half filled orbitals, okay? So here we can, so this, what is this negative charge cell? Gaining another electron, right? So boron here can gain another electron. So we've got that sort of situation and you don't have to do all this if you can do it on your own without drawing all those valence electrons, okay? So it says that we've got a negative charge. Where is that negative charge going to be located on the boron? Should we do the formal charge calculation? Are you guys pretty good with looking at them now? So that's what it's going to look like. So that's the Lewis structure showing all atoms. So if you wanted to, can I erase this portion of it? If you wanted to talk about Lewis structure, you can do something like that just to emphasize the close proximity between the two ions, okay? Showing all atoms, all valence electrons, there, we didn't have them all there. All formal charges for the bonds we see. So that's it? Yep. What's the molecular geometry around the boron? Tetrahedral. What's the ideal bonding? 1 and 9 and a half. Yeah. What would be the hybridization? Sv3. Sv3? Very good. Does that make sense? Is that what you, ladies, put? Yep. I'd say that's what I put. I actually want 3rc. Okay, well we'll do that one next. Any other questions on this one? Should we kill it? Yeah, you can't put brackets around it. You got to put the formal charge on the actual atom. You have to.