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Chapter 10: Problem 67

Use the VSEPR theory to predict the shapes of the anions (a) \(\mathrm{ClO}_{4}^{-} ;\) (b) \(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\left(\text { that is, } \mathrm{SSO}_{3}^{2-}\right) ;\) (c) \(\mathrm{PF}_{6}^{-}\); (d) I \(_{3}^{-}\).

Short Answer

Expert verified
The shape of \(ClO_{4}^{-}\) is tetrahedral, \(S_{2}O_{3}^{2-}\) is trigonal pyramidal around each S atom, \(PF_{6}^{-}\) is octahedral, and \(I_{3}^{-}\) is linear.

Step by step solution

01

Determine Shape of \(ClO_{4}^{-}\)

For the anion \(ClO_{4}^{-}\), there is one central Cl atom surrounded by 4 O atoms. Each O atom creates a bonding pair with the Cl atom and there are no lone pairs on the central atom. Therefore, following the VSEPR theory, this molecule will have tetrahedral shape.
02

Determine Shape of \(S_{2}O_{3}^{2-}\)

For the anion \(S_{2}O_{3}^{2-}\), there are two central S atoms and three surrounding O atoms. Two O atoms each forms a bonding pair with one S atom, and one O atom has bonds with both S atoms (forming a bridge). The S atoms are effectively bonded to 3 atoms each (two O and one S), and have a lone pair. Following the VSEPR theory, the shape around each S atom is trigonal pyramidal.
03

Determine Shape of \(PF_{6}^{-}\)

In the anion \(PF_{6}^{-}\), the central P atom is surrounded by 6 F atoms, resulting in 6 bonding pairs and no lone pair. According to the VSEPR theory, the shape of this anion will be octahedral.
04

Determine Shape of \(I_{3}^{-}\)

For the anion \(I_{3}^{-}\), there are 3 I atoms and 3 lone pairs around the central atom. This arrangement, following the VSEPR theory, forms a linear shape.

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Most popular questions from this chapter

Derive the correct formulas for the following ionic compounds by writing Lewis structures. (a) lithium sulfide; (b) sodium fluoride; (c) calcium iodide; (d) scandium chloride.

Of the following species, the one with a triple covalent bond is (a) \(\mathrm{NO}_{3}^{-} ;\) (b) \(\mathrm{CN}^{-} ;\) (c) \(\mathrm{CO}_{2} ;\) (d) \(\mathrm{AlCl}_{3}\).

The molecular shape of \(\mathrm{BF}_{3}\) is planar (see Table 10.1 ). If a fluoride ion is attached to the \(B\) atom of \(B F_{3}\) through a coordinate covalent bond, the ion \(\mathrm{BF}_{4}^{-}\) results. What is the shape of this ion?

A compound consists of \(47.5 \%\) S and \(52.5 \%\) Cl, by mass. Write a Lewis structure based on the empirical formula of this compound, and comment on its deficiencies. Write a more plausible structure with the same ratio of \(\mathrm{S}\) to \(\mathrm{Cl}\).

Sketch the propene molecule, \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?
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