(b) How many of the MOs from part (a) would be occupied by electrons?

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First, identify the molecule or ion for which you are determining the molecular orbitals (MOs). This will help you understand the electron configuration and the number of electrons involved.

Determine the total number of valence electrons in the molecule or ion. This is typically done by adding up the valence electrons from each atom in the molecule.

Use the molecular orbital theory to construct the molecular orbital diagram for the molecule or ion. This involves arranging the MOs in order of increasing energy, typically starting with bonding orbitals, followed by non-bonding and then anti-bonding orbitals.

Fill the molecular orbitals with electrons according to the Aufbau principle, starting from the lowest energy orbital and moving upwards. Each orbital can hold a maximum of two electrons with opposite spins.

Count the number of occupied molecular orbitals. An occupied orbital is one that contains one or two electrons. This will give you the number of MOs that are occupied by electrons.

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Textbook Question

Azo dyes are organic dyes that are used for many applications, such as the coloring of fabrics. Many azo dyes are derivatives of the organic substance azobenzene, C12H10N2. A closely related substance is hydrazobenzene, C12H12N2. The Lewis structures of these two substances are

(Recall the shorthand notation used for benzene.) (b) How many unhybridized atomic orbitals are there on the N and the C atoms in each of the substances? How many unhybridized atomic orbitals are there on the N and the C atoms in hydrazobenzene?

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Textbook Question

(Recall the shorthand notation used for benzene.) (c) Predict the N¬N¬C angles in each of the substances.

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Textbook Question

a) Using only the valence atomic orbitals of a hydrogen atom and a fluorine atom, and following the model of Figure 9.46, how many MOs would you expect for the HF molecule?

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Textbook Question

(c) It turns out that the difference in energies between the valence atomic orbitals of H and F are sufficiently different that we can neglect the interaction of the 1s orbital of hydrogen with the 2s orbital of fluorine.

The 1s orbital of hydrogen will mix only with one 2p orbital of fluorine. Draw pictures showing the proper orientation of all three 2p orbitals on F interacting with a 1s orbital on H. Which of the 2p orbitals can actually make a bond with a 1s orbital, assuming that the atoms lie on the z-axis?

Textbook Question

Carbon monoxide, CO, is isoelectronic to N2. (d) Would you expect the p2p MOs of CO to have equal atomic orbital contributions from the C and O atoms? If not, which atom would have the greater contribution?

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Textbook Question

The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding π orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the p2p to the p*2p molecular orbital. (a) Assuming this electronic transition corresponds to the HOMO-LUMO transition, what is the HOMO in ethylene?

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