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Chapter 9: Problem 32

In which of the following AF \(_{n}\) molecules or ions is there more than one \(\mathrm{F}-\mathrm{A}-\mathrm{F}\) bond angle: $\mathrm{PF}_{6}^{-}, \mathrm{SbF}_{\mathrm{s}}, \mathrm{SF}_{4} ?$

Short Answer

Expert verified
The molecular geometry of each molecule/ion is as follows: 1. PF6-: Octahedral 2. SbFs: Trigonal bipyramidal 3. SF4: Seesaw or distorted tetrahedral All three molecules or ions, PF6-, SbFs, and SF4, have more than one F-A-F bond angle.

Step by step solution

01

1. PF6-

Phosphorus (P) has 5 valence electrons and Fluorine (F) has 7 valence electrons. The PF6- ion has 5+6(7)+1(extra electron) = 48 electrons. In this complex, P is the central atom, surrounded by 6 fluorine atoms. To minimize the repulsion between electron pairs, the molecular geometry of PF6- will be an octahedral, with 6 F-A (P-F) bonds. This structure will have several F-P-F angles of 90 and 180 degrees. Therefore, PF6- has more than one F-A-F bond angle.
02

₂. SbFs

Antimony (Sb) has 5 valence electrons, and Fluorine (F) has 7 valence electrons. The overall molecule has 5+5(7) = 40 electrons. In this molecule, Sb is the central atom, surrounded by 5 fluorine atoms. To minimize the repulsion between electron pairs, the molecular geometry of SbFs is trigonal bipyramidal, with 5 F-A (Sb-F) bonds. SbFs has 3 equatorial (F-Sb-F) angles equal to 120 degrees (at the central plane), and 2 axial (F-Sb-F) angles equal to 180 degrees, perpendicular to the central plane. Therefore, there are multiple F-A-F bond angles in SbFs.
03

₃. SF4

Sulfur (S) has 6 valence electrons and Fluorine (F) has 7 valence electrons. In the SF4 molecule, there are 6+4(7) = 34 electrons. In this molecule, S is the central atom, surrounded by 4 fluorine atoms with one lone pair on S. The molecular geometry of SF4 is called seesaw or distorted tetrahedral. The SF4 molecule has two S-F bond angles in the equatorial plane, equal to 120 degrees; and on each of two axial positions perpendicular (F-S-F) to the central plane, the angle is 180 degrees. Thus, there are more than one F-A-F bond angles in SF4. All three molecules or ions, PF6-, SbFs, and SF4, have more than one F-A-F bond angle.

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Most popular questions from this chapter

In ozone, \(\mathrm{O}_{3}\), the two oxygen atoms on the ends of the molecule are equivalent to one another. (a) What is the best choice of hybridization scheme for the atoms of ozone? (b) For one of the resonance forms of ozone, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons? (c) Which of the orbitals can be used to delocalize the \(\pi\) electrons? (d) How many electrons are delocalized in the \(\pi\) system of ozone?

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, \(\mathrm{C}_{12} \mathrm{H}_{10} \mathrm{~N}_{2}\) A closely related substance is hydrazobenzene, $\mathrm{C}_{12} \mathrm{H}_{12} \mathrm{~N}_{2}$ (Recall the shorthand notation used for benzene.) (a) What is the hybridization at the \(\mathrm{N}\) atom in each of the substances? (b) How many unhybridized atomic orbitals are there on the \(\mathrm{N}\) and the \(\mathrm{C}\) atoms in each of the substances? (c) Predict the \(\mathrm{N}-\mathrm{N}-\mathrm{C}\) angles in each of the substances. (d) Azobenzene is said to have greater delocalization of its \(\pi\) electrons than hydrazobenzene. Discuss this statement in light of your answers to (a) and (b). (e) All the atoms of azobenzene lie in one plane, whereas those of hydrazobenzene do not. Is this observation consistent with the statement in part (d)? (f) Azobenzene is an intense red-orange color, whereas hydrazobenzene is nearly colorless. Which molecule would be a better one to use in a solar energy conversion device? (See the "Chemistry Put to Work" box for more information about solar cells.)

What is the distinction between a bond dipole and a molecular dipole moment?

Consider the molecule \(\mathrm{PF}_{4}\) Cl. (a) Draw a Lewis structure for the molecule, and predict its electron-domain geometry. (b) Which would you expect to take up more space, a \(\mathrm{P}-\mathrm{F}\) bond or a \(\mathrm{P}-\mathrm{Cl}\) bond? Explain. (c) Predict the molecular geometry of \(\mathrm{PF}_{4} \mathrm{Cl}\). How did your answer for part (b) influence your answer here in part (c)? (d) Would you expect the molecule to distort from its ideal electron-domain geometry? If so, how would it distort?

How would you expect the extent of overlap of the bonding atomic orbitals to vary in the series IF, ICl, IBr, and \(I_{2}\) ? Explain your answer.
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