Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 79d

Chapter 9, Problem 79d

Using Figures 9.39 and 9.43 as guides, draw the molecular-orbital electron configuration for (d) Ne22+. In each case indicate whether the addition of an electron to the ion would increase or decrease the bond order of the species.

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Step 1: Identify the atomic number of Ne (Neon). The atomic number of Neon is 10. However, since we are dealing with Ne22+, it means that it has lost two electrons, so it has 8 electrons.

Step 2: Draw the molecular orbital diagram for Ne22+. The molecular orbital diagram for a molecule with 8 electrons would have 2 electrons in the 1s orbital, 2 electrons in the 2s orbital, and 4 electrons in the 2p orbital.

Step 3: Calculate the bond order. The bond order is calculated as (number of electrons in bonding orbitals - number of electrons in antibonding orbitals) / 2. In this case, all the electrons are in bonding orbitals, so the bond order is (8 - 0) / 2 = 4.

Step 4: Determine the effect of adding an electron. If an electron is added to Ne22+, it would go into an antibonding orbital, which would decrease the bond order.

Step 5: Summarize the results. The molecular orbital electron configuration for Ne22+ has a bond order of 4. Adding an electron to the ion would decrease the bond order.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molecular Orbital Theory

Molecular Orbital Theory describes how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons. In this theory, electrons are delocalized over the entire molecule rather than being confined to individual atoms. Understanding this concept is crucial for determining the electron configuration of molecules and ions, as well as predicting their stability and bond order.

Bond Order

Bond order is a measure of the number of chemical bonds between a pair of atoms, calculated as the difference between the number of bonding and antibonding electrons divided by two. A higher bond order indicates a stronger bond and greater stability of the molecule. In the context of the question, determining how the addition of an electron affects bond order is essential for understanding the stability of the Ne22+ ion.

Electron Configuration

Electron configuration refers to the distribution of electrons in an atom or ion's molecular orbitals. For ions like Ne22+, the electron configuration must account for the loss of electrons due to ionization. Accurately drawing the electron configuration is vital for predicting how the addition of an electron will influence the bond order and overall stability of the species.

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Textbook Question

Determine the electron configurations for CN+, CN, and CN-. (a) Which species has the strongest C¬N bond?

Textbook Question

If we assume that the energy-level diagrams for homonuclear diatomic molecules shown in Figure 9.43 can be applied to heteronuclear diatomic molecules and ions, predict the bond order and magnetic behavior of b. NO–

Textbook Question

a. Based on its molecular-orbital diagram, what is the bond order of the O2 molecule?

b. What is the expected bond order for the peroxide ion, O22−?

c. What is the expected bond order for the superoxide ion, O2−?

d. From shortest to longest, predict the ordering of the bond lengths for O2, O22−, and O2−.

e. From weakest to strongest, predict the ordering of the bond strengths for O2, O22−, and O2−.

Textbook Question

a. Which of the following is expected to be paramagnetic: Ne, Li2, Li2+, N2, N2+, N22−? b. For each of the substances in part (a) that is paramagnetic, determine the number of unpaired electrons it has.

Textbook Question

Determine whether each of the following statements about diamagnetism and paramagnetism is true or false:

a. A diamagnetic substance is weakly repelled from a magnetic field.

b. A substance with unpaired electrons will be diamagnetic.

c. A paramagnetic substance is attracted to a magnetic field.

d. The O2 molecule is paramagnetic.