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Chapter 11: Problem 105

Which of these diatomic molecules do you think has the greater bond energy, \(\mathrm{Li}_{2}\) or \(\mathrm{C}_{2} ?\) Explain.

Short Answer

Expert verified
C2 has a greater bond energy than Li2 because carbon is more electronegative and has a smaller atomic size than lithium, leading to stronger bonding.

Step by step solution

01

Understand Bond Energy

Bond energy is the amount of energy required to break one mole of a bond in a substance in gaseous state. It also represents the strength of a bond; a higher bond energy indicates a stronger bond.
02

Compare Atomic Sizes and Electronegativities

Compare the atomic sizes and the electronegativities of lithium and carbon. Carbon is smaller and more electronegative than lithium. As we go across the periodic table, atomic size decreases and electronegativity increases.
03

Understand the Effect on Bond Energy

A smaller atomic size and a higher electronegativity generally lead to a greater bond energy, since the bond is stronger due to the stronger pull on the shared electrons.
04

deduce Bond Energy

Based on the described trends, C2 with a greater electronegativity and smaller atomic size than Li2 is likely to have a stronger bond and hence a greater bond energy.

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Most popular questions from this chapter

Propose a hybridization scheme to account for bonds formed by the central carbon atom in each of the following molecules: (a) hydrogen cyanide, HCN; (b) methyl alcohol, \(\mathrm{CH}_{3} \mathrm{OH} ;\) (c) acetone, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO}\) (d) carbamic acid,

In which of the following molecules would you expect to find delocalized molecular orbitals: (a) \(\mathrm{C}_{2} \mathrm{H}_{4}\) (b) \(\mathrm{SO}_{2} ;\) (c) \(\mathrm{H}_{2} \mathrm{CO}\) ? Explain.

Match each of the following species with one of these hybridization schemes: \(s p, s p^{2}, s p^{3}, s p^{3} d, s p^{3} d^{2} .\) (a) \(\mathrm{PF}_{6}^{-}\) (b) \(\operatorname{COS} ;\) (c) \(\operatorname{SiCl}_{4} ;\) (d) \(\mathrm{NO}_{3}^{-}\);(e) AsF \(_{5}\)

Draw a Lewis structure(s) for the nitrite ion, \(\mathrm{NO}_{2}^{-}\) Then propose a bonding scheme to describe the \(\sigma\) and the bonding in this ion. What conclusion can you reach about the number and types of \(\pi\) molecular orbitals in this ion? Explain.

For the following pairs of molecular orbitals, indicate the one you expect to have the lower energy, and state the reason for your choice. (a) \(\sigma_{1 s}\) or \(\sigma_{1 s}^{*} ;\) (b) \(\sigma_{2 s}\) or \(\sigma_{2 p}\) (c) \(\sigma_{1 s}^{*}\) or \(\sigma_{2 s} ;\) (d) \(\sigma_{2 p}\) or \(\sigma_{2 p}^{*}\)
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