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Chapter 6: Problem 43

Are dipole-dipole forces between molecules as strong as the forces between oppositely charged ions? Explain.

Short Answer

Expert verified
Dipole-dipole forces between molecules are not as strong as the forces between oppositely charged ions. This is because dipole-dipole forces arise from partial charges due to differences in electronegativity, while ionic forces involve full charges resulting from electron transfer, leading to stronger attractive forces in ionic bonds.

Step by step solution

01

Understanding Dipole-Dipole Forces

Dipole-dipole forces are intermolecular forces that occur between polar molecules. A polar molecule has a positive and a negative end due to the uneven distribution of electrons within the molecule. These positive and negative ends of molecules interact with the opposite charges on neighboring molecules.
02

Understanding Ionic Forces

Ionic forces are the forces of attraction between oppositely charged ions. These forces occur when a metal atom transfers one or more electrons to a non-metal atom, creating positive and negative ions. The oppositely charged ions attract each other, forming an ionic bond.
03

Comparing Dipole-Dipole Forces and Ionic Forces

While both dipole-dipole forces and ionic forces involve interactions between opposite charges, the forces involved have different strengths. In ionic forces, the attractive force is stronger due to the full transfer of electrons between atoms, resulting in complete positive and negative charges. On the other hand, dipole-dipole forces arise from slight differences in electronegativity between atoms within the molecule. This leads to a partial positive and partial negative charge on different ends of the molecule. As a result, the attraction between these partial charges is weaker than the attraction between full charges in ionic forces.
04

Concluding

In conclusion, dipole-dipole forces between molecules are not as strong as the forces between oppositely charged ions. This is because the charges involved in dipole-dipole forces are partial, while ionic forces involve full charges, leading to a stronger attractive force in ionic bonds.

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Most popular questions from this chapter

Consider the molecules \(\mathrm{HCl}\) and \(\mathrm{HBr}\). (a) Which molecule has the larger bond dipole moment? Explain why. (b) Which molecule is more polar? Explain why.

Consider the molecule \(\mathrm{SO}_{3}\). (a) Draw the dot diagram. (b) Draw the molecule's three-dimensional shape, and label the numeric value of all bond angles. (c) What is the shape of this molecule? (d) Draw in the individual bond dipole moments. (e) Is the molecule polar? If yes, draw the molecular dipole moment vector.

Why do we use an arrow to represent a bond dipole moment? Why not just use a number?

Two molecules may both be correctly described as bent, even though one has a bond angle of approximately \(118^{\circ}\) and the other has a bond angle of approximately \(105^{\circ} .\) How is this possible?

Consider the \(\mathrm{CH}_{3}\) anion. (a) Draw and name its three-dimensional shape and indicate the predicted values of its bond angles. (b) Explain how the structure of this anion would compare with that of \(\mathrm{NH}_{3}\) and why both would have bond angles that are less than ideal.
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