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Chapter 9: Problem 11

An \(\mathrm{AB}_{2}\) molecule is described as linear, and the \(\mathrm{A}-\mathrm{B}\) bond length is known. (a) Does this information completely describe the geometry of the molecule? (b) Can you tell how many nonbonding pairs of electrons are around the A atom from this information?

Short Answer

Expert verified
(a) No, the given information does not completely describe the geometry of the molecule, as knowledge of the bond angle, and the hybridization is also essential. (b) No, we cannot determine the number of nonbonding pairs of electrons around the A atom from the given information.

Step by step solution

01

Molecular Geometry: Linear Molecules

In a linear AB2 molecule, the central atom (A) is bonded to two peripheral atoms (B). The electronic geometry of the molecule, describing the arrangement of the electron pairs, is determined by considering the central atom A. Let us call the bond angle between the two B atoms as θ. If the two B atoms are identical, hybridization will be required for A to bond with both B atoms. If the molecule has 180 degrees as bond angle (θ), this indicates that the geometry of the molecule is linear. The spatial orientation of the molecule is such that all the atoms are placed in a straight line.
02

Importance of Bond Length

Knowing the bond length of A-B is helpful to describe the distance between two adjacent atoms in the molecule. However, simply knowing the bond length does not fully describe the geometry of the molecule as we still need to know the bond angle (θ) to determine the electronic geometry based on the hybridization. Since the molecule is linear, we can easily conclude that the bond angle will be 180 degrees.
03

Determining Nonbonding Pairs of Electrons

Analyzing the information regarding the number of nonbonding electron pairs is crucial to fully describe the geometry of the molecule. However, the given information does not provide any insight into the electron pairs present around the central atom A. Consequently, we cannot deduce the number of nonbonding electron pairs around the A atom from the current information. To answer the questions in the exercise: (a) No, the given information does not completely describe the geometry of the molecule, as knowledge of the bond angle and the hybridization is also essential. (b) No, we cannot determine the number of nonbonding pairs of electrons around the A atom from the given information.

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Most popular questions from this chapter

(a) What is the probability of finding an electron on the internuclear axis if the electron occupies a \(\pi\) molecular orbital? (b) For a homonuclear diatomic molecule, what similarities and differences are there between the \(\pi_{2 p}\) MO made from the \(2 p_{x}\) atomic orbitals and the \(\pi_{2 p}\) MO made from the \(2 p_{y}\) atomic orbitals? (c) Why are the \(\pi_{2 p}\) MOs lower in energy than the \(\pi_{2 p}^{*}\) MOs?

(a) Explain why the following ions have different bond angles: \(\mathrm{C} 1 \mathrm{O}_{2}^{-}\) and \(\mathrm{NO}_{2}^{-}\). Predict the bond angle in each case. (b) Explain why the \(\mathrm{XeF}_{2}\) molecule is linear and not bent.

Why are there no \(s p^{4}\) or \(s p^{5}\) hybrid orbitals?

Many compounds of the transition-metal elements contain direct bonds between metal atoms. We will assume that the \(z\) -axis is defined as the metal-metal bond axis. (a) Which of the \(3 d\) orbitals (Figure 6.24) can be used to make a \(\sigma\) bond between metal atoms? (b) Sketch the \(\sigma_{3 d}\) bonding and \(\sigma_{3 d}^{*}\) antibonding MOs. (c) With reference to the "Closer Look" box on the phases of orbitals, explain why a node is generated in the \(\sigma_{3 d}^{*}\) MO. (d) Sketch the energy-level diagram for the \(\mathrm{Sc}_{2}\) molecule, assuming that only the \(3 d\) orbital from part (a) is important. (e) What is the bond order in \(\mathrm{Sc}_{2} ?\)

(a) The nitric oxide molecule, NO, readily loses one electron to form the \(\mathrm{NO}^{+}\) ion. Why is this consistent with the electronic structure of NO? (b) Predict the order of the \(\mathrm{N}-\mathrm{O}\) bond strengths in \(\mathrm{NO}, \mathrm{NO}^{+}\), and \(\mathrm{NO}^{-}\), and describe the magnetic properties of each (c) With what neutral homonuclear diatomic molecules are the \(\mathrm{NO}^{+}\) and \(\mathrm{NO}^{-}\) ions isoelectronic (same number of electrons)?
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