 All right, let me do a little video on the psionic bonding stuff because as I said we're going through the notes really quick because most of this is review and There are a lot of you that have the flu so you need to know what you're doing First things first Ionic bonding Occurs when you have an atom of a metal and a non-metal You need this combination because you need something with a low ionization energy something that it's easy to remove electrons from and Something with a high electron affinity something that stands to Gain a lot when it gains electrons But I mean by that is it becomes more stable when it gains electrons and that's what non-metals do In this ionic bonding process your metal will Lose all It's valence electrons It has to lose the entire set it can't lose a partial number because that would actually make it less stable than What it would have been to begin with? It'll form a positive. I am Losing electrons means you're losing negative charges. You'll end up with more protons than electrons Giving it the overall positive charge Or resemble the noble gas They came before it That is to say it will lose electrons and it's a number of electrons will decrease Until it matches that of a noble gas And it will lose an energy level in the process as It loses those valence electrons. It loses its entire outermost energy level Now metals are the opposite side of the story. They're going to gain They're going to gain enough electrons To have eight in their outermost level and valence electrons For my negative. I am When they do so the world symbol the noble gas that comes after it That is to say the number of electrons will increase to the point where it matches a noble gas And as such they don't lose energy levels. So enough of that boring stuff. Let's get right down to it Let's get down to the stuff that matters What is going to be able to do with this? So let's take a look at this little thing. This is a knot an assignment that I passed out in class This is an old one. I have I might give it out to you as a study guide and we'll get closer to the test Let's work through some things We're going to take an element and we're going to find out if it's a metal or not metal by looking at Where it's that on the periodic table How many valence electrons it has by looking at its group number? Based on these two things we'll figure out what it needs to do to become stable in the ionic bonding process We'll work out the number of protons and the number of electrons and Then we'll work the charge out mathematically So let's start with sodium First thing you need to do is figure out if it is a metal or not metal. Well, there it is The metalloids are over here It's definitely to the left of the metalloids That makes it a metal. Next thing up is valence electrons there is sodium in group one And as we know the members of group one have one valence electron Now because it's a metal as I said before it has to lose all of its valence electrons in order to become stable and that's what it's going to do in Ionic bonding it's going to lose one electron What it does this the number of protons does not change the number of protons is still equal to the atomic number What should be 11 the old neutral atom? The protons and electrons are the same had 11 of them But now that we're going to lose one The ion will have only 10 So we look to see what we did here to figure out what we're going to do there for the equation The positive charge is the number of protons There are 11 of them and each proton has a plus one charge So the total positive charge in a sodium atom or ion is positive 11 And we're going to work out for the ion here not the neutral atom with the number of electrons in the charges so we can figure out The overall charge so to that we're going to add negative 10. It is positive 11 plus negative 10 Positive coming from the protons negative coming from the electrons and we add those two things together We end up with positive one Which is the oxidation number and charge for sodium? Let's try chlorine There it is Chlorine there's our metalloids is on the right-hand side That makes chlorine a Nonmetal now we need to figure out the number of valence electrons. There's chlorine group 17 Means it has seven of them now these things together determine what we're going to answer here It is a nonmetal and as I said before and I'll probably say again Nonmetals gain enough electrons to have eight If we got seven we need one more Again, we got to work out some atomic structure stuff First the number of protons That's the atomic number 17 in the neutral atom. We will also have 17 electrons, but that's about the change because we're going to gain one Giving us 18 in the ion now for the charge math number of protons is the positive part positive 17 For the negative part we're adding to it. It's right there under the ion negative 18 positive 17 plus negative 18 is negative 1 the charge or oxidation number For chlorine in addition to all that fine excitement. You have to work with the electron configurations Remember when you're doing electron configurations. You have to know the order of orbitals 1s 2s 2p 3s 3p Now before we can go to 3d. We have to fill up 4s Then we can go back to 3d and 4p and Then 5s and that will cover everything that you need to be able to write electron configurations for in CP chemistry So let's write some electron configurations. We're going to start with NA and then we're going to do the CO First is the neutral configuration For the neutral configuration we go back to the first thing we did Where we had the neutral atom and we see how many electrons it had it had 11 So we got to put 11 electrons into this configuration The first two go in 1s because an S can only hold two The next two go in 2s because again an S can only hold two we're up to four Next is 2p P's can hold six two plus two is four plus six is ten one more to go And it goes in 3s Now for the ions electron configuration we go back to the number of electrons in the ion there were ten of them So we're going to put ten electrons in this configuration Again the first two go in 1s because that's all they can hold The next two go in 2s because that's all it can hold Then we have 2p and we're going to fill it up with six two plus two is four plus six is the ten that we need note all we did was knock off that 3s one that was at the end of the configuration and that makes sense when we consider what it had to do to become stable What it had to do to become stable was lose one electron So basically we just lop that one electron off At this point we have ten electrons Ten electrons and it's electron configuration would match The electron configuration of me. I know you want to do more so let's do chlorine because this is just That's a lot of fun as you know Let's start out with a neutral atom The neutral atom if I get it in the screen here. I'm not watching the camera It's 17 So we got to put 17 electrons into our electron configuration S2 to S2 to p6 that's because that gets us up to 10 We still got some more to go we got seven more to go There's two more. So that's 12 five more to go They go right there three p5 pure rules can hold six, but we don't have to fill it up if it's the last one Just five in that one now. We got a look at the ion the ion had 18 So again one s2 Two s2 to p6 takes me up to 10 three s2 Takes me up to 12. I got six more And they all fit in that p orbital See what we did here is we just took that incomplete p orbital at the end and we filled it up because that's what it Takes to make it stable Think if we look back at what it did to become stable that makes sense it gained one electron We were only at p5 so we could put that one new electron in p6 2 plus 2 is 4 plus 6 is 10 plus 2 is 12 plus 6 is 18 and 18 Is the pirates favorite element? our god our That should be enough fun and excitement to get you through the first few things that we're doing here I'll add some more as I Review some more and we already do have a video for nomenclature, so I don't think I have to do another one for that We already have a video for the crisscross methods. I don't think I have to do one for that, but I will do one eventually for Lewis dot diagrams and modeling ionic bonding