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Chapter 10: Problem 38

Identify the most important types of interparticle forces present in the solids of each of the following substances. a. \(\mathrm{BaSO}_{4}\) b. \(\mathrm{H}_{2} \mathrm{S}\) c. \(\mathrm{Xe}\) d. \(\mathrm{C}_{2} \mathrm{H}_{6}\) e. \(\mathrm{CsI}\) f. \(P_{4}\) g. \(\mathrm{NH}_{3}\)

Short Answer

Expert verified
a. BaSO4: Ionic Bonds b. H2S: Dipole-Dipole Interactions and London Dispersion Forces c. Xe: London Dispersion Forces d. C2H6: London Dispersion Forces e. CsI: Ionic Bonds f. P4: Covalent Bonds and London Dispersion Forces g. NH3: Hydrogen Bonds, Dipole-Dipole Interactions, and London Dispersion Forces

Step by step solution

01

a. BaSO4: Ionic Bonds

Barium sulfate (BaSO4) is an ionic compound composed of a metal (Barium) and a polyatomic ion (sulfate). In the solid state, the particles are held together by the strong electrostatic attraction between the positive and negative ions (Barium and sulfate), forming an ionic crystal lattice. Thus, the most important type of interparticle force present in this solid is the ionic bond.
02

b. H2S: Dipole-Dipole Interactions and London Dispersion Forces

Hydrogen sulfide (H2S) is a polar covalent molecule. The electrostatic attraction between the oppositely charged ends of adjacent polar molecules results in dipole-dipole interactions, which significantly contribute to holding the molecules together in the solid state. Additionally, as a nonpolar molecule, H2S also exhibits London dispersion forces (temporary induced dipoles), although these forces are relatively weaker compared to dipole-dipole interactions in this case.
03

c. Xe: London Dispersion Forces

Xenon (Xe) is a noble gas and therefore exists as independent atoms in the solid state. It exhibits only London dispersion forces, which are temporary induced dipoles arising from the fluctuations of electron distribution in atoms. These weak van der Waals forces are responsible for holding the xenon atoms together in the solid state.
04

d. C2H6: London Dispersion Forces

Ethane (C2H6) is a nonpolar covalent molecule. Due to its nonpolarity, the primary interparticle forces are London dispersion forces, which are temporary induced dipoles resulting from the fluctuation of electron distribution around the atoms.
05

e. CsI: Ionic Bonds

Cesium iodide (CsI) is an ionic compound composed of a metal (Cesium) and a nonmetal (Iodine). In the solid state, they form an ionic crystal lattice, where the particles are held together by the strong electrostatic attraction between the positively charged cesium ions and the negatively charged iodide ions. Consequently, the most important interparticle force in this compound is the ionic bond.
06

f. P4: Covalent Bonds and London Dispersion Forces

Phosphorus (P4) is a nonmetal that forms a tetrahedral molecular structure, with covalent bonds between the phosphorus atoms. These covalent bonds hold the atoms together within the molecule. Additionally, as a nonpolar molecule, P4 also exhibits London dispersion forces (temporary induced dipoles) between the P4 molecules in the solid state.
07

g. NH3: Hydrogen Bonds, Dipole-Dipole Interactions, and London Dispersion Forces

Ammonia (NH3) is a polar covalent molecule consisting of nitrogen and hydrogen atoms. The primary interparticle force responsible for holding ammonia molecules together in the solid state is the hydrogen bond, which is a particularly strong dipole-dipole interaction between an electronegative atom (nitrogen in this case) and a hydrogen atom bonded to another highly electronegative atom. Additionally, there are other weaker forces such as general dipole-dipole interactions and London dispersion forces between the molecules.

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Most popular questions from this chapter

Argon has a cubic closest packed structure as a solid. Assuming that argon has a radius of 190. pm, calculate the density of solid argon

Some water is placed in a sealed glass container connected to a vacuum pump (a device used to pump gases from a container), and the pump is turned on. The water appears to boil and then freezes. Explain these changes using the phase diagram for water. What would happen to the ice if the vacuum pump was left on indefinitely?

Describe what is meant by a dynamic equilibrium in terms of the vapor pressure of a liquid.

A 20.0 -g sample of ice at \(-10.0^{\circ} \mathrm{C}\) is mixed with 100.0 g water at \(80.0^{\circ} \mathrm{C}\) . Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of \(\mathrm{H}_{2} \mathrm{O}(s)\) and \(\mathrm{H}_{2} \mathrm{O}(l)\) are 2.03 and \(4.18 \mathrm{J} / \mathrm{g} \cdot^{\circ} \mathrm{C},\) respectively, and the enthalpy of fusion for ice is 6.02 \(\mathrm{kJ} / \mathrm{mol} .\)

Carbon diselenide (CSe_ \(_{2} )\) is a liquid at room temperature. The normal boiling point is \(125^{\circ} \mathrm{C},\) and the melting point is \(-45.5^{\circ} \mathrm{C}\) . Carbon disulfide \(\left(\mathrm{CS}_{2}\right)\) is also a liquid at room temperature with normal boiling and melting points of \(46.5^{\circ} \mathrm{C}\) and \(-111.6^{\circ} \mathrm{C},\) respectively. How do the strengths of the intermolecular forces vary from \(\mathrm{CO}_{2}\) to \(\mathrm{CS}_{2}\) to \(\mathrm{CSe}_{2} ?\) Explain.
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