Which of the following molecules would you expect to have a...

Which of the following molecules would you expect to have a dipole moment of zero? a. $\mathrm{CH}_{3} \mathrm{CH}_{3}$ b. $\mathrm{H}_{2} \mathrm{C}=\mathrm{O}$ c. $\mathrm{CH}_{2} \mathrm{Cl}_{2}$ d. $\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}$ e. $\mathrm{H}_{2} \mathrm{C}=\mathrm{CHBr}$

Which of the following molecules would you expect to have a dipole moment of zero?
a. $\mathrm{CH}_{3} \mathrm{CH}_{3}$
b. $\mathrm{H}_{2} \mathrm{C}=\mathrm{O}$
c. $\mathrm{CH}_{2} \mathrm{Cl}_{2}$
d. $\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}$
e. $\mathrm{H}_{2} \mathrm{C}=\mathrm{CHBr}$

Key Concepts

Polar Bonds

Polar bonds occur when there is a significant difference in electronegativity between two atoms, leading to an uneven distribution of electron density. Although polar bonds are the source of individual dipole moments, the overall molecular dipole depends on how these bonds are spatially arranged in the molecule.

Molecular Symmetry

Molecular symmetry involves the balanced, often repetitive arrangement of atoms in a molecule. High symmetry in a molecule often leads to the cancellation of individual bond dipoles, resulting in a net dipole moment of zero, even when polar bonds are present.

Dipole Moment

The dipole moment is a measure of the separation between positive and negative charges in a molecule. It arises when there are polar bonds—as a result of differences in electronegativity between atoms—but its net value depends on both the magnitude and the direction of these bond dipoles, which can cancel out depending on the geometry of the molecule.

Molecular Geometry

Molecular geometry refers to the three?dimensional arrangement of atoms within a molecule. The shape determines how the individual bond dipoles are oriented in space, which affects whether they add up to produce a net dipole moment or cancel each other out.

Transcript

00:01 In this question we have been given five different molecules and out of these five molecules we need to identify the ones that have a dipole moment of zero which means that the molecule should not have any kind of divol moment so for solving this question first of all we need to understand what is actually the meaning of dipole moment right now the dipole moment is given by this symbol mu and it is going to be expressed by the expression q multiplied by r so q here is the measurement of charge or we can say the magnitude of charge or we can say the difference of charge between the two atoms or the two ends because we are talking about a dipole which means that there should be two folds one should be the positive one and other should be the negative one so q is the charge difference between these two charges and r is the distance between these two charge or we can say the charge separation so the dipole moment would be the product of the charge magnitude and the distance between these two charges so in the given molecules the molecules are first of all we have c h 3 ch3 and the second molecule we have is h2c double bond o h2c double bond o it is and the third molecule that we have is ch2 cl2 the fourth molecule we have would be h2c double bond ch2 and lastly the fifth molecule we have would be h2c double bond chbr so now in this question we can clearly say that there should be a charge difference between the two bonded atoms for dipole moment to be there.

01:33 Now in the molecules a and d, we can say that the bond is between the identical atoms, which means that in a, the bond is between carbon and carbon and the three hydrogens are attached to these carbons.

01:45 And in the molecule d, we have another bond between these two carbon atoms, which is double bond here.

01:50 And then two hydrogations are attached to each of these double bonded carbons...

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