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Chapter 9: Problem 36

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. Xe d. \(C_{2} H_{6}\) $$\begin{array}{l} \text { e. } \mathrm{CsI} \\ \text { f. } \mathrm{P}_{4} \\ \text { g. } \mathrm{NH}_{3} \end{array}$$

Short Answer

Expert verified
a. Ionic bonds (Ba²⁺ and SO₄²⁻) b. Dipole-dipole interactions (H2S) c. London dispersion forces (Xe) d. London dispersion forces (C2H6) e. Ionic bonds (Cs⁺ and I⁻) f. Van der Waals forces (P4) g. Hydrogen bonds (NH3)

Step by step solution

01

a. BaSO4

BaSO4 is an ionic compound, composed of the ions Ba²⁺ and SO₄²⁻. The strongest interparticle force in this solid is the ionic bond between these ions.
02

b. H2S

H2S is a polar covalent molecule with hydrogen atoms covalently bonded to a sulfur atom. In its solid state, the most important interparticle force is the dipole-dipole interaction between the polar H2S molecules.
03

c. Xe

Xe is a noble gas, and its atoms interact through weak London dispersion forces (Van der Waals forces) in the solid state. These forces arise from temporary fluctuations in the electron distribution.
04

d. C2H6

C2H6 is a nonpolar covalent molecule known as ethane. In its solid state, the most important interparticle force is the London dispersion force due to temporary fluctuations in electron distribution.
05

e. CsI

CsI is an ionic compound composed of the ions Cs⁺ and I⁻. The strongest interparticle force in this solid is the ionic bond between these ions.
06

f. P4

P4 is a molecular solid, with covalent bonds between phosphorus atoms forming P4 molecules. In its solid state, the most important interparticle force is the Van der Waals force, as there are no hydrogen or dipole-dipole interactions present in the structure.
07

g. NH3

NH3, also known as ammonia, is a polar covalent molecule with nitrogen and hydrogen atoms covalently bonded. In its solid state, the most important interparticle force is the hydrogen bond between the nitrogen atom of one molecule and the hydrogen atom of another molecule.

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Most popular questions from this chapter

You have three covalent compounds with three very different boiling points. All of the compounds have similar molar mass and relative shape. Explain how these three compounds could have very different boiling points.

Iodine, like most substances, exhibits only three phases: solid, liquid, and vapor. The triple point of iodine is at 90 torr and \(115^{\circ} \mathrm{C} .\) Which of the following statements concerning liquid \(\mathrm{I}_{2}\) must be true? Explain your answer. a. \(\mathrm{I}_{2}(l)\) is more dense than \(\mathrm{I}_{2}(g).\) b. \(\mathrm{I}_{2}(l)\) cannot exist above \(115^{\circ} \mathrm{C}.\) c. \(\mathrm{I}_{2}(l)\) cannot exist at 1 atmosphere pressure. d. \(\mathrm{I}_{2}(l)\) cannot have a vapor pressure greater than 90 torr. e. \(\mathrm{I}_{2}(l)\) cannot exist at a pressure of 10 torr.

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