Identify any formal charges in the following structures:
Hey everyone, let's take a look at our problem, let's draw it out first, this is going to be our structure, we have two sets of lone pairs on it, and it wants us to identify the formal charge, okay? So let's look at that nitrogen. Now, notice that a nitrogen has one would you say? two bonds to it, right? And then two lone pairs, so we're going to say our nitrogen has two bonds and two lone pairs, so remember what's the ideal situation for nitrogen to be in when dealing with valence electrons? nitrogen likes five valence electrons, right? to be neutral, so if it has anything less than that or anything more it's going to have a formal charge, so let's count the bonds electrons, here we have one N one, right? That's two valence electrons from those Sigma bonds and then what about our lone pairs, right? Well, we're going to say this is two and two, so what we can do just add all those up, 2 plus 2 plus 1 plus one, what does that give us? take a look, it gives us six valence electrons, six valence electrons, so we know that this nitrogen is going to have a formal charge but is it going to be positive or negative? Well, remember if we had less valence electrons than one, if let's say we had four the nitrogen will be positive but since we have more electrons than we want we're gonna say this nitrogen actually has a negative charge on it guys, okay? So hopefully that makes sense and let me know if you have any questions.