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Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure
McMurry - Chemistry 8th Edition
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Capitolo 8, Problema 107b

Carbon monoxide is produced by incomplete combustion of fossil fuels. (b) Do you expect CO to be paramagnetic or diamagnetic?

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Understand the terms: Paramagnetic substances are attracted to magnetic fields due to unpaired electrons in their atomic or molecular structures, while diamagnetic substances are repelled by magnetic fields as all their electrons are paired.
Determine the electron configuration of carbon monoxide (CO). Carbon has an atomic number of 6 and oxygen has an atomic number of 8. In the CO molecule, these atoms share electrons.
Analyze the bonding in CO: CO has a triple bond between the carbon and oxygen atoms (one sigma bond and two pi bonds), and there is also a lone pair of electrons on the carbon.
Examine the molecular orbital diagram for CO, focusing on the highest occupied molecular orbital (HOMO) to check for the presence of unpaired electrons.
Conclude whether CO is paramagnetic or diamagnetic based on the presence or absence of unpaired electrons in the molecular orbitals.

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Paramagnetism and Diamagnetism

Paramagnetism occurs in substances that have unpaired electrons, which create a net magnetic moment, allowing them to be attracted to magnetic fields. In contrast, diamagnetism is exhibited by substances with all paired electrons, resulting in no net magnetic moment, causing them to be weakly repelled by magnetic fields. Understanding these properties is essential for predicting the magnetic behavior of molecules.
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01:33
Paramagnetism and Diamagnetism

Molecular Orbital Theory

Molecular Orbital Theory explains how atomic orbitals combine to form molecular orbitals, which can be occupied by electrons. In this theory, electrons are distributed among bonding, antibonding, and non-bonding orbitals. The arrangement of electrons in these orbitals determines whether a molecule is paramagnetic or diamagnetic, based on the presence of unpaired electrons.
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Molecular Orbital Theory

Electron Configuration of Carbon Monoxide (CO)

Carbon monoxide (CO) consists of one carbon atom and one oxygen atom, and its electron configuration can be analyzed using molecular orbital theory. In CO, the molecular orbitals are filled according to the Aufbau principle, leading to a configuration where there is one unpaired electron in a π* antibonding orbital. This unpaired electron is what makes CO paramagnetic, as it contributes to a net magnetic moment.
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Electron Configuration Example
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At high temperatures, sulfur vapor is predominantly in the form of S2(g) molecules. (a) Assuming that the molecular orbitals for third-row diatomic molecules are analogous to those for second-row molecules, construct an MO diagram for the valence orbitals of S2(g).

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Carbon monoxide is produced by incomplete combustion of fossil fuels. (c) What is the bond order of CO? Does this match the bond order predicted by the electron-dot structure?

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Carbon monoxide is produced by incomplete combustion of fossil fuels. (a) Give the electron configuration for the valence molecular orbitals of CO. The orbitals have the same energy order as those of the N2 molecule.

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In the cyanate ion, OCN-, carbon is the central atom. (d) Which hybrid orbitals are used by the C atom, and how many p bonds does the C atom form?
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Make a sketch showing the location and geometry of the p orbitals in the nitrite ion, NO2-. Describe the bonding in this ion using a localized valence bond model for s bonding and a delocalized MO model for p bonding.
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At high temperatures, sulfur vapor is predominantly in the form of S2(g) molecules. (d) When two electrons are added to S2, the disulfide ion S22- is formed. Is the bond length in S22- likely to be shorter or longer than the bond length in S2? Explain.

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