Sorry, I'm later. Hi. Okay, so we'll just get straight in with the content today. Now we're going to be doing chemistry again because we did biology on Friday. And so I just want na do a little bit of a recap of the last thing that we did in the chemistry lesson so that you know the point at which we're picking up from so in the end of the last week's lesson for chemistry, we started to look at the periodic table information and what it means and how we can draw an atom based on the information that we can gather from the periodic table. So we looked at this helium atom, the helium information on the periodic table. And remember me saying that here at the top we have the number four, which is the MaaS number. Okay, so there at the top, the number four, the MaaS number. That always tells us the number of protons plus neutrons. So the total number in the nucleus. Then down here we had the smaller number, so the number two. This tells us the proton number, so the number of protons. And then the final thing we learned was that in an atom, you always have the same number of protons as electrons. Okay? So electrons and protons are always the same. So if you've got two plus, you also have two minus because they have to balance each other out. So the last thing that we did was we worked out how many protons, neutrons and electrons were present in an atom of bora using the periodic table information. So this number here was five. So that told us that we had five protons, right? Because that's the proton number. But we also knew that if we had five protons, we also had to have five electrons too, because they have to be the same. And then we know that this number is protons plus neutrons. So if we know that we have eleven in total and we have five protons, we know that we have a total of six neutrons. So to find out the neutron number, we always do the MaaS number, this one. Take away the proton number, this one, okay? And that gives us the number of neutrons. So we're going to start by doing a little bit of practice, okay, with three elements. First of all, then we're gonna to move on to how many electrons can go in the different shells. And then we would look at the groups on the periodic table if we get time. So with lithium, okay, we know that the bottom number is three. So this tells us that there are three protons, okay? So there are three protons. That number always tells us the number of protons. So now I know lithium has three protons plus. Now that also means that lithium has to have three electrons, because I know that the plus and the minus must always be the same. Now using this number, how many neutrons does lithium have? Four. Well done. Four, excellent. Because there are seven altogether three protons. So there's four in terms of neutrons. Well done. Okay, let's have a go. So I've done that one. Let's have a go at sodium then. So I'll leave this up. So you tell me how many protons, electrons and neutrons does sodium have? The next element. Protons, eleven protons. And if eleven electrons and love neutrons, excellent. Well done. So eleven protons, eleven electrons and twelve neutrons. And then the last one, iron. 26 protons, 26 electrons and 30 blue Trowell done fantastic. So we're happy with that. Okay, well done too. That's what the periodic information, the numbers tell you. Brilliant. Great start. Okay, so now we're gonna to move on to something new called the electron configuration. So before we do that, I'm gonna to scroll back up to this image of the atom that we drew last week. Now remember, the atom has the protons and the neutrons in the middle, and we call that area the nucleus, bit similar to the nucleus of a cell. The word is nucleus. So the protons and the neutrons are in the nucleus, but the electrons around the outside. And remember, they orbit around, so they don't just stay in one place, they all move around the outer. Well, not just the outer, but the inner too. They just move around their pathways, their shells, we call them. So they're always moving. But sometimes you'll see atoms with one shell. Sometimes you'll see atoms with two shells, sometimes with three. Like here I drew one shell for helium, but I've drawn two shells for boron. So we're going to learn why that is and how many electrons can go in each shell. So you correctly identified here that sodium has eleven protons and eleven electrons. So that's what I've drawn down here. Okay? I've drawn the nucleus of sodium. So in there there is eleven electrons, sorry, eleven protons and twelve neutrons. Okay, so in here, eleven protons and twelve neutrons. Here are your eleven electrons and we're gonna to figure out where they all go. Okay? So sodium has eleven electrons. You worked that one out before. Sodium has eleven electrons. So we're going to figure out where these electrons go. So first of all, shell number one, I'm going to take two of these electrons and put those two in the first shell. Now why I'm doing that is because the first shell or the first pathway, the first electron shell. Can hold a maximum of two electrons. Okay? So there will never be more than two electrons in the first shell. That's it. It's full now. So this shell is full because it has two electrons in it. The second shell can hold eight electrons. Okay? So the second shell. Can hold a maximum. Of eight electrons. So the first one's the smallest, okay, the second one can hold eight. So we already know that we've got two in here in the first shell. Now I'm going to add the next eight into the second shell. So one, two, three, four, five. Seven, eight. Okay, so I've now put eight more electrons in nutshell and it's full now. It has a full shell. There's still one left though. Okay, I've still got one more electron. My first shell is full. My second shell is full, but I've got one more. So I have to open up a third shell. Okay, so that's where the third one here comes in. Let me just copy this. So now you already have your first ten electrons, and I can put that eleventh one, the last one here, into my final shell around the outside into that third one. Now this shell is not full, okay, because the third shell also has a maximum of eight, okay? So the third shell. Can? Hold a maximum. Of eight electrons. Now for p stage three and gcse, that's it. We don't need to know any more shells. There are more. Okay? So as atoms get bigger and bigger, they have more and more shells. We only have to know about the first three, okay? So the first shell can hold two, the second shell can hold eight, and the third shell can hold eight. Now there are a couple of rules when drawing the electron configuration. So first of all. Each shell has its own maximum capacity. We've already talked about that. So each shell has a maximum capacity, which means it can only hold a set number of electrons. So each shell has a maximum capacity. We cannot go over that. So the first shell can only hold two electrons. So you can't put three in there. There's no space, only two. So we cannot go over the maximum. The second rule is. A shell must be filled. Before a new one is opened. Okay? So what I mean by that is before a new one is opened. So what I mean by that is with sodium, okay? We said that it has three shells. Okay? So one. Two. Three now it has eleven electrons in total. Okay, so there's I'm only drawing the shells and the electrons here. I'm not drawing the protons and neutrons again right now. So it has three shells. So the first one can hold two right? So I'm gonna to put two in there. The second one can hold eight but I'm only gonna to put four in there. I'm gonna to do one, two, three, four and then how many have I got left over? So six. So I'm going to put five in the outer shell. Okay now this is wrong because the second shell is not full. This shell is not full here. This second one. So this shell is not full. So we would never open another shell before filling up the first one. So this shell. Is not full. This would never, ever happen. So what youactually have to do is this youhave to have your three shells. First of all, you do the first one. So you've got one, two in there. Now that's full. Now we move on to the next one. Then one, two, three, four, and I'm on seone two, three, four, five, six, seven, eight. Now that shell is full, we move on to the next one and then we just have one left over. Okay? So in this one, the first two shells are full. So the outer shell is the only one that is allowed to be not full, okay? Because you you might not have enough electrons to fulfill it. So the outer shell is the only shell. That can exist without being full because it's the last one. So you might not fill the last one. In fact, usually you don't, but we have to fill the others. So this is always the outer shell, okay? So the one on the outside is the outer shell. That's the outer shell of sodium. If you only have one shell, then that's your outer shell, okay? So with helium, even though it only has one shell, that's what we count as its outer shell because it's the one on the outside, okay? With boron, boron had two shells, so this one is the outer shell, okay? So the outer shell is just always the one on the outside. Your outer shell can be your first shell. It can be your second shell, or it can be your third shell. It depends how many shells that your atom has, okay? So outer shell is always the last one, right? I'm just going to write out some information on one of a new element and we're going to figure out how many shells it has based on the information. Okay, so let's go back to let's go back to lithium. Okay, let's take lithium. Here we go. We said correctly, you managed to identify this one. Oh no, I did this one, didn't I? We said that lithium has three protons and three electrons. Okay? Now remember, here are the rules, shell one. Two electrons maximum. Shell two. Eight electrons maximum. And shelf three, also eight electrons maximum. Okay, so shell one, 23. Okay, so we're going to start with lithium. Okay, so lithium has three electrons, so let's draw them out. So here are lithiums three electrons. Okay, so here we are. That's number one. That's number two and that's number three. Okay? So it has three electrons. So if I start with one shell, okay, so here is just the first shell. How many electrons can I put in that first shell? Two, well done. So I'm going to put these two there. Okay, so what do I need to do next? Make a new shell. Make a new shell. Perfect. So there's the next one. And then I just have that one electron there. Okay, so for lithium, this is the outer shell, and it has one electron in the outer shuokay. Now when it comes to writing electron configuration, we kind of put numbers together with commas in between them to say how many electrons are in each shell. So let me just go back here to sodium. Okay? So this was our final atom of sodium, okay? This had eleven electrons in it. So the way I write the electron configuration is this, okay? So electron configuration, I write how many electrons are in the first shell? Two with a comma. Okay. How many electrons are in the second shell? Eight with a comma. How many electrons are in the third shell? One. Okay, so that is my electron configuration. So you can see there now that there are three shells, because there are three numbers. There's two electrons in the first shell, there's eight electrons in the second shell, and there's just one electron in the third shell. So that is your electron configuration. Let me go back up to where we drew boron. Okay? So boron to write the electron configuration. Just means how the electrons are arranged, okay? And it's a way that we express it numerically. So the electron configuration for boron, okay? How many electrons are in the first shell? Two. Comma. How many electrons are in the second shell? Three. Okay. And that's it. So we know that there are two shells because there are two numbers. I know that there are two electrons in the first shell and that there are three electrons in my second shell. Okay, next one. Then the one that we just did for lithium, the electron configuration would be. So the electron configuration would be two because there's two electrons in the first shell and then one because there's only one electron in the second shell. Okay, so that's how I would write my electron configuration, right? We're gonna to have another go. I am gonna to copy this so you can see this and I'm just gonna to let you do this one yourself. Now you Yeah what I'll do is I'll give you the pen I'll make this smaller and I want you to draw the atom on the side of the screen here. Let's see if I can can I make this smaller? Surely I can Yeah I can't make any smaller than that but if I give you the pen you can write the atomic structure over here. Okay, so like something like that over here in whatever color you want to so I'm gonna to give you which element am I gonna to give you 1s? Let me just have a look at my periodic table. I'm going to go with magnesium. Okay, so I'm going to put the information for magnesium here and you've got to figure out how many electrons magnesium has and therefore what an atom of magnesium would look like. Okay, so magnesium. Okay. And I'm leaving the rules up there as well. I would maybe just if I was you, use you know just use the pen and draw the dots like this because it doesn't have to be perfect, because it might be a bit easier than trying to get the circle shape. Yeah, that's perfect. Just one thing. So you've drawn three on the outer shell. How many have you got in your second shell? Oh, I forgot, there we go. And then so how many would be left on the outer shell? Well, if you've already done two plus eight in the first two shells. Or but what's two plus eight? N ten. So you've already drawn ten in the first two shells. So how many are left for the last shell? Two. Well done. There we go. Perfect. Okay, great work. Well done. You did really, really well done. And I could see you thinking through it as you were going through. I could see you thinking about drawing each new shell. Okay, so well done there. I'm did a screenshot that so I can add it into our note. Okay. So Isabella, how would the electron configuration be? You know like this number? What would we write for magnesium? 282. Brilliant. Well done. So the electron configuration would be 282. Okay excellent well done. Let's just have a go one more just so I know for sure and then we will move on to talk about the periodic table. So I'm gonna to go with I'm going to go with neon actually. Okay, so I'm just going to make this one smaller. So same thing again now and this time we're going to do neon. So this is neon. The numbers are. Okay, so just have a go if you can. I wonder if I can just delete this whole link? There we go. So just have a go at drawing the electron shelves for neon please. Okay, perfect. That is absolutely brilliant, brother. So what would the electron configuration be? 828. Well done, Isabella. That is perfect. Let me take screenshot of this one so I can add it in there. Okay, excellent. Yes. So Interestingly, neon has a full outer shell, doesn't it? Because there's no more space in that outer shell. Now if it was to add an electron, it would have to add a new shell. So that's something to keep in mind because that's significant a bit later on. Okay, great work. Well done. Right now we're going to look at the periodic table. Okay, so this periodic table, you will have seen it before. We talked about it very briefly the other day. We're going to talk about more about where the atoms are on the periodic table and what that tells us about them. So we're not necessarily going to talk about the number of protons, neutrons and electrons. Now we're going to talk about the structure of the whole atom based on where it is. So as you can see, this periodic table has these two outlined. Okay? So these are your groups. So this is group one, this is group two. This is group three, group four, group five, group six, group seven, and group zero. Okay? So group zero is a little bit different to the others. And you might think, well, what about these in the middle? Now these do not have a group. We call these the transition metals. So don't worry about those for now. We are going to talk about those at a later date. Okay? So just don't worry about these for now. We want to focus on the groups. So group one is here, group two is here, group three, group four, group five, group six, group seven, and then group zero. So that's one, two, three, four, five, six, seven and then zero. Now the group number actually tells us some information about the element. So the group tells us the number. Of electrons. In the outer shell. Of an atom and that tells you the group. Okay. So for example, group one, all of the elements in group one have one electron in their outer shell. Now we did one of these, didn't we? We had sodium. We did sodium. So if the rule is group one tells us that all elements in group one have one electron in their outer shell, let's go back up to sodium and see if it's let's have a look. Is it Yeah, sodium has one electron in its outer shell. It had two, then eight, and then just the one on the outside. Okay. Did we do lithium? I don't think we did lithium or did we? Yes, we did. Here we go. Lithiumalso in group one. Okay, so that tells us that lithium should also have one electron in its outer shell. Is that Yeah, lithium does have one electron in its outer shell. Okay? So the group number tells you the number of electrons in the outer shell. So if an element is in group one, it has one electron in the outer shell. So it doesn't matter how many shells it has, it will always have one as the last number. So for example, lithium is two, one, sodium is two, eight, one, potassium is two, eight, eight, one. Okay? But notice how they all have one at the end. So lithium is the first one in group one that's here. Okay? Then we have sodium, which is the second one here. And then we have potassium, which is the third one here. And the reason I'm not going beyond that, Isabella, is because we don't talk about the other elements. They're too big. Okay? So the first three in group one will be the will be the metals that we talk about. So if you're in group one, you have one electron in your outer shell. So let's go back up to when we did boron. Okay, so let's go to boron. So what group do you think that boron should be in? Also third the one the third group excellent. And let's see is boron in group three. Yep, there it is. Okay, boron is in group three right there. Okay, well done. So the group number tells us the number of electrons in the outer shell. The period number tells us the number of shells. Okay, so the number. Of shells that an atom has. Okay, so that an atom has. So the periods are the rows. The groups go down and the periods go across. Okay? So this here, this is period two. This is period three. This is period four, period five, period six, period seven, period one. H should actually be here. H is part of period one. There are only two elements in period one because there's only two spaces. Okay, so hydrogen and helium are period one. So for example, lithium is in period two, group one. So we know that because it's in group one, it has one electron on the outer shell. Because it's in period two, it has two shells. Let's double check it. Lithium, two shells, one electron on the outer shelell. Yeah, that is exactly how we drew it. So let's have a look at these three elements and we're gonna to try and identify them without even saying how many electrons they have. So let's start with the first one. How many shells does this first element have? Two shells. So it's in period two, right? So two shells, period two, how many outer shell electrons does it have? One doesn't know three, three, so three outer electrons. So that tells us it's got to be in group three, right? It's got to be in group three, sort of group three. So we know that this element is period two, group three. So without even counting the electrons, if I go up period two, group three here, this is boron. Okay? So that's boron. Let's do the next one. So this element is boron. Okay, let's do the next one. How many shelves does the next one have? So three shells. So we know it's in period three. How many outer shell electrons does it have? One, one electron. So we know that it's in period three, group one. So what element would this be if I zoom in period three, group one? Na na, well done. So that's sodium. So boron is b sodium is na. Okay, great work. And a then the last one. Okay, now this is interesting. How many shells does it have? It has one. How many outer shell electrons does it have? Now here, this is where things get slightly different. Okay? This is where this element here is not in group two. Okay? This element here is not in group two. Even though we've just learned that the number of outer shell electrons tells us the group, there is one exception to the rule. And that rule is if the outer shell of an atom is full. So if the outer shell of an atom is full. The element is in group zero, okay? So the element is in group zero. The zero. Is for zero spaces left in the shell. Okay? So the zero spaces left in the shell. Now this final atom is in group zero because it has two electrons in its outer shell, right? And what did we say was the maximum capacity of two shuthe first shell? Sorry. How many what's the maximum number of electrons that can go in the first shell? So this shell is full, isn't it? Because there's two in there already. So that would be in group zero. Okay. So let's go back up. If it's in period one in group zero, which element do you think that it is? Eight. H. It's got a bit in group zero right on the end. E H, exactly. This is helium. Okay? It's H E helium. So helium gas. He e, okay, right. That brings me onto this part, which is what we're gonna to talk about. We are gonna to talk about group seven right now. I don't know if I've got one where it's outlined. No, maybe not. I'll just add in my overall period table like this again. So group zero, which is the noble gases at the end. Okay. So we are specifically now going to talk about group zero. The one right on the end, because there are a couple of groups that we have to know, group one, group seven and group zero. Okay, we kind of have to study those in a bit more detail. So group zero are the noble gases, we call them. So group zero, the noble gases. So the noble gases. Now every element, like we said in group zero, has a full outer shell. So we know that helium has an electron configuration of two. Okay? So this here is helium, right? This is helium electron configuration of two. There are two electrons. Neon was one that you drew before, okay? So I asked you to draw neon and you drew me two shells, the first one with two electrons and the second one with, Hey, okay, so you did this neon. Okay so we got one, two, three, four, five, six, seven. I'm not made enough space there. Eight. So there's eight electrons on the outer shell. So again that is full, right? So there's 28. The first shell is full, which it always has to be if we're gonna open a second one anyway. And then the second shell is also full. So this is helium, this is neon. There are ten electrons in neon. The electron configuration is two. For this one, it is 28. Let's do the next one. Then let's do argon. Okay, so let's do argon. How many electrons would there be? Argon? 1818. So if I draw another shell, how many electrons should be in that outer shell? If I add one more shell, which I know I have to because this argon is in period three, so it's in the third row. So I know there's gonna to be three shells. How many electrons need to be in the third shell? Yeah, well done. So one. One, two, three, four, five, six, seven, eight. So I have another eight electrons and so that shell is also full. So neon, helium and argon, all three of those are noble gases. Argon has a total of 18 and its electron configuration is going to be two, eight, eight. Okay, so two, eight, eight, a little bit of a trick as well to figure out how to write the electron configuration of something really quickly. Okay, so we're gonna to choose an element. So if I choose, I'm going to choose calcium. Okay, so here's calcium. Now which group is calcium in? The second group. Yeah. So it's in group two. Which period is calcium in. Or period four. So if calcium in group two period four, what does that tell you about calcium? For electrons. And just once that it's in group two, period four. So how many electrons does it have on the outer shell? That's the number of. Oh, two. Okay. So calcium has two electrons on the outer shell. And what does it have? Four of? Lord south, yes. So it has four shells. Now, before we even know how many electrons it has, if it has four shells, you know that the first three shells have to be full, don't you? Yeah, the first three are full. So how many shells, how many electrons can go in the first shell? Okay, how many electrons can go in the second shell? Eight, eight, how many electrons can go in the third shell? Okay. And how many electrons did we say calcium has in its outer shell? Just double check. So even without looking at the number of electrons, I can write the electron configuration. Okay? So even without knowing the number of electrons, just by knowing where something is on the periodic table, I've been able to write that because I know calcium is in group two, so it has two electrons on the outer shell. I know that it has four shells because it's in period four. We also know that if there are four shells, the first three are full, because, as we said, each time we open a new shell, the one below it has to be full. So I know that the first shell is going to have two, the second shell is going to have eight. The third shell is going to have eight. And because there's a fourth one, that's the outer shell. And I know that there's two electrons in there because it's group two. Let's try this trick with another one. Let's do, let's do silicon. Okay? So let's do silicon. This one over here. What group is silicon in? Group four, what period is silicon in? 33, okay, so silicon. Is group four period three. Okay. So tell me what does that tell us about silicon? It has. Has two, has four electrons on the outer shwell done. Okay. So what would the electron configuration be? Two, eight, four. Well done. Brilliant. Okay, fantastic. Great work. So the electron configuration, so there's a few ways that we can work out electron configuration. Either you can count the number of electrons and you can physically you know identify it, or you can have a look at the periods and the rows, sorry, the periin, the groups, and you can figure it out that way. Okay, really great work. Well done. Okay. That wasn't the end for the noble gases I just had in my mind to go through that trick. So the noble gases are a very unique group of elements. Okay, so group zero are the noble gases, as I mentioned above. So groups zero, the noble gases, all elements in this group have a full outer shell. Now let me tell you the significance of a full outer shell in chemistry. Oh, what have I written there? In chemistry, having a full outer shell means that the atom. Is extremely stable. Okay, extremely stable, which means it is really, really unreactive. Okay? Extremely stable and unreactive. Now, what do you think I mean by unreactive? If something is unreactive, what does that mean? Real o. Say that again. Real real. Yeah, okay, what do you mean by that real? Not it's not wrong. It's. Real, okay. So when we say unreactive in chemistry, what this word means is these elements will not form chemical reactions or take part in chemical reactions with other elements. So these atoms. Will not. Take part in chemical reactions. So they will not take part in chemical reactions with other atoms easily, or maybe not at all. So they will not take part. Unreactive might not always mean that they won't, but it might mean that they don't do it very easily. So these atoms will not take part in chemical reactions with other atoms easily, if at all. Okay, easily, if at all. So helium does not form bonds. So helium. Neon. And argon. Do not. Form bonds. With other atoms, okay? So they don't they don't take part in bonds. They don't form molecules. They don't do chemical reactions. They are completely uninterested because they are unreactive. So what that tells us is, if you have a full outer shell, you don't need to change anything about yourself. If an atom has a full outer shell, there is no need to change. There is no space on the outer shell. These elements could not gain any electrons. They couldn't gain any more even if they wanted to, because they are already full. And that's what makes them stable. Okay? So in chemistry, stability, chemical stability, is having a full outer shelf. That's what stability means. If an element doesn't have a full outer shell, it's unstable, it's reactive. Whereas if it has a full outer shell, it's stable and it's unreactive. So helium could be near another helium atom. So if we had two helioms, they would never, ever bond together, okay? They would just stay like this. So helium, neon and argon, they never form bonds with anything else, whether it's with atoms of the same type or with atoms of different types. They would never do it. They don't need to. So I'm just going na get rid of this. And I'm going to say, in chemistry, stability is linked to the fullness of the outer shell. So in chemistry, atomic stability is linked to the fullness of the outer shell. Atoms with a full outer shell are stable and will not react. Atoms without a full outer shell are unstable and will react. Okay. So outer shell is really the important one. When we're talking about reactions and bonding. We don't consider the other shells because they're shielded almost. It doesn't really matter. They're already full anyway. The only one that matters is the outer shell. So to us, in chemistry, the outer shell is going to be our most important tool to helping us to predict whether an atom will be stable, unstable and how it will form bonds. Okay, right. We're going to stop there because I obviously don't have time to go through the actual idea of bonding with you. But next time we do have a chemistry lesson, we're gonna to be talking about bonding. Okay? We're gonna to be talking about covalent, ionic and metallic bonding. Now, are those words that you recognize? Do you recognize covalent bonding or metallic or ionic? No. Okay, that's fine. I'm going to send you a bit of reading to do. The next chemistry lesson will be in a few days, so it's quite a while off yet. So I'll give you a little bit of reading or watch a video to get some underlying information and then we'll get started straight on the bonding topic. Okay, Yeah. All right. Well, well done Isabella. You've done really well today. I will see you tomorrow for a lesson, but we'll be doing physics tomorrow. Okay, okay, okay. Bye bye. Bye bye. See you. Bye.