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Chapter 8: Problem 57

True or false: \((\mathbf{a})\) The \(\mathrm{C}-\mathrm{C}\) bonds in benzene are all the same length and correspond to typical single \(\mathrm{C}-\mathrm{C}\) bond lengths. (b) The \(\mathrm{C}-\mathrm{C}\) bond in acetylene, \(\mathrm{HCCH}\), is longer than the average \(\mathrm{C}-\mathrm{C}\) bond length in benzene.

Short Answer

Expert verified
(a) False: All C-C bonds in benzene are the same length, but they have an intermediate length between typical single and double C-C bond lengths due to resonance. (b) False: The C-C bond in acetylene is shorter, not longer, than the average C-C bond length in benzene because it is a triple bond formed by the overlap of sp-hybridized orbitals.

Step by step solution

01

Statement A: Benzene C-C bonds are all the same length and correspond to typical single C-C bond lengths

Benzene has a planar, hexagonal ring structure with alternating single and double bonds between carbon atoms. However, due to resonance, the pi electrons in these double bonds are delocalized across all six carbon atoms, resulting in a bond length that is intermediate between a typical single bond and a double bond. Therefore, it's true that all C-C bonds in benzene are the same length, but they do not correspond to typical single C-C bond lengths. As a consequence, statement A is false.
02

Statement B: The C-C bond in acetylene is longer than the average C-C bond length in benzene

Acetylene has a triple bond between its two carbon atoms, which results from the overlap of sp-hybridized orbitals. Triple bonds are shorter and stronger than single or double bonds. So, the C-C bond in acetylene is actually shorter than the average C-C bond length in benzene. Therefore, statement B is false. Both statements A and B are false.

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Most popular questions from this chapter

Although \(\mathrm{I}_{3}^{-}\) is a known ion, \(\mathrm{F}_{3}^{-}\) is not. \((\mathbf{a})\) Draw the Lewis structure for \(I_{3}^{-}\) (it is linear, not a triangle). (b) One of your classmates says that \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because it would violate the octet rule. Is this classmate possibly correct? (d) Yet another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too small to make bonds to more than one atom. Is this classmate possibly correct?

Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) the central oxygen atom in \(\mathrm{O}_{3},(\mathbf{b})\) phosphorus in \(\mathrm{PF}_{6}^{-},(\mathbf{c})\) nitrogen in \(\mathrm{NO}_{2}\), (d) iodine in ICl \(_{3}\), (e) chlorine in \(\mathrm{HClO}_{4}\) (hydrogen is bonded to \(\mathrm{O}\) ).

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3}\), (b) \(\mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6}\), (c) \(\mathrm{PbCl}_{4}\) and RbCl.

Potassium peroxide is composed of \(70.96 \% \mathrm{~K}\) and $29.04 \% \mathrm{O}\(. Each peroxide ion has a net charge of \)2^{-}$. (a) Given the molecular weight of the compound is 110.19 , determine the chemical formula of potassium peroxide. \((\mathbf{b})\) What is the number of valance electron pairs in the peroxide ion? (c) Draw the Lewis structure of the peroxide ion. (d) Compare the \(\mathrm{O}-\mathrm{O}\) bond distance in oxygen molecule and potassium peroxide.

(a) Draw the dominant Lewis structure for the phosphorus trifluoride molecule, \(\mathrm{PF}_{3}\). (b) Determine the oxidation numbers of the \(\mathrm{P}\) and \(\mathrm{F}\) atoms. \((\mathbf{c})\) Determine the formal charges of the \(\mathrm{P}\) and \(\mathrm{F}\) atoms.
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