Draw a Lewis dot structure for each of the following compounds:
Alright guys. So, in this problem we need to go ahead and draw the Lewis dot structure for our CH3, right? Our CH3CN, okay? So let's just go ahead and draw out our central atom, so we know we have a carbon, we've got another carbon and then we've got our nitrogen on one of our carbons, right? What do we also know, we also we have three hydrogens directly attached to our first carbon, so it should look like this and now let's go ahead and add our electrons, so we can at least get our bonds going, right? We know that we need two bonds here, two electrons to form a bond, right? Okay, so now guys if you actually look our first carbon has its octet filled, right? And our hydrogens are satisfied, right? they've got their two electrons in their shell, that's how they like it, and then over here this carbon is missing how many electrons? Well, it's a 1, 2, 3, 4, it's missing electrons and our nitrogen guys it's also missing two bonds. Alright. So, four electrons because it we know that it also has its own lone care but the question is now does this lone pair go here to form another bond with carbon? Well, guys, nitrogen likes to have three bonds, this carbon right now only has two bonds, this nitrogen only has one, so what can we do? we can form a triple bond between these and are now our nitrogen, if you look our carbon has its octet filled, right? It's got 1, 2, 3, 4, 5, 6, 7, 8 electrons around it and our nitrogen has 1, 2, 3, 4, 5, 6, 7, 8 because it's got that lone pair, okay? Alright guys, let's move on to the next question.