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Chapter 10: Problem 4

Is it possible for the dispersion forces in a particular substance to be stronger than the hydrogen bonding forces in another substance? Explain your answer

Short Answer

Expert verified
Yes, it is possible for the dispersion forces in a particular substance to be stronger than the hydrogen bonding forces in another substance. This can occur when the substance with dispersion forces has a large number of electrons, larger size, and an elongated shape, and the substance with hydrogen bonding forces has relatively smaller molecules and weaker hydrogen bonds. However, the overall strength of all intermolecular forces, including dipole-dipole interactions and ion-dipole interactions, should be considered when comparing the interactions between substances.

Step by step solution

01

Understanding Dispersion Forces and Hydrogen Bonding Forces

Dispersion forces, also called London dispersion forces or van der Waals forces, are weak intermolecular forces that arise due to temporary fluctuations in electron distribution around molecules. They are present in all substances including nonpolar and polar molecules. On the other hand, hydrogen bonding forces are a type of strong intermolecular force that occurs between a hydrogen atom and a highly electronegative atom like oxygen, nitrogen, or fluorine. These forces are generally stronger than dispersion forces but are only present in polar molecules containing H-O, H-N, or H-F bonds.
02

Comparing Dispersion and Hydrogen Bonding Forces

In general, hydrogen bonding forces are stronger than dispersion forces. However, this does not mean that dispersion forces in a particular substance cannot be stronger than hydrogen bonding forces in another substance. Dispersion forces depend on several factors, including the size and shape of the molecules and the number of electrons in the molecules. As the size and number of electrons in the molecules increase, the dispersion forces become stronger.
03

Conditions for Strong Dispersion Forces

It is possible for the dispersion forces in a particular substance to be stronger than the hydrogen bonding forces in another substance, under certain conditions. For this to happen, the molecules of the substance with dispersion forces should have a large number of electrons, larger size, and an elongated shape. On the other hand, the substance with hydrogen bonding forces should have relatively smaller molecules and weaker hydrogen bonds.
04

Conclusion

In conclusion, under specific circumstances, the dispersion forces in a particular substance can be stronger than the hydrogen bonding forces in another substance. This is due to the dependence of dispersion forces on factors like molecular size, shape, and the number of electrons in the molecules. However, it is essential to consider the overall strength of all intermolecular forces, including dipole-dipole interactions and ion-dipole interactions, when comparing the interactions between substances.

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Most popular questions from this chapter

Compare and contrast the structures of the following solids. a. \(\mathrm{CO}_{2}(s)\) versus \(\mathrm{H}_{2} \mathrm{O}(s)\) b. \(\mathrm{NaCl}(s)\) versus \(\mathrm{CsCl}(s)\) ; see Exercise 71 for the structures.

What type of solid (network, metallic, Group 8A, ionic, or molecular) will each of the following substances form? a. \(\mathrm{Kr}\) b. \(\mathrm{SO}_{2}\) c. \(\mathrm{Ni}\) d. \(\mathrm{SiO}_{2}\) e. \(\mathrm{NH}_{3}\) f. \(\mathrm{Pt}\)

The radius of tungsten is 137 \(\mathrm{pm}\) and the density is 19.3 \(\mathrm{g} / \mathrm{cm}^{3}\) . Does elemental tungsten have a face-centered cubic structure or a body- centered cubic structure?

Consider the data for substance \(X\) given in Exercise 117 . When the temperature of 1.000 mole of \(X(g)\) is lowered from \(100.0^{\circ} \mathrm{C}\) to form \(\mathrm{X}(l)\) at \(50.0^{\circ} \mathrm{C}, 28.75 \mathrm{kJ}\) of heat is released. Calculate the specific heat capacity of \(\mathrm{X}(g)\)

Rubidium chloride has the sodium chloride structure at normal pressures but assumes the cesium chloride structure at high pressures. (See Exercise $71 . )$ What ratio of densities is expected for these two forms? Does this change in structure make sense on the basis of simple models? The ionic radius is 148 \(\mathrm{pm}\) for \(\mathrm{Rb}^{+}\) and 181 \(\mathrm{pm}\) for \(\mathrm{Cl}^{-} .\)
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