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Chapter 22: Problem 37

Use Lewis structures and other information to explain the observation that (a) \(\mathrm{H}_{2} \mathrm{S}\) is a gas at room temperature, whereas \(\mathrm{H}_{2} \mathrm{O}\) is a liquid. (b) \(\mathrm{O}_{3}\) is diamagnetic.

Short Answer

Expert verified
H2S is a gas at room temperature, and H2O is a liquid due to the differing strength of their intermolecular forces. H2O has strong hydrogen bonding, whereas H2S has weaker dipole-dipole interactions. O3 is diamagnetic because all its electrons are paired in its molecular orbitals, giving it no net magnetic moment.

Step by step solution

01

Drawing Lewis Structures

First, we draw the Lewis structures of the molecules in question. Lewis structures, also known as Lewis-dot diagrams, show the bonding relationship between atoms of a molecule. They also highlight the lone pairs of electrons. The Lewis structure for H2S is H-S-H with two lone pairs of electrons around S. The Lewis structure for H2O is H-O-H with two lone pairs of electrons around O. The Lewis structure for O3 shows a resonance structure with one of the double bonds shifting among the three oxygen atoms.
02

Compare Intermolecular Forces in H2S and H2O

Intermolecular forces are responsible for the physical states of the molecules. In H2O, due to the presence of two hydrogen bonds between the molecules, there is a stronger intermolecular force. This high intermolecular force causes H2O to be in the liquid state at room temperature. In H2S, the intermolecular force comes only from dipole-dipole interactions and dispersion forces, which are considerably weaker than hydrogen bonds. This causes H2S to be in the gas state at room temperature.
03

Analyze O3's Magnetic Properties

A molecule is diamagnetic when all the electrons are paired. In this case, the O3 molecule has all the electrons paired in its molecular orbitals. This means that it doesn't have unpaired electrons to create a net magnetic moment. Therefore, O3 is diamagnetic, which means it doesn't get attracted into a magnetic field.

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Most popular questions from this chapter

All of the following compounds yield \(\mathrm{O}_{2}(\mathrm{g})\) when heated to about \(1000 \mathrm{K}\) except (a) \(\mathrm{KClO}_{3} ;\) (b) \(\mathrm{KClO}_{4}\) (c) \(\mathrm{N}_{2} \mathrm{O} ;\) (d) \(\mathrm{CaCO}_{3} ;\) (e) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\).

Various thermochemical cycles are being explored as possible sources of \(\mathrm{H}_{2}(\mathrm{g}) .\) The object is to find a series of reactions that can be conducted at moderate temperatures (about \(500^{\circ} \mathrm{C}\) ) and that results in the decomposition of water into \(\mathrm{H}_{2}\) and \(\mathrm{O}_{2} .\) Show that the following series of reactions meets these requirements. $$\begin{aligned}\mathrm{FeCl}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Fe}_{3} \mathrm{O}_{4}+\mathrm{HCl}+\mathrm{H}_{2} \\\\\mathrm{Fe}_{3} \mathrm{O}_{4}+\mathrm{HCl}+\mathrm{Cl}_{2} & \longrightarrow \mathrm{FeCl}_{3}+\mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2} \\\\\mathrm{FeCl}_{3} \longrightarrow & \mathrm{FeCl}_{2}+\mathrm{Cl}_{2}\end{aligned}$$

Write a plausible chemical equation to represent the reaction of \((\mathrm{a}) \mathrm{Cl}_{2}(\mathrm{g}) \quad\) with cold \(\quad \mathrm{NaOH}(\mathrm{aq})\) (b) \(\mathrm{NaI}(\mathrm{s})\) with hot \(\mathrm{H}_{2} \mathrm{SO}_{4}(\text { concd aq }) ;\) (c) \(\mathrm{Cl}_{2}(\mathrm{g})\) with \(\mathrm{KI}_{3}(\mathrm{aq}) ; \quad\) (d) \(\quad \mathrm{NaBr}(\mathrm{s}) \quad\) with hot \(\mathrm{H}_{3} \mathrm{PO}_{4}\) \((\text { concd aq })\) (e) \(\mathrm{NaHSO}_{3}(\mathrm{aq})\) with \(\mathrm{MnO}_{4}^{-1}(\mathrm{aq})\) in dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\).

Make a general prediction about which of the halogen elements, \(\mathrm{F}_{2}, \mathrm{Cl}_{2}, \mathrm{Br}_{2},\) or \(\mathrm{I}_{2},\) displaces other halogens from a solution of halide ions. Which of the halogens is able to displace \(\mathrm{O}_{2}(\mathrm{g})\) from water? Which is able to displace \(\mathrm{H}_{2}(\mathrm{g})\) from water?

\(\mathrm{O}_{3}(\mathrm{g})\) is a powerful oxidizing agent. Write equations to represent oxidation of \((a) I^{-}\) to \(I_{2}\) in acidic solution; (b) sulfur in the presence of moisture to sulfuric acid; (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) to \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) in basic solution. In each case \(\mathrm{O}_{3}(\mathrm{g})\) is reduced to \(\mathrm{O}_{2}(\mathrm{g})\).
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