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Chapter 9: Problem 75

Using an MO energy-level diagram, would you expect \(\mathrm{F}_{2}\) to have a lower or higher first ionization energy than atomic fluorine? Why?

Short Answer

Expert verified
Using the MO energy-level diagram, F2 would have a lower first ionization energy than atomic fluorine. This is because F2's highest occupied molecular orbital (HOMO) is the π*2p orbital, which has a higher energy than fluorine's 2p orbital. Consequently, it takes less energy to remove an electron from F2.

Step by step solution

01

Recall the Molecular Orbital (MO) theory

The Molecular Orbital theory helps us understand the bonding, anti-bonding, and non-bonding energies in a molecule. In an MO energy-level diagram, the x-axis represents the energy level of the orbitals, and the y-axis represents the positions of the atomic nuclei.
02

Draw the MO energy-level diagram for F2

Consider the electron configurations of fluorine atoms: Fluorine (F): 1s² 2s² 2p⁵ Since there are two fluorine atoms in F2, the total number of electrons is 14. The energy order for molecular orbitals in the second period of the periodic table is: σ1s < σ*1s < σ2s < σ*2s < π2p < π*2p < σ2p < σ*2p Start filling the molecular orbitals based on the energy levels, and follow the Pauli Exclusion Principle and Hund's rule: F2 MO electron configuration: (σ1s)² (σ*1s)² (σ2s)² (σ*2s)² (π2p)⁴ (π*2p)²
03

Compare the ionization energies

To determine whether F2 has a lower or higher first ionization energy than atomic fluorine, consider the valence electrons in each species: - F2: The highest occupied molecular orbital is π*2p and this is the orbital where electrons would be removed from F2. - Atomic fluorine: The electron configuration of atomic fluorine is 1s² 2s² 2p⁵, so an electron will be removed from the 2p orbital. Now, let's compare the energies: - π*2p in F2: In F2, π*2p is an anti-bonding orbital with higher energy than the bonding π2p orbital. - 2p in atomic Fluorine: In atomic fluorine, the 2p orbital is a valence shell electron with intermediate energy.
04

Conclusion

Since the HOMO (highest occupied molecular orbital) of F2 is the π*2p orbital that has higher energy than fluorine's 2p orbital, it will require less energy to remove an electron from F2. Therefore, F2 has a lower first ionization energy than atomic fluorine.

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Most popular questions from this chapter

What type of molecular orbital would result from the in-phase combination of two \(d_{x z}\) atomic orbitals shown below? Assume the \(x\) -axis is the internuclear axis.

As the head engineer of your starship in charge of the warp drive, you notice that the supply of dilithium is critically low. While searching for a replacement fuel, you discover some diboron, \(\mathrm{B}_{2}\). a. What is the bond order in \(\mathrm{Li}_{2}\) and \(\mathrm{B}_{2}\) ? b. How many electrons must be removed from \(\mathrm{B}_{2}\) to make it isoelectronic with \(\mathrm{Li}_{2}\) so that it might be used in the warp drive? c. The reaction to make \(\mathrm{B}_{2}\) isoelectronic with \(\mathrm{Li}_{2}\) is generalized (where \(n=\) number of electrons determined in part b) as follows: $$ \mathrm{B}_{2} \longrightarrow \mathrm{B}_{2}^{n+}+n \mathrm{e}^{-} \quad \Delta H=6455 \mathrm{~kJ} / \mathrm{mol} $$ How much energy is needed to ionize \(1.5 \mathrm{~kg} \mathrm{~B}_{2}\) to the desired isoelectronic species?

Which of the following are predicted by the molecular orbital model to be stable diatomic species? a. \(\mathrm{N}_{2}{ }^{2-}, \mathrm{O}_{2}^{2-}, \mathrm{F}_{2}^{2-}\) b. \(\mathrm{Be}_{2}, \mathrm{~B}_{2}, \mathrm{Ne}_{2}\)

Acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) can be produced from the reaction of calcium carbide \(\left(\mathrm{CaC}_{2}\right)\) with water. Use both the localized electron and molecular orbital models to describe the bonding in the acetylide anion \(\left(\mathrm{C}_{2}^{2-}\right)\)

The \(\mathrm{N}_{2} \mathrm{O}\) molecule is linear and polar. a. On the basis of this experimental evidence, which arrangement, NNO or NON, is correct? Explain your answer. b. On the basis of your answer to part a, write the Lewis structure of \(\mathrm{N}_{2} \mathrm{O}\) (including resonance forms). Give the formal charge on each atom and the hybridization of the central atom. c. How would the multiple bonding in \(: \mathrm{N} \equiv \mathrm{N}-\mathrm{O}:\) be described in terms of orbitals?
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