Ch.9 - Molecular Geometry and Bonding Theories

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.9 - Molecular Geometry and Bonding Theories

Problem 79d

Chapter 9, Problem 79d

Using Figures 9.35 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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Identify the total number of electrons in the neutral Ne2 molecule. Neon (Ne) has 10 electrons, so Ne2 has 20 electrons.

Since Ne2^2+ is given, remove 2 electrons from the total electron count of Ne2, resulting in 18 electrons for Ne2^2+.

Draw the molecular orbital (MO) diagram for Ne2^2+. Start by filling the molecular orbitals with the 18 electrons, following the order: \(\sigma_{1s}, \sigma_{1s}^*, \sigma_{2s}, \sigma_{2s}^*, \sigma_{2p_z}, \pi_{2p_x} = \pi_{2p_y}, \pi_{2p_x}^* = \pi_{2p_y}^*, \sigma_{2p_z}^*\).

Calculate the bond order using the formula: \(\text{Bond Order} = \frac{(\text{Number of bonding electrons} - \text{Number of antibonding electrons})}{2}\).

Consider the effect of adding an electron to Ne2^2+. Determine if the electron would enter a bonding or antibonding orbital and how this would affect 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 associated with 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. It is represented by a series of numbers and letters that indicate the energy levels and types of orbitals occupied by electrons. For Ne22 +, accurately drawing the electron configuration is necessary to analyze how the addition of an electron influences the overall molecular stability and bond characteristics.

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Textbook Question

Explain the following: (c) The O22 + ion has a stronger O—O bond than O2 itself.

How would we describe a substance that contains only paired electrons and is weakly repelled by a magnetic field? Which of the following ions would you expect to possess similar characteristics: H2-, Ne2+, F2, O22 +?

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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+.

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

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