Use the electronegativity table given in Figure 2

Key Concepts

Dipole Moment

The dipole moment is a measure of the separation of positive and negative charges in a bond. It not only provides information on the magnitude of polarity but also indicates the direction in which the electron density is shifted, pointing from the positive end to the negative end of the bond.

Electronegativity

Electronegativity is a measure of an atom's tendency to attract electrons towards itself when it forms a chemical bond. Understanding electronegativity is crucial in predicting how electrons will be distributed between two bonded atoms, and it forms the basis for determining bond polarity in molecules.

Electronegativity Difference

The electronegativity difference between two bonded atoms is the key factor that influences the degree of electron sharing or transfer. A larger difference typically results in a more polar bond or even an ionic bond if the difference is significant enough, while a small or zero difference leads to nonpolar covalent bonds.

Bond Polarity

Bond polarity refers to the distribution of electrical charge over the atoms in a bond. When there is an unequal sharing of electrons due to differences in electronegativity, one end of the bond becomes partially negative and the other partially positive, creating a dipole moment along the bond.

Transcript

00:01 Hi, so for this problem, we are going to use the electro -negativity table given in figure 2 in your text book to predict which bind is more polar and indicate the direction of polarity for each compound.

00:21 Okay, so the way this works is, well, we just got to evaluate which.

00:30 Has a greater difference in electro -negativity to determine which one is more polar as opposed to the one that is less polar.

00:43 Or in a case of molecules where the two species, the two atoms are the same, such as molecular chlorine and molecular oxygen.

00:54 We have non -polar molecules and also places where, i'm sorry, compounds where, or dipose can, so that's also considered non -polar.

01:11 Okay, so i'm going to use a completely different electro -negativity table because i don't really have access to your book at a moment.

01:26 So on one side of the bot, we have a carbon which forms a bond with chlorine.

01:44 Well, which one is more electrolytrogative? the chlorine is more electrolytrov negative because if you look at a table, it has a value of 3 .18.

01:56 And we start our arrow from the site where it is less electrical negative.

02:07 So less electronegative.

02:10 That's how i symbolize elitrown negativity.

02:13 Pointing towards the side where there is the side which is more electronegative.

02:20 Here we have chlorine, two chlorines that are forming a point and making a molecule.

02:27 And as a result, this is non -polar.

02:29 So you automatically know that a bond between the methyl group, i'm sorry, and the chlorine.

02:38 Are actually more polar.

02:45 However, you can also go ahead and calculate that electronegativity difference.

02:53 And the difference in electrical negativity between chlorine and carbon is basically 3 .18, which is the electronegativity for chlorine minus 2 .55.

03:11 And here you can go ahead and get a calculator and calculate an electronegativity difference.

03:24 0 .63.

03:26 So this is a little bit more polar.

03:31 I guess you can go ahead and say that this is partial, the carbon is a partial positive, and the chlorine is a partial negative.

03:42 Yeah, and that's all you can see for this.

03:45 For part of this problem.

03:48 Also, you can go ahead and calculate the difference of electronic negativity between the chlorine.

03:53 So you have 3 .18 minus 3 .18.

03:57 So hopefully you understand now why this is less polar or i might say non -polar compared to this molecule, for example.

04:11 Right.

04:12 So now for part b, we're going to have the very same problem, really.

04:20 Let's see.

04:25 Yeah, you have methane bonded to a hydrogen or a hydrogen bonded to chlorine.

04:37 Now, again, you're going to use the table the electro -negativity of the elements table in your textbook in determining which wine is more electric -negative.

04:48 The one that is more electrolytrov negative, obviously, is the carbon.

04:55 And in this case, it's the chlorine.

04:57 Now, which one is more electrolytrov negative? well, we have 3 .18.

05:06 That's the chlorine minus 2 .55.

05:10 I think it's similar to what we did earlier...

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