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Chapter 9: Problem 23

Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom: (a) four bonding domains and no nonbonding domains, (b) three bonding domains and two nonbonding domains, (c) five bonding domains and one nonbonding domain, (d) four bonding domains and two nonbonding domains.

Short Answer

Expert verified
(a) Electron-domain geometry: tetrahedral, Molecular geometry: tetrahedral (e.g. CH4) (b) Electron-domain geometry: trigonal bipyramidal, Molecular geometry: T-shaped (e.g. ClF3) (c) Electron-domain geometry: octahedral, Molecular geometry: square pyramidal (e.g. SF6) (d) Electron-domain geometry: octahedral, Molecular geometry: square planar (e.g. XeF4)

Step by step solution

01

(a) Four bonding domains and no nonbonding domains

With four bonding domains and no nonbonding domains, the electron-domain geometry is tetrahedral, as all electron pairs are equally distributed around the central atom. Since all the electrons are involved in bonding, the molecular geometry is also tetrahedral. An example of a molecule with this configuration would be methane (CH4).
02

(b) Three bonding domains and two nonbonding domains

With three bonding domains and two nonbonding domains, the electron-domain geometry is trigonal bipyramidal. In this case, due to the presence of two nonbonding domains, the molecular geometry will be T-shaped. An example of a molecule with this configuration would be chlorine trifluoride (ClF3).
03

(c) Five bonding domains and one nonbonding domain

With five bonding domains and one nonbonding domain, the electron-domain geometry is octahedral. The molecular geometry will be square pyramidal, as only five electron domains are involved in bonding. An example of a molecule with this configuration would be sulfur hexafluoride (SF6).
04

(d) Four bonding domains and two nonbonding domains

With four bonding domains and two nonbonding domains, the electron-domain geometry is octahedral. However, due to the presence of two nonbonding domains, the molecular geometry will be square planar. An example of a molecule with this configuration would be xenon hexafluoride (XeF4).

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Most popular questions from this chapter

The structure of borazine, \(\mathrm{B}_{3} \mathrm{~N}_{3} \mathrm{H}_{6},\) is a six-membered ring of alternating \(\mathrm{B}\) and \(\mathrm{N}\) atoms. There is one \(\mathrm{H}\) atom bonded to each \(B\) and to each \(\mathrm{N}\) atom. The molecule is planar. (a) Write a Lewis structure for borazine in which the formal charge on every atom is zero. (b) Write a Lewis structure for borazine in which the octet rule is satisfied for every atom. (c) What are the formal charges on the atoms in the Lewis structure from part (b)? Given the electronegativities of \(B\) and \(N,\) do the formal charges seem favorable or unfavorable? (d) Do either of the Lewis structures in parts (a) and (b) have multiple resonance structures? (e) What are the hybridizations at the \(\mathrm{B}\) and \(\mathrm{N}\) atoms in the Lewis structures from parts (a) and (b)? Would you expect the molecule to be planar for both Lewis structures? (f) The six \(\mathrm{B}-\mathrm{N}\) bonds in the borazine molecule are all identical in length at \(144 \mathrm{pm} .\) Typical values for the bond lengths of \(\mathrm{B}-\mathrm{N}\) single and double bonds are \(151 \mathrm{pm}\) and \(131 \mathrm{pm},\) respectively. Does the value of the \(\mathrm{B}-\mathrm{N}\) bond length seem to favor one Lewis structure over the other? (g) How many electrons are in the \(\pi\) system of botazine?

(a) An \(\mathrm{AB}_{6}\) molecule has no lone pairs of electrons on the \(\mathrm{A}\) atom. What is its molecular geometry? (b) An \(\mathrm{AB}_{4}\) molecule has two lone pairs of electrons on the A atom (in addition to the four \(\mathrm{B}\) atoms). What is the electron-domain geometry around the A atom? (c) For the \(\mathrm{AB}_{4}\) molecule in part (b), predict the molecular geometry.

Determine the electron configurations for \(\mathrm{CN}^{+}, \mathrm{CN}\), and \(\mathrm{CN}^{-}\). (a) Which species has the strongest \(\mathrm{C}-\mathrm{N}\) bond? (b) Which species, if any, has unpaired electrons?

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 6.23 ) is most likely 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 oforbitals, explain why a node is generated in the \(\sigma_{3 d}^{*}\) MO. (d) Sketch the energylevel 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) Draw a picture showing how two \(p\) orbitals on two different atoms can be combined to make a \(\sigma\) bond. (b) Sketch a \(\pi\) bond that is constructed from \(p\) orbitals. (c) Which is generally stronger, a \(\sigma\) bond or a \(\pi\) bond? Explain. (d) Can two s orbitals combine to form a \(\pi\) bond? Explain.
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