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Moving to another question will save this response:Question 23What is the formal charge on the carbon atom in the structure

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Moving to another question will save this response: Question 23 What is the formal charge on the carbon atom in the structure below? 7 =a Moving m queston 61v Lhds response


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Lewis structure of the molecule, What is the formal charge on carbon?

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So before calculating the formal charge, you want to draw the Louis structure out for each one of these molecules or compounds. And so, for example, we have ozone here also knows, try oxygen. And so we count the number of total balance electrons, and so that allows us to draw the Louis structure. And so I went ahead and drew the little structure of heat for each one of these. And so now we can go on determined the formal charge for the indicated Adam.

And so to do this, we need to take the number of Valence electrons that for the Adam that they're asking for the formal charges. And then we need to subtract this from the number of non body electrons, plus the number of bonds around this Adam. And so let's look at our 1st 1 with try oxygen or ozone. And so we see here that looking at the pier a table, that there are six bands, electrons with oxygen, and so when we're currently have formal charge for this oxygen, we can say that there are six bands, electrons minus the number of non bonding electrons, and you can see that there are a total of two non bonding electrons right here. And so these were not participating, bonding.

And so this will go here, and then we can add this up with the number of bonds, we can see that there are 123 bonds. And so this gives us a total of a plus one charge moving on to the next one of ale aged four with the minus one charge. We will calculate the total number of immense electrons and see that because of this minus one charge, we're going to add and like Tom because this negative charge indicates that they're more electrons. And so here I do the Louis structure. And as you can see here that there are no lone pairs around this aluminum Adam that we're trying to find the formal charge on.

And so, looking at the period table, we're going to calculate the formal charge. I'm using the number of fans electrons with aluminum, which is three minus the number of non bonding electrons here, which is zero because they're no lone pairs or loan electrons. And so then we can add at the number of bonds and there are four bonds, all two hydrogen atoms. And so this gives us a total of a minus one charge on this central aluminum Adam. So next we have this quarry Anne on.

And so this one, if you draw the Louis structure without the's double bonds here in, find that this is going to have a two plus charge, and then these we're gonna have a one minus charge, and so this would be highly unstable and unfavorable. And so what we have to do here was to give this to two double bonds to stabilize this. And so, if you remember from the octet expansion rules that chlorine is based on the period table is located, and period three and so it can expand it on its octet. And so this is our most stable Lewis structure here. And so now we can go ahead and calculate the formal charge on the central chlorine atom.

And so we see from the pure table that there are seven valence electrons. So subtract this from the number of non bonding electrons, and so there are two from right here, and then we can add this to the number bonds. And so if you count them up. There are 12345 And so this gives us a formal charge of zero. Okay, let's move on to our next one.

And so I'm for the central Adam going to the period table. We see that it has a, um has four valence electrons Subtracting this from the number of non binding like John's. And there are no lone pairs here on. And so then we can add this to the number of bonds and there are six bonds to Florian Adams, Okay, and then this gives us a total of a minus two charge. And so, lastly, we have clf three and so drawing out the Louis structure here, there are two lone pairs on the central chlorine atom inside.

When we want the form in charge of this chlorine, we're going to include these non Bonnie electrons, and that's something to keep in mind as well. And so we know chlorine has seven valence electrons, and here we have a total of four non bonding electrons, and so then we can add this to the number of bonds with just three. And then, lastly, this gives us a final formal chart of zero on this chlorine atom.

To calculate formal charge. It is equal to the number of valence electrons. Subtract half the number of bonding electrons. Subtract the number of non bonding electrons. Let's calculate the formal charge for each atom for a in the Cyan eight iron sign.

Eight. Iron this iron here to calculate the formal charge of nitrogen, we'll abbreviate FC nitrogen has five billion electrons, minus number of bonding. Electrons is four, and the number of non bonding electrons is for the formal charge on nitrogen is equal to minus one carbon. The formal charge Carbon has four valence electrons, minus half the number of bonding electrons. There is zero non bonding electrons.

The formal charge for carbon works out to zero and for oxygen. On the right hand side, the formal charge is equal to oxygen. Here has six films. Electrons has four bonding electrons for non bonding electrons in the formal charge of oxygen works out to be zero. So if we include these in the molecule, nitrogen has a formal treasure of minus one.

Carbon zero Oxygen zero. Mhm. Now let's calculate the formal charge in the ozone molecule a lone pairs in, so we'll first start with the oxygen on the left formal charge. Oxygen has six valence electrons, two bonding. Six.

Non bonding formal charge works out to be minus one for the oxygen in the middle. Formal charges equal to six minus half, and we have six bonding electrons to non bonding. The formal charge works out to be plus one and for the oxygen on the far right. Formal charges equal six minus half number of bonding electrons when it's non bonding electrons and the formal charge here works out to be zero, so the formal charge would be minus one plus one and zero for the ozone molecule..

Let us now solve this problem from the chapter chemical bonding. But one basic concepts. This is based on the formal charge and we need to calculate the formal charge in the given structures. So let us understand the formula. Former judge Formal charge is equal to number of where in the electrons in the free item minus numbers of lone pair electrons in the living structure of the given substance minus half the number of born P electrons in the given level structure.

So first of all, let us draw the living structure of this Oh three. We can draw it as oxygen, single bond, oxygen and double born with an extra oxygen and putting the lone pairs of electrons, we can have this structure now. This is the central oxygen it, um for which we need to calculate a formal charge that is, formal charges equals to six valence electron in the free oxygen eight um minus two lone pair electrons here in the structure minus half into six born Pierre electrons in the structure and all calculating. We get the value of plus one, which is the formal charge on the central oxygen atom in three molecule. The second one is aluminum in a l H four.

Now writing the Levis structure for this iron, we can have this now calculating the formal charges. And William, we can right three in the free aluminum atom, minus zero lone pairs shown in the structure minus half and 28 born pair electrons. And this gives the value as minus one. The next one is chlorine in seal 03 negatives. Let us do the structure of this iron.

It can be represented as the given structure. No calculating the formal charges, including we can have seven valence electrons in the free chlorine atom minus two lone pair electrons on the clothing in this structure minus half into 10 born pairs of electrons then on calculating rigid the value as zero. So there is zero formal charge on declaring in this given iron. The next one is to calculate the formal charge in silicon in S I F six to negative. Now let us draw.

The liver structure of this iron can be represented by connecting six flooring items by single born with silicon in the center, and each Florentine has three lone pairs of electrons. Overall, there is too negative. Judge on this molecule now calculating. Using the given formula, we can calculate formal charge of silicon that is four valence electrons in the free silicon minus zero Electrons show in the silicon minus half into 12 electrons for their bones. I know in calculating we get minus two as the formal charge on silicon.

Then next is chlorine in seal F three. If we draw the structure of CLF three, we can draw it like this, including in the center, with two lone pairs on including and three lone pairs on each of the flooring. Now mhm calculating the formal charge on chlorine. We can have seven wells electrons in the free chlorine, minus four electrons as lone pairs in the structure, minus half multiplied by six electrons of the bond. Then, on calculating, we get the value as zero.

So there is zero formal charge on the chlorine atom in the given structure. So these are the formal charges, as asked in each part of the problem. Yeah,.

Every day in this video we are going to draw the structure of hydroxy airline. We're gonna sign the formal charges to it and then we'll look up the actual structure for drugs Dolomite and check if the formal charges coincide with the actual structure. Okay, so to start off we need to identify the total number of valence electrons and it will be three. Sorry It is one electron fire region times three plus five valence electrons for nitrogen plus six valence electrons for oxygen. This gives a total of 14.

So draw this. So now we can draw the blood structure. So nitrogen is the least. Electoral negative elements are put it in the middle and the oxygen and hydrogen then we assign the bonding electrons. So there's 2, 4, 68.

These are all stable nitrogen is a full oct eight. So the remaining six electrons will go on to oxygen right now. We need to calculate the formal charges for each of them. So for hydrogen for each of the elements for hydrogen. So it's equal to the Total number of valence electrons, hydrogen which is one and then we subtract the number one de valence electrons which is zero for hydrogen And then we subtract the total of electrons hydrogen which is two divided by two.

So that's two oh two and that's zero. So the formal charges will be zero. All the hydrogen singers there funding the same and then the formal charge for nitrogen Valence electrons is five minus we have zero 9.8 Electrons. And then we have quite a total of eight bonding electrons over to And so the formal charge for nitrogen is plus one And then for oxygen We have six valence electrons minus. We have got to cease valence electrons that are not bonding and then we have got to Bonding electrons divided by two and that is culture zero.

So those are the charges for more charges for drugs. Now we can have a second structure. five drugs so am I. So still the total number of valence electrons is 14. So we put the nitrogen and then the oxygen where we will have one hydrogen responding to oxygen and then we've got the other two ponding to nitrogen.

So we assigned it to the finding peers of electrons. So it's 2, 4, 6, 8 electrons. And so we've got six more non nitrogen requires too and that is now stable. So the remaining for are placed on the oxygen now to calculate the formal charges. Okay, so for hydrogen we've got one.

I know zero minus the two, one electrons or two. You got zero for nitrogen We have five valence electrons -2 valence electrons that are not bonding -6 electrons that are bonding developed to Which is equal to zero and for oxygen it is six electrons minus four Non Bonding Electrons -2. So minus four Bonding electrons divided by two equal to zero. And now when we compare this with the actual structure for drugs of women will, we can notice that the structure that gives the zero formal charges is consistent with the actuals with the actual structure. So this one is our structure for, Hey, don't slamming.

Thank you..

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