Describe the hybridization of the carbon atom in the poisonous gas phosgene, Cl2CO, and make a rough sketch of the molecule showing its hybrid orbitals and p bonds.

Video transcript

Hello everyone in this video, we want to identify the hybridization of the carbon item in formaldehyde, which has a formula of siege too. So we want to go ahead and also draw the orbital overlap for each of these bonds. So first things first, let's go ahead and figure out what the Lewis structure is and we'll base the orbital overlap diagram from the Lewis structure. So first thing to do when drawing out a Lewis structure is to count the total number of valence electrons present in this molecule. So for carbon we have one carbon atom. Each contributes for valence electrons because it is a group for a. Now hydrogen contributes One electron and there's two atoms, so two times one is equal to two. And then for oxygen it's in group six a so it contributes six fans electrons. So you take the sum of these three. So four plus two and six we get a total of 12 vans electrons present in this Lewis structure. So carbon is the least electro negative out of all the other atoms, which is hydrogen oxygen. So it's gonna go ahead and be the central item in our lowest structure. So we have our carbon and it's connected to to hire agents and one auction. So I put a double bond on the auction because first of all, carbon likes to have four bonds and auction likes to have two bonds and then we'll go ahead and add the low comparison for our auction. So you can see here first for our hydrogen atoms it only contains us orbital. As for our central carbon atom here, it's It has three bonding groups Since we have three bonding groups, it's S. P two hybridized. And for auction item on top here we have one bonding group and two lone pairs and this is S. P two hybridized. So for overlap, then carbon and hygiene have an overlap for carbons sp two with hydrogen S orbital. And then for our carbon auction sigma bond. So sigma here, we have the overlap of the carbons sp two orbital and auctions sp two orbital. And let's see our carbon auction pi bond because we have a double bond here, it's the overlap of the carbons pi bond or p orbital as well as auctions p orbital. So now drawing our structure using this. Then again, we have our auction atom, we have our carbon and then we have our two high regions. Maybe we need a little bit more space in between. All right, so, we said earlier for our first statement here for the carbon hydrogen overlap, we have the carbon sp two and the hydrogen s orbital overlapping. So, we know that s orbital is circular and then we have the carbons sp two to look something like this. So, this bottom little circle here is the s orbital. And now, for the interaction between carbon and auction, we said for the sigma von we have the overlap of the sp two and sp two be something like this. And we have the pie overlap or the pi bond between the carbon auction, and we have overlap of the carbons p orbital and auctions p orbital. So go ahead and draw this in red. We have the anti bonding and bonding. Alright. And lastly, of course, from the auction, we have these two lone pairs, so it is drawn in like so. All right, so the final answer then, is the structure right here. This is going to be my final structure for the over the orbital overlap of formaldehyde.