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.

검증된 단계별 안내

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).

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주요 개념

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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.