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Chapter 11: Problem 35

Write plausible molecular orbital diagrams for the following heteronuclear diatomic species: (a) \(\mathrm{NO} ;\) (b) \(\mathrm{NO}^{+}\) (c) \(\mathrm{CO} ;\) (d) \(\mathrm{CN} ;\) (e) \(\mathrm{CN}^{-} ;\) (f) \(\mathrm{CN}^{+} ;\) (g) BN.

Short Answer

Expert verified
The molecular orbital diagrams for these molecules and ions involve determining the total number of electons and filling in the orbitals from lowest to highest energy. For \(\mathrm{NO}\), there are 11 electons, one in \(\sigma_\mathrm{2s}\), one in \(\sigma^*_\mathrm{2s}\), two in \(\sigma_\mathrm{2p}\), four in \(\pi_\mathrm{2p}\), one in \(\pi^*_\mathrm{2p}\), and none in \(\sigma^*_\mathrm{2p}\). Follow this procedure for the other molecules and ions.

Step by step solution

01

Electron Configuration

First determine the total number of valence electrons in the molecule or ion. Use the electron configuration of each atom to determine this. For example, if we consider \(\mathrm{NO}\), Nitrogen (N) has 5 valence electrons and Oxygen (O) has 6, giving us a total of 11 electrons.
02

Construct the Diagram

Draw a horizontal line to represent each molecular orbital. The energy levels of the atomic orbitals of nitrogen and oxygen are similar, so we can place them at the same energy level. The general order for energies of molecular orbitals is \(\sigma_\mathrm{2s}, \sigma^*_\mathrm{2s}, \sigma_\mathrm{2p}, \pi_\mathrm{2p}, \pi^*_\mathrm{2p}, \sigma^*_\mathrm{2p}\). Fill the molecular orbitals with the 11 electrons, starting from the lowest energy orbital and going upwards. If an orbital is filled, proceed to the next one. The π_\mathrm{2p} orbitals can hold 4 electrons, so fill both orbitals with two electrons each. The last electron will go into the \(\pi_\mathrm{2p}\) anti-bonding orbital.
03

Repeat the Process

Repeat steps 1 and 2 for \(\mathrm{NO^{+}}\), \(\mathrm{CO}\), \(\mathrm{CN}\), \(\mathrm{CN^{-}}\), \(\mathrm{CN^{+}}\) and \(\mathrm{BN}\). Remember that a positive charge means one less electron, a negative charge means an extra electron, and that Carbon (C) and Boron (B) both have 4 valence electrons

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Most popular questions from this chapter

A solar cell that is \(15 \%\) efficient in converting solar to electric energy produces an energy flow of \(1.00 \mathrm{kW} / \mathrm{m}^{2}\) when exposed to full sunlight. (a) If the cell has an area of \(40.0 \mathrm{cm}^{2}\), what is the power output of the cell, in watts? (b) If the power calculated in part (a) is produced at \(0.45 \mathrm{V},\) how much current does the cell deliver?

For the following pairs of molecular orbitals, indicate the one you expect to have the lower energy, and state the reason for your choice. (a) \(\sigma_{1 s}\) or \(\sigma_{1 s}^{*} ;\) (b) \(\sigma_{2 s}\) or \(\sigma_{2 p}\) (c) \(\sigma_{1 s}^{*}\) or \(\sigma_{2 s} ;\) (d) \(\sigma_{2 p}\) or \(\sigma_{2 p}^{*}\)

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