How to write Structural and Dot and Cross Diagram | Convalent Bonding

[00:00:00]Hey everybody, welcome to this platform.

[00:00:03]This is the Chama Jacob and I'm pretty sure each and everybody is doing great this evening. I've got this and this, which I would like to discuss with you. So, let's start with what we call structural diagram in chemistry as well as a dot and cross diagram. Have you ever come across these two? So, let me show you what it means.

[00:00:33]So, when we talk about structural diagram, this is simply the bonding and it's also called covalent bonding, the same as this. So, it's just a different way of showing the diagram here and here of the same thing. So, let's do this. Let's say you've got a F.

[00:01:01]So, when you nicely check on your periodic table, this is a fluorine and fluorine has got seven electrons. The outer shell of fluorine has got seven electrons. So, let's say this is equal to seven electrons.

[00:01:27]So, basically to show the bonding of this fluorine with another one because there are two. Another one also seven electrons.

[00:01:45]So, there are seven electrons. Now, to show the bonding that will take place right between these two fluorines, it will be like this.

[00:01:58]You can see that there are seven electrons in the outermost shell. So, for you, you're going to write another fluorine, which is this and this. You can see they're right over here. And to show the structural the structural diagram of this fluorine, it's supposed to be You say, "Okay, if I get this bar, I write it like this to show that they are combining, okay? They are combining. So, from this seven, they will share one electron. If this and this share one electron, they're going to have eight electrons in the outer shell. Now, for structural diagram, you're just going to write the bar like this. And then, in your mind, you say, "Okay, this fluorine has shared one electron.

[00:02:54]>> [clears throat] >> This also has shared another one electron." So, so far, they've got two electrons each of them since they have shared one one, it's equal to two. So, now, out of these seven, how many electrons are remaining right here? They are going to be six of them.

[00:03:17]So, you just write them outside like this.

[00:03:20]So, this one has got 1 2 3 4 5 6 7 8.

[00:03:24]Remember, here they're sharing one one, which is equal to two. So, when you count, this is 1 2 3 4 5 6 7 8. Also, this one.

[00:03:35]Just like that.

[00:03:41]1 2 3 4 5 6 7 8. So, this is called structural diagram of a the covalent bonding.

[00:03:52]So, when covalent bonding is taking place and they've asked you to use structural diagram, this is how you do it. And of course, this can be called single single bonding or single covalent bonding. Okay? So, when you they talk about single, how do you now get to know that this is single? You just look at this single bar, just like this.

[00:04:22]I will show you the double, the way it will look. Now, let's try to move to dot and cross diagram on the same thing. So, we know that fluorine has got seven electrons.

[00:04:35]Even here, fluorine is seven electrons.

[00:04:39]So now, to show the dot and cross diagram, you're going to do this.

[00:04:50]There are two of them.

[00:04:52]This is F, fluorine, another one, fluorine. This one and this one. So, they will share each.

[00:05:00]Okay? Each one of them will share uh an electron.

[00:05:04]So, here there will be two electrons.

[00:05:10]So, this one will have one, two, three, four, five, six, seven. Now, they've shared here, meaning it has got eight electrons in the outermost shell. So, this is 1 2 3 4 5 6 7 8.

[00:05:29]So, this other one also is a sharing the dots.

[00:05:37]So, you have to differentiate.

[00:05:39]They are the same. They are all F. This is F and this is F, but they are sharing. Okay? Now, to show that they are different atoms, not really different, should I say they're two atoms that you have over the same, which is F and F. One of them should get X, the other one should get the dot. That's why it's called dot and cross. So, these are dots and cross. So, they'll come and share right here in between. This is where they're sharing. This one has donated one, and this one also has donated one. That's how it is.

[00:06:16]Let's try to do maybe oxygen.

[00:06:20]Oxygen, we know that oxygen has got six, okay, electrons.

[00:06:30]So, now, the two of them, if I get this oxygen right here, and another oxygen, they're bonding. These are nonmetal.

[00:06:44]They're bonding.

[00:06:45]So, we know that they've got six electrons each. So, how many electrons are missing for the outermost shell to be to be full? It's two. Meaning, this one is missing two electrons.

[00:07:05]So, what we're going to do here, we're going to say they will share. The two bars here will show like this. Now, on these two bars, remember each bar is containing how many electrons? Two. So, now, if they do this, meaning they have shared, and how many electrons do we have so far? They are four of them. Because there is this one, two, three, and four. They're sharing uh two each, and they are four all together, the electrons.

[00:07:39]So, here, since it was six, so they have shared one one each, meaning this one has remained with how many?

[00:07:47]I want you to see, it has remained with four.

[00:07:51]So, don't make that mistake. It has remained with four. And the way I'm writing this is not how it's supposed to be.

[00:07:58]This is not not how it's supposed to be.

[00:07:59]Oh, sorry.

[00:08:01]So, it's like this. So, just write them outside like this.

[00:08:06]So, in case you don't know, let me talk about what is happening here.

[00:08:10]So, there are these four, 1 2 3 4.

[00:08:14]Plus the four here, 1 2 3 4. On the bus, there are four. So, all together, there are eight for this one. Even this one also, if we do this, there are eight. So, this is structural diagram of what? Of oxygen.

[00:08:30]We can show here by simply doing the drawings like this.

[00:08:40]Okay. So, that's it. Now, they are sharing how many? Two each. So, one of them will have these one, two. The other one, one, two. So, that's how the four is coming about. They are sharing two each, and the total number of those electrons they are becoming how many?

[00:08:58]Four right here, where they are sharing.

[00:09:01]So, now, here, we can now write two of them like that. If you want, you can use the crosses, it's okay. If you want the dots, so I'll use the cross here, cross here, cross here, and here the dot, the dot, the dot, the dot. So, if we count, this is 1 2 3 4 5 6 7 8. 1 2 3 4 5 6 7 8. Just like that. And this is called double.

[00:09:33]This is double, 1 2.

[00:09:35]That's it.

[00:09:37]Let's try one more, which is uh nitrogen. We try nitrogen. How many electrons are there in nitrogen? This is something that is very important and something that you must be knowing. So, when it comes to nitrogen, let me write here. Nitrogen has got five. You need to know that it's five electrons.

[00:09:58]So, now showing this Let me Let me clear up here.

[00:10:02]So, showing this for for nitrogen you're going to say N.

[00:10:10]If there are two of them, you want to combine the nitrogens, two of them.

[00:10:14]There will be N and here also N, okay? So, remember they are sharing >> [snorts] >> three bars.

[00:10:25]Why three bars? It's because we've got five. And how many are missing?

[00:10:31]There uh three which are missing. Okay? Three electrons which are missing to make it eight. So, we're going to say these three bars are like this, meaning they've got This one has shared three and this one also has shared three. So, how many have remained here if we total up all of them here? We are remaining with uh uh Here is six, seven, eight. Two.

[00:10:58]Also here, two.

[00:10:59]Because each line is containing two electrons.

[00:11:04]So, these three lines, they have six electrons.

[00:11:10]So, now that's six. How many now are remaining for us to make eight? It's just two. So, one, two, one, two.

[00:11:18]And one quick thing. One quick thing.

[00:11:21]These bars will show you the the You can write representing these bars. For example, this one, you can write it as a 2 e like that. The number of electrons, there are two electrons. So, for this bar it has got two electrons. If this bar has got two electrons, what about this one?

[00:11:43]It has got four electrons.

[00:11:47]1 2 3 4. This one, it's a six electrons.

[00:11:54]I don't know why I'm putting in this.

[00:11:55]I'm thinking in mathematics. So, that's it.

[00:11:59]That's it for this one. And this is called triple.

[00:12:03]This is a triple bonding. This one, triple 1 2 3.

[00:12:07]So, here this is a single.

[00:12:13]This is double.

[00:12:17]So, for the triple here it will look like this.

[00:12:22]Remember here each is donating donating three. So, we shall have 1 2 3.

[00:12:32]1 2 3. And then here 1 2. So, 1 2 3 4 5 6 7 8. 1 2.

[00:12:42]1 2 3 4 5 6 7 8. Just like that. And this is also triple bonding.

[00:12:50]Thank you so much for watching. I guess you've learned one or two things out of this on how to do the covalent bonding of single, a double, and a triple. This has been Mr. Shamba Jacob. Please remember to share the video and bye-bye.