Problem

For the molecule allene, $\mathrm{H}_{2} \mathrm{…

04:33

Problem 25 Easy Difficulty

A useful solvent that will dissolve salts as organic compounds is the compound acetonitrile, $\mathrm{H}_{3} \mathrm{CCN}$ . It is present in paint strippers.
(a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule.
(b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form ? bonds.
(c) Describe the atomic orbitals that form the $\pi$ bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.

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Chemistry 101

Chemistry

Chapter 8

Advanced Theories of Covalent Bonding

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Video Transcript

all right, Question 91 is asking us about the molecule for acetone. And the formula for acetone is ch three two CEO Question part ay says to draw the Louis structure for acetone and predict the geometry at each carbon. So Asa tune it has a double bonded oxygen to the central carbon with two unshared pairs on it and carbon coming off of each side with the three hydrogen Tze That's the CH three coming up of each of off the central Adam. So there is our Louis structure for acetone. Um, that own refers to this structure right here the carbon with the double bonded oxygen and carpets on each side of that, then the we want the geometry at each carbon. So the central carbon here has three electron clouds around it each. The bonds are electron clouds. In this double bond accounts is one electron cloud. So there are three electron clouds or three electron domains. You might hear it said around the central Adam. Therefore, the central carbon, with its three electron domains, is gonna be have a shape of tribunal plainer, and then the outer carbons, the peripheral ones, the ones with the ch three on them. Okay, those carbons are have 1234 electron clouds around each of them. Therefore, they're going to be Tetra Hydro. And that answers part, eh? Part B says the acetone is as the tone molecule, polar or non polar, this oxygen in the middle here. This part right here is going to make this molecule very polar. That oxygen has a hi Elektra negativity. Um and we're going to create having this oxygen in the middle of the molecule like this. We're going to create a significant die pole. They're forthis molecule is very definitely a polar molecule. Hurt. See, we want to know what types of intra molecular forces as the tone molecules have between them. Well, first off, everything has London dispersion. All molecules have linden dispersion forces, so we will definitely have l d efs. And then because this is a polar molecule, there are also die. People die pole interactions happening. So those are to inter molecular forces that will be that will occur between aceto molecules. Finally, Part D says that one propane all. So the formula for one pro panel is ch three ch to see h 20 H that one prop it all has a molecular weight similar to acid tone. Um however, the one propane all boils. Its boiling point is at 97.2 degrees Celsius, where Assad tones boiling point that appear. It's boiling point is at 56.5 degrees, six Celsius. So why does the one propane all have such so much higher of a boiling point in? The answer has to do with inter Muckler forces. In order to boil, you have to break the Internet with forces that are holding the molecules together as a liquid. In the stronger or more types of inter Michael forces you have, the higher the boiling point will be, the more energy it will take to break apart those molecules. Um, and while the acetone only has London dispersion and die, people die pole. The pro panel has an added intermingle forces fairly strong one. And that is because of you. We have this hydrogen here bonded to an oxygen. We can also have hydrogen bonding with the one profitable and hydrogen bonding is a strong type of inter michaela force between molecules. Therefore, these molecules are gonna be held together more tightly. They're gonna It's gonna take more energy to break those a trim uncle of forces. Therefore, it has the higher boiling point.

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