6 for each of the following identify the i geometry of...

6. For each of the following, identify the: i) geometry of electron pairs (including lone pairs) ii. Shape iii. Polarity a) CCl4 b) SeF2 c) NCl3 7. Which of the compounds in problem 6 have dipole-dipole forces?

Transcript

00:01 First of all, let's have a look what all is given in the problem.

00:04 Given is three compounds are given that is carbon tetrachloride, second one is scf2 and the last one that is given is ncl3.

00:12 These are the three compounds that are given.

00:15 What we are supposed to do is in the sixth part, we are supposed to tell about the geometry of the electron pairs.

00:22 We have to tell about the geometry.

00:24 Next, we have to tell a shape and the last one we have to tell about the polarity.

00:30 After that in the 7th part we have to tell in which of the compound dipole -dipole forces are present.

00:36 So let's try to look at the structures of these compounds.

00:41 Let's try to draw their shapes.

00:43 So we can see that if we draw ccl4 it will look like this.

00:48 So here the lone pairs will be present on chlorine because chlorine is a halogen.

00:53 It has 7 electrons in its outermost shell.

00:55 Overall the molecule is non -polar in nature due to the cancellation of dipoles.

01:00 It will be like this.

01:02 Overall dipoles will get cancelled out because chlorine is more electronegative than carbon.

01:07 So overall dipole will get cancelled out.

01:09 If we talk about the geometry and the shape of ccl4, it remains the same.

01:15 That is tetrahedral only.

01:17 Both the geometry and the shape is tetrahedral.

01:20 Overall molecular polarity is non -polar.

01:23 Next we have is sef2.

01:26 So we know that selenium belongs to oxygen family...

Question

6. For each of the following, identify the: i) geometry of electron pairs (including lone pairs) ii. Shape iii. Polarity a) CCl4 b) SeF2 c) NCl3 7. Which of the compounds in problem 6 have dipole-dipole forces?

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