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Chapter 11: Problem 104

Use the valence molecular orbital configuration to determine which of the following species is expected to have the greatest electron affinity: (a) \(\mathrm{C}_{2}^{+} ;\) (b) \(\mathrm{Be}_{2}\) (c) \(\mathrm{F}_{2} ;\) (d) \(\mathrm{B}_{2}^{+}\)

Short Answer

Expert verified
Out of \[\mathrm{C}_{2}^{+}\], \[\mathrm{Be}_{2}\], \[\mathrm{F}_{2}\], and \[\mathrm{B}_{2}^{+}\], \[\mathrm{C}_{2}^{+}\] has the greatest electron affinity.

Step by step solution

01

Identify the molecular orbital configuration

The first step is to know the molecular orbital configuration of each species. The molecular orbital configuration can be derived from the periodic table by identifying the total number of valence electrons for each atom in a molecule. \[\mathrm{C}_{2}^{+}\] has 7 valence electrons, \[\mathrm{Be}_{2}\] has 4 valence electrons, \[\mathrm{F}_{2}\] has 14 valence electrons and \[\mathrm{B}_{2}^{+}\] has 5 valence electrons.
02

Determine electron cloud vacancy

Next, identify which of these species have more vacancies for electrons in their valence electron cloud. \[\mathrm{C}_{2}^{+}\] and \[\mathrm{B}_{2}^{+}\] have an odd number of valence electrons, meaning they have one unpaired electron each. \[\mathrm{Be}_{2}\] has its electron cloud full and does not have space for more electrons. \[\mathrm{F}_{2}\] has paired electrons only, meaning its electron cloud is almost full with just a little space for more electrons.
03

Determine electron affinity

Species with more vacancies in their electron cloud are more likely to receive an electron. Species with an unpaired electron have larger electron affinity because the contact of an extra electron with the unpaired electron leads to a stable pairing. Therefore \[\mathrm{C}_{2}^{+}\] and \[\mathrm{B}_{2}^{+}\] have a higher electron affinity compared to \[\mathrm{Be}_{2}\] and \[\mathrm{F}_{2}\] . Among \[\mathrm{C}_{2}^{+}\] and \[\mathrm{B}_{2}^{+}\] , \[\mathrm{C}_{2}^{+}\] has a greater electron affinity because it is on the right side of the Periodic Table where elements are more likely to accept electrons.

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Most popular questions from this chapter

The paramagnetism of gaseous \(\mathrm{B}_{2}\) has been established. Explain how this observation confirms that the \(\pi_{2 p}\) orbitals are at a lower energy than the \(\sigma_{2 p}\) orbital for \(\mathrm{B}_{2}\)

In which of the following, \(\mathrm{CO}_{3}^{2-}, \mathrm{SO}_{2}, \mathrm{CCl}_{4}, \mathrm{CO}\) \(\mathrm{NO}_{2}^{-},\) would you expect to find \(s p^{2}\) hybridization of the central atom? Explain.

A conjugated hydrocarbon has an alternation of double and single bonds. Draw the molecular orbitals of the \(\pi\) system of 1,3,5 -hexatriene. If the energy required to excite an electron from the HOMO to the LUMO corresponds to a wavelength of \(256 \mathrm{nm},\) do you expect the wavelength for the corresponding excitation in 1,3,5,7 -octatetraene to be a longer or shorter wavelength?

Construct a concept map that embodies the ideas of valence bond theory.

Of the following, the species with a bond order of 1 is (a) \(\mathrm{H}_{2}^{+} ;\) (b) \(\mathrm{Li}_{2} ;\) (c) \(\mathrm{He}_{2} ;\) (d) \(\mathrm{H}_{2}^{-}\)
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