For each compound, draw the Lewis structure, determine the...

Name: Problem 55, Chapter 6: Chemistry: Structure and Properties
Uploaded: 2019-01-22T04:27:14-08:00
Duration: 5 min 16 s
Channel: Joshua Speer
Description: For each compound, draw the Lewis structure, determine the geometry using VSEPR theory, determine whether the molecule is polar, identify the hybridization of all interior atoms, and make a sketch of the molecule, according to valence bond theory, showing orbital overlap. a. COF2 (carbon is the central atom) b. S2Cl2 (ClSSCl) c. SF4

For each compound, draw the Lewis structure, determine the geometry using VSEPR theory, determine whether the molecule is polar, identify the hybridization of all interior atoms, and make a sketch of the molecule, according to valence bond theory, showing orbital overlap. a. COF2 (carbon is the central atom) b. S2Cl2 (ClSSCl) c. SF4

For each compound, draw the Lewis structure, determine the geometry using VSEPR theory, determine whether the molecule is polar, identify the hybridization of all interior atoms, and make a sketch of the molecule, according to valence bond theory, showing orbital overlap.
a. COF2 (carbon is the central atom)
b. S2Cl2 (ClSSCl)
c. SF4

Transcript

00:01 All right, so this question asks us to do a lot of things with this orbital here.

00:05 I'm only going to have enough room to do the lewis structure, so i'll just tell you guys what to do for the vesper structure.

00:15 So for this first molecule, we know that carbon is essential atoms.

00:18 We can start there.

00:20 It's got an oxygen and two fluorines attached to it.

00:27 And since that's everything, we know it's a neutral molecule.

00:30 We know carbon wants four bonds, oxygen wants to.

00:33 So we put an extra bond here.

00:36 Now everyone's happy.

00:39 We need to determine the hybridization of the interior atoms first.

00:46 So since carbon has three things around it, it's going to share those into three even orbitals.

00:51 That's going to be sp2.

00:53 And the extra p -orbital that we didn't blend into this hybridization mix makes that double bond with oxygen.

01:02 And so if we were to draw this according to balance bond theory, we wouldn't use these right angles here because this is going to be trigonal pointer.

01:11 So these are all going to be 120 degree angles.

01:14 It's going to fit essentially a triangle.

01:17 And that will help us answer whether or not this molecule is polar.

01:21 So we've got polar bonds here.

01:24 Oxygen and fluorine are all electronegatives.

01:27 I'm drawing these sort of at angles to indicate that they should be pointing away from each other.

01:33 And if these were all the same molecule, they would perfectly cancel each other out.

01:38 But because oxygen and forene are going to pull differently, this molecule will be polar.

01:47 They don't perfectly cancel each other out.

01:52 So next we have s2, cl2.

01:55 And this little in -script here tells us that we're going to have a corine bonded to a sulfur, bonded to a sulfur, bonded to a corin.

02:08 It's a neutral molecule.

02:10 Corine likes to have one bone.

02:11 Bond, sulfur likes to have, i forgot those long pairs, uh, sulfur likes to have two.

02:17 So everything is happy.

02:19 They all have the right number of bonds...

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