Draw the Lewis structure for each of the following:
b. H...

Question

Draw the Lewis structure for each of the following:

b. H₂NOH (N is the central atom)

Accepted Answer

Welcome back, everyone. We need to consider the bonding preference of each atom and show the best Lewis dot structure for N methyl hydroxylamine H three C H N O H where N here is going to be our central atom. Now, we're going to need to based on this chemical formula given for N methyl hydroxylamine H three C H N O H calculate total valence electrons in order to draw our structure. So beginning with our atom hydrogen in our chemical formula, we have a subscript of three next to the first hydrogen indicating we have a total of three moles plus our two additional hydrogens within our chemical formula which give us a total of five atoms of hydrogen. Now recall that hydrogen is located in group one a on our periodic table corresponding to one valence electron. So we're going to take this one vols electron and multiply by our five atoms of hydrogen and they will yield in total a contribution of five valence electrons. Next, we have our atom carbon which we just have one carbon within our chemical formula of N methyl hydroxylamine. And recall that carbon is located in group four A corresponding to four valence electrons. Next, we have our atom nitrogen, which again is our central atom. And we just have one mole of and nitrogen we should recognize is located in group five A on our periodic table corresponding to five valence electrons. And last, we have one mole of oxygen in our chemical formula where we should recall on our periodic table, oxygen is located in group six A corresponding to six valence electrons. So next, we're just going to take up the total of each of our valence electrons. So we'll have five plus four plus five plus six. And that's going to yield a total of 20 volt electrons for our structure. Now, next, we're going to draw nitrogen again as our central atom. And we're going to need to think of bonding preference for each of the atoms making up our structure. So, beginning with nitrogen, let's recall that it has a bonding preference of having three covalent bonds to other non metal atoms and one lone pair. And next, we have the bonding preference of hydrogen which because it has just one valance electron is typically going to just be a terminal atom And basically just form one bond. Next, we have our bonding preference of carbon Which because it has four rounds, electrons will form four bonds to have a full octet and to be stable with the formal charge of zero. And last, we have oxygen's bonding preference, which because it's a group six, a element with six films electrons. It has a bonding preference of forming two bonds and having two lon pairs on itself to have a formal charge of zero. And a full octet. Take note that nitrogen, carbon and oxygen are all period two elements and must follow the octet rule along with hydrogen, which is across period one on our periodic table. So with this all in mind, if we understand that nitrogen should have three bonds and one lone pair in itself, we can draw in a lone pair on nitrogen at the top. And we're going to draw in our atom carbon on the left of nitrogen, then we would have oxygen to the right. And we can draw one of our five terminal hydrogens at the bottom of this nitrogen in the center. And with these atoms surrounding our central nitrogen, we're going to form a total of three covalent bonds. So that now we can observe that nitrogen is bonded by its bonding preference of having three bonds and one lone parent itself for its full octet and a formal charge of zero. And in summary, we've used a total of 2468 of our 20 vals electrons total. And this leaves us with a balance of 12 v electrons remaining. Now, next, because we've only used five or sorry, one of our five total hydrogen atoms we're going to need to fill in four more terminal hydrogens. And as we noted on the right, we have oxygen's bonding preference of forming two bonds to other atoms and having two lone pairs on itself. So we can go ahead and draw in another terminal hydrogen bonded to oxygen on the right. And then we would fill in two lone pairs on this oxygen atom. And in doing so, we would have used a total of six of our 12 volt electrons leaving us with a balance of six where now we can focus on our carbon at the leftmost end of our structure, which currently only has one covalent bond to our central nitrogen. So it's missing a total of three more bonds because again, it has a bonding preference of forming four bonds. And because we still have just two of our five hydrogens present in the structure, we can complete the bonding preference of carbon and its octet by making three covalent bonds to our remaining three terminal hydrogen atoms. And this is going to complete our structure and use up because we've drawn in those three bonds, our last six remaining electrons leaving us with a balance of zero. And this will be our final answer as the best Lewis structure for N methyl hydroxylamine because we have a net formal charge of zero and all of our atoms have a full octet and that formal charges of zero. So I hope that this made sense and let us know if you have any questions

Draw the Lewis structure for each of the following:
b. H₂NOH (N is the central atom)

Key Concepts

Lewis Structure

Valence Electrons

Molecular Geometry

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