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Chapter 8: Q23 E (page 449)

The bond energy of a C–C single bond averages \({\rm{347 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\); that of a

C ≡ C triple bond averages \({\rm{839 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). Explain why the triple bond is not three times as strong as a single bond.

Short Answer

Expert verified

A triple bond has an \({\rm{\sigma }}\) bond and two \({\rm{\pi }}\) bonds, whereas a single bond has only an \({\rm{\sigma }}\) bond. Because sigma bonds are far stronger than \({\rm{\pi }}\) bonds, a triple bond including one \({\rm{\sigma }}\) and two \({\rm{\pi }}\) bonds are not three times as strong as a single bond.

Step by step solution

01

Define bond energy

The amount of energy required to break apart a mole of molecules into its component atoms is known as bond energy (E). It's a metric for how strong a chemical bond is.

02

Explanation

The triple bond has an \({\rm{\sigma }}\) bond and two \({\rm{\pi }}\) bonds rather of three sigma bonds, whereas a single bond only has an \({\rm{\sigma }}\) bond. The triple bond, which consists of an \({\rm{\sigma }}\)bond and two \({\rm{\pi }}\) bonds, is not three times as strong as a single bond because sigma bonds are much stronger than \({\rm{\pi }}\) bonds.

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Most popular questions from this chapter

For each of the following structures, determine the hybridization requested and whether the electrons will be delocalized:

(a)Hybridization of each carbon

(b)Hybridization of sulphur


(c)

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For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains \({\rm{77}}{\rm{.55\% }}\)Xe and \({\rm{22}}{\rm{.45\% \;F}}\)by mass.

(a) What is the formula of the compound?

(b) Write a Lewis structure for the compound.

(c) Predict the shape of the molecules of the compound.

(d) What hybridization is consistent with the shape you predicted?

Sketch the distribution of electron density in the bonding and antibonding molecular orbitals formed from two S orbitals and from two P orbitals.

Draw a curve that describes the energy of a system with H and CI atoms at varying distances. Then, find the minimum energy of this curve two ways.

(a) Use the bond energy found in Table 8.1 to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?)

(b) Use the enthalpy of reaction and the bond energies for \({{\rm{H}}_{\rm{2}}}\)and \({\rm{C}}{{\rm{l}}_{\rm{2}}}\)to solve for the energy of one mole of \({\rm{HCl}}\)bonds.

\({{\text{H}}_{\text{2}}}{\text{(g) + C}}{{\text{l}}_{\text{2}}}{\text{(g)}} \rightleftharpoons {\text{2HCl(g)}}\) ΔH°rxn = −184.7 kJ/mol

For the first ionization energy for an \({{\rm{N}}_2}\) molecule, what molecular orbital is the electron removed from?
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