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Chapter 8: Problem 24

Which of the following statements is(are) true? Correct the false statements. a. It is impossible to satisfy the octet rule for all atoms in \(\mathrm{XeF}_{2}\). b. Because \(\mathrm{SF}_{4}\) exists, \(\mathrm{OF}_{4}\) should also exist because oxygen is in the same family as sulfur. c. The bond in \(\mathrm{NO}^{+}\) should be stronger than the bond in \(\mathrm{NO}^{-}\). d. As predicted from the two Lewis structures for ozone, one oxygen-oxygen bond is stronger than the other oxygenoxygen bond.

Short Answer

Expert verified
Statement a: False. Corrected statement: "It is possible to satisfy the octet rule for all atoms in XeF2 due to xenon's ability to form an expanded octet." Statement b: False. Corrected statement: "Although SF4 exists, OF4 does not exist because oxygen cannot exceed the octet rule like sulfur." Statement c: True. Statement d: False. Corrected statement: "As predicted from the two Lewis structures for ozone, both oxygen-oxygen bonds are equivalent and have equal bond strengths."

Step by step solution

01

Statement a: Octet rule in XeF2

XeF2 is an exception to the octet rule as xenon can exceed the octet rule by utilizing its empty d orbitals. In XeF2, xenon has 3 lone pairs and 2 fluorine atoms attached, which means it follows an expanded octet. So, the statement is false. The corrected version would be: "It is possible to satisfy the octet rule for all atoms in XeF2 due to xenon's ability to form an expanded octet."
02

Statement b: Existence of OF4

Although oxygen and sulfur are in the same group, they don't always exhibit similar properties. In this case, while SF4 exists, OF4 does not exist. This is because sulfur can exceed the octet rule due to its ability to use empty d orbitals, while oxygen can't. So, the statement is false. The corrected version would be: "Although SF4 exists, OF4 does not exist because oxygen cannot exceed the octet rule like sulfur."
03

Statement c: Comparing bond strengths in NO+ and NO-

In NO+, there is a double bond between nitrogen and oxygen, whereas in NO-, there is a single bond between nitrogen and oxygen (due to an additional electron). Double bonds are stronger than single bonds, so the bond in NO+ should be stronger than the bond in NO-. Therefore, the statement is true.
04

Statement d: Oxygen-oxygen bonds in ozone

In ozone (O3), two equivalent resonance structures can be drawn, one with a double bond between the central oxygen and each of the side oxygens. The true structure of ozone is an average of these two resonance structures, meaning that both oxygen-oxygen bonds are equivalent and have equal bond strengths. The statement is false. The corrected version would be: "As predicted from the two Lewis structures for ozone, both oxygen-oxygen bonds are equivalent and have equal bond strengths."

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Most popular questions from this chapter

Use the following data to estimate \(\Delta H\) for the reaction \(\mathrm{S}^{-}(g)+\) \(\mathrm{e}^{-} \rightarrow \mathrm{S}^{2-}(g)\). Include an estimate of uncertainty. $$ \begin{array}{|lcccc|} \hline & & \text { Lattice } & & \Delta H_{\text {sub }} \\ & \Delta \boldsymbol{H}_{\mathrm{t}}^{\circ} & \text { Energy } & \text { I.E. of } \mathbf{M} & \text { of M } \\ \hline \mathrm{Na}_{2} \mathrm{~S} & -365 & -2203 & 495 & 109 \\ \mathrm{~K}_{2} \mathrm{~S} & -381 & -2052 & 419 & 90 \\ \mathrm{Rb}_{2} \mathrm{~S} & -361 & -1949 & 409 & 82 \\ \mathrm{Cs}_{2} \mathrm{~S} & -360 & -1850 & 382 & 78 \\ \hline \end{array} $$ $$ \begin{aligned} \mathrm{S}(s) & \longrightarrow \mathrm{S}(g) & \Delta H &=227 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{S}(g)+\mathrm{e}^{-} & \longrightarrow \mathrm{S}^{-}(g) & \Delta H &=-200 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ Assume that all values are known to \(\pm 1 \mathrm{~kJ} / \mathrm{mol}\).

Which compound in each of the following pairs of ionic substances has the most exothermic lattice energy? Justify your answers. a. \(\mathrm{NaCl}, \mathrm{KCl}\) b. \(\mathrm{LiF}, \mathrm{LiCl}\) c. \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgO}\) d. \(\mathrm{Fe}(\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}\) e. \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{O}\) f. \(\mathrm{MgO}, \mathrm{BaS}\)

Compare the electron affinity of fluorine to the ionization energy of sodium. Is the process of an electron being "pulled" from the sodium atom to the fluorine atom exothermic or endothermic? Why is NaF a stable compound? Is the overall formation of NaF endothermic or exothermic? How can this be?

Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form between the following pairs of elements. a. \(\mathrm{Rb}\) and \(\mathrm{Cl}\) d. \(\mathrm{Ba}\) and \(\mathrm{S}\) b. \(S\) and \(S\) e. \(\mathrm{N}\) and \(\mathrm{P}\) c. \(C\) and \(\bar{F}\) f. \(\mathrm{B}\) and \(\mathrm{H}\)

Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those that are incorrect. a. \(^{8+} \mathrm{H}-\mathrm{F}^{\delta-}\) d. \(^{\delta}+\mathrm{Br}-\mathrm{Br}^{8}\) b. \(^{\delta+} \mathrm{Cl}-\mathrm{I}^{8}-\) e. \(^{\delta+} \mathrm{O}-\mathrm{P}^{\delta-}\) c. \(^{\delta+} \mathrm{Si}-\mathrm{S}^{8-}\)
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