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.

Verified step by step guidance

Identify the atomic numbers of carbon (C) and oxygen (O) to determine the number of electrons each atom contributes. Carbon has 6 electrons and oxygen has 8 electrons.

Calculate the total number of electrons in the CO molecule, which is the sum of electrons from both carbon and oxygen.

Refer to the molecular orbital theory and the order of energy levels for N2, since CO has the same energy order. The order is: 1σ, 2σ, 1π, 3σ, 2π, 4σ.

Fill the molecular orbitals with the total number of electrons calculated in step 2, starting from the lowest energy orbital (1σ) to the highest energy orbital that can be filled with the available electrons.

Write the electron configuration for the valence molecular orbitals of CO, focusing on the orbitals that are occupied in the valence shell (outermost electrons).

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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 diatomic molecules like CO, these orbitals can be bonding, antibonding, or non-bonding, and their energy levels determine the stability and properties of the molecule. Understanding this theory is essential for predicting the electron configuration of molecules.

Electron Configuration

Electron configuration refers to the distribution of electrons in the molecular orbitals of a molecule. For CO, the electron configuration is derived from the combination of the atomic orbitals of carbon and oxygen, following the principles of Aufbau, Pauli exclusion, and Hund's rule. This configuration helps in understanding the bonding characteristics and reactivity of the molecule.

Energy Order of Molecular Orbitals

The energy order of molecular orbitals is crucial for determining how electrons fill these orbitals. For CO, the energy order is similar to that of N2, where the σ(2s) and σ*(2s) orbitals are lower in energy than the π(2p) and σ(2p) orbitals. This order influences the stability and magnetic properties of the molecule, making it important for analyzing molecular behavior.

Recommended video:

Guided course

03:33

Molecular Orbital Diagram

Related Practice

Textbook Question

Calcium carbide, CaC2, reacts with water to produce acetylene,C2H2, and is sometimes used as a convenient source ofthat substance. Use the MO energy diagram in Figure 8.22ato describe the bonding in the carbide anion, C22-. What isits bond order?

Textbook Question

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).

Textbook Question

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 S₂^2- is formed. Is the bond length in S₂^2- likely to be shorter or longer than the bond length in S₂? Explain.

Textbook Question

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

views

Textbook Question

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?

Textbook Question

Make a sketch showing the location and geometry of thep orbitals in the nitrite ion, NO2-. Describe the bonding inthis ion using a localized valence bond model for s bondingand a delocalized MO model for p bonding.