Expand the following condensed structures into the correct structural formulas.
c. CH₃CH₂OCH₂Cl

Question

Expand the following condensed structures into the correct structural formulas.

c. CH₃CH₂OCH₂Cl

Accepted Answer

Welcome back, everyone, give the condensed structure of two chloral with oxy propane and expand it to its corresponding structural formula. So we need to begin by calculating total valence electrons for our compounds in which we call that for carbon. It's located on a periodic table in group for a corresponding to four valence electrons. Next, we want to recognize that we have a total of five carbon atoms in the structure in our formula. So we are going to multiply our four valence electrons times are five atoms of carbon in which we will have a contribution of 20 valence electrons from carbon. Now, moving on to hydrogen recall that hydrogen is located in group one, a corresponding to one valence electron in which we multiply by our 11 atoms of hydrogen in our in our formula. This will give a contribution of 11 valence electrons from hydrogen. Next, we have our atoms of oxygen in which we recall is located in group six A on the periodic table corresponding to six valence electrons notice that we just have one atom of oxygen. So this will give a contribution of just six valence electrons from oxygen. And lastly, we have chlorine, which we should recall is located in group 78 on the periodic table corresponding to seven valence electrons where we count a total of just one chlorine atom. So multiplying seven valence electrons times one atom gives us a contribution of seven valence electrons from chlorine. Taking the sum between all of our contribution of valence electrons. We come up with 44 valence electrons total for our structure. We want to make note of bonding preferences to maintain stability of our atoms. Recall that for carbon, it prefers to have four bonds. Recall that oxygen prefers to have one bond Or sorry, not one bond, but rather oxygen prefers to have two bonds and two lone pairs to be stable. And then recall that chlorine prefers to have one bond in any structure. So we're going to begin by drawing out the backbone of our structure in which we have our carbon atoms bonded to one another where we have again, a total of five carbon atoms. So we have three here four and actually let's make this atom in oxygen so that we can take care of our oxygen bonded to two bonds or two atoms. Rather, this would be four carbons so far where we would have our fifth carbon here and then our chlorine atom bonded here since we know it should, it prefers to only have one bond. Next, we can fill in our lone pairs on oxygen. So we'll have two lone pairs left for its directly attached 123456 valence electrons to be stable. And then we'll have three lone pairs on chlorine so that it has its directly attached 1234567 valence electrons, which is, which is what it expects to have being a group seven a atom to be stable and have a formal charge of zero. Now, we want to fill in our hydrogen. So we counted a total of 11 atoms of hydrogen in our structure. Meaning that for this first carbon, we have three hydrogen we can fill in. So we'll do this outside of our backbone. So that will be our next step is add hydrogen where we have now to our backbone. For the first carbon, we have three hydrogen, we can add, then we have two hydrogen, we can add to the second carbon giving it its four bonds. Then to this third carbon, we can also add two hydrogen also giving it four bonds to be stable. So far, we've used seven of our 11 hydrogen. For this fourth carbon, we can add two hydrogen bonds giving it four bonds to be stable. And for this fifth carbon, we also can add its two bonds to hydrogen to give it four bonds total to be stable. This use uses up our 11 hydrogen bonds and in summary, we've used up all of our 44 valence electrons which again include our lone pairs on our oxygen and chlorine atoms. So looking at our answer choices, the correct choice looks like it's going to be the structure which matches what we've drawn out, which is choice B as the correct condensed structure for two chloral it oxy propane. So B is our final answer. I hope this made sense and let us know if you have any questions.

Expand the following condensed structures into the correct structural formulas.
c. CH₃CH₂OCH₂Cl

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Expand the following condensed structures into the correct structural formulas. c. CH3CH2OCH2Cl

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Expand the following condensed structures into the correct structural formulas.
c. CH₃CH₂OCH₂Cl