Ethyl propanoate, CH₃CH₂COOCH₂CH₃, gives a fruity pineapple-like smell. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many s and how many p bonds are in the molecule?

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well every once in this video we're trying to complete the electron dot structure of this compound right over here by adding necessary lone pair electrons. So we have um different elements here that we're working with, we're dealing with carbon, hydrogen, oxygen, nitrogen and chlorine. And each has a predictable amount of bonds and lone pairs that likes to have. So we'll go ahead and use those rules apply and complete this electron dot structure of deco finnic. So carbon likes to have four bonds to complete its octet. And we can see here that all the carbons in our element or in our molecule here will have four bonds. So don't doesn't need any lone pairs. So we'll just leave carbon ads is next element that will deal with is hydrogen. So all these terminal high regions here um all the way down here as well, it likes to have one bond because it needs to fulfill its duet role. So it just needs to vent electrons to be happy. So, in our structure here, all the hydrogen in a molecule um does have a single bond, so does not need any lone pairs. So the higher regions will be left alone. Next element that will analyzes oxygen. So all our oxygen's here is just this one and this one here. So auction likes to have two bonds and two lone pairs to fulfill its octet. And we can see here from the molecule that all of our oxygen atoms has two bonds in different variations. So this double bond here just to bonds. And then this terminal more terminal um auction has these two single bonds, so still two different bonds, but because it has two bonds going to go ahead and add those necessary to long pairs. So we'll go ahead and add those in here and the next element we'll go ahead and analyzes nitrogen. So nitrogen usually likes to have three bonds and one lone pair to fulfill its octet. So looking at the compound here, we see our one nitrogen and we see that it does have indeed three bonds to go ahead and add that one long, prepare one lone pair to go ahead and fulfill its octet. So go ahead and draw that one long pair in for nitrogen. And lastly we're dealing with chlorine in the small kill. We have this one chlorine off to the side here. So chlorine likes to have one bond and three lone pairs to fulfill its octet. So looking at the chlorine, like we said, we have just one singular bond here. So we need to add those three necessary lone pairs. So have three lone pairs surrounding this chlorine atom. And that's the answer to completing the electron dot structure of diclofenac

Ethyl propanoate, CH₃CH₂COOCH₂CH₃, gives a fruity pineapple-like smell. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many s and how many p bonds are in the molecule?

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Key Concepts

Lewis Structures

Types of Chemical Bonds

Hybridization

Ethyl propanoate, CH3CH2COOCH2CH3, gives a fruity pineapple-like smell. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many s and how many p bonds are in the molecule?

Recommended similar problem, with video answer:

Verified Solution

Key Concepts

Lewis Structures

Types of Chemical Bonds

Hybridization

Ethyl propanoate, CH₃CH₂COOCH₂CH₃, gives a fruity pineapple-like smell. (a) Draw the Lewis structure for the molecule, assuming that carbon always forms four bonds in its stable compounds. (b) How many s and how many p bonds are in the molecule?