Use the electronegativity table given in Figure 2.2 on page...

Use the electronegativity table given in Figure 2.2 on page 35 to predict which bond in each of the following pairs is more polar, and indicate the direction of bond polarity for each compound. (a) $\mathrm{H}_{3} \mathrm{C}-\mathrm{Cl}$ or $\mathrm{Cl}-\mathrm{Cl}$ (b) $\mathrm{H}_{3} \mathrm{C}-\mathrm{H}$ or $\mathrm{H}-\mathrm{Cl}$ (c) $\mathrm{HO}-\mathrm{CH}_{3}$ or $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{Si}-\mathrm{CH}_{3}$ (d) $\mathrm{H}_{3} \mathrm{C}$ -Li or Li-OH

Use the electronegativity table given in Figure 2.2 on page 35 to predict which bond in each of the following pairs is more polar, and indicate the direction of bond polarity for each compound.
(a) $\mathrm{H}_{3} \mathrm{C}-\mathrm{Cl}$ or $\mathrm{Cl}-\mathrm{Cl}$
(b) $\mathrm{H}_{3} \mathrm{C}-\mathrm{H}$ or $\mathrm{H}-\mathrm{Cl}$
(c) $\mathrm{HO}-\mathrm{CH}_{3}$ or $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{Si}-\mathrm{CH}_{3}$
(d) $\mathrm{H}_{3} \mathrm{C}$ -Li or Li-OH

Key Concepts

Electronegativity

Electronegativity is a measure of an atom’s ability to attract and hold electrons when it forms a chemical bond. This property helps explain the uneven distribution of electron density in bonds, which in turn influences chemical reactivity and physical properties.

Bond Polarity

Bond polarity arises when two bonded atoms have a difference in electronegativity. The more electronegative atom pulls the shared electrons closer to itself, creating a partial negative charge on one side of the bond and a corresponding partial positive charge on the other, leading to a dipole moment.

Dipole Moment and Direction

The dipole moment is a vector quantity that indicates both the magnitude and direction of the separation of electrical charge in a bond. It points from the region of partial positive charge to the region of partial negative charge, serving as a key indicator of how polar a bond is.

Transcript

00:01 They want us to use the electronegativity table on page 35 to predict which of the bond's pairs are going to be more polar, and then we also want to indicate the direction of the polarity for each bond for those compounds that i have on the board here.

00:17 So let's go ahead and just start with a, and then we can work our way down.

00:22 So we're going to first be comparing carbon to chlorine.

00:26 So normally whenever you have a halide and another atom, normally the halide is going to be more electronegative, but let's just double check.

00:35 So here we have carbon, and then there we have chlorine.

00:41 So the difference between those, or first the chlorine is going to be more electronegative.

00:47 So that means it's going to be positive here, going towards the chlorine, or i should say delta positive.

00:55 And the difference between those will we do 3 minus 2 .5, so that's going to be 0 .5.

01:02 Now what about for our chlorines? well, if we have two atoms bonded together, this is just going to be non -polar.

01:13 So that's just non -polar.

01:15 So we can't really say what direction it is.

01:18 Because if we were to come over here and subtract, we'd have 3 minus 3, which is going to be 0.

01:23 So this methyl or chloromethyl right here is going to be the.

01:36 More polar of the box now over here we have methyl versus hydrochloric acid well if we were to come over here and check so the carbon is 2 .5 the hydrogen is 2 so that means carbon is more electronegative so the hydrogen is going to have the plus and then we're gonna go out to the left towards the carbon like that and the difference between those is going to be 0 .4 now what about for hydrochloric acid? so we already know the hydrogen is 2 .1.

02:12 The chlorine is 3.

02:14 So that means, again, the hydrogen is going to have the plus, and it's going to go towards the chlorine...

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