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Chapter 10: Problem 68

Use the VSEPR theory to predict the shape of (a) the molecule OSF \(_{2} ;\) (b) the molecule \(\mathrm{O}_{2} \mathrm{SF}_{2} ;\) (c) the ion \(\mathrm{SF}_{5}^{-} ;\) (d) the ion \(\mathrm{ClO}_{4}^{-} ;\) (e) the ion \(\mathrm{ClO}_{3}^{-}\).

Short Answer

Expert verified
The molecule OSF2 has a T-shaped, O2SF2 and ClO4- are tetrahedral, SF5- is square pyramidal, and ClO3- is a Trigonal Pyramid.

Step by step solution

01

Identify the central atom

For OSF2, O2SF2, SF5-, and ClO4-, the central atom is S. For ClO3-, it's Cl.
02

Drawing the Lewis structures

Draw structures showcasing all involved bonds and lone electron pairs. This helps to visualize the layout of the molecules/ions. You get for OSF2: S is bounded to O and two F with two lone pairs on S. O2SF2 has S bounded to two O and two F, with no lone pairs. SF5- has S surrounded by five one-bonded F atoms with one lone pair. ClO4- has Cl surrounded by four one-bonded O atoms with no lone pairs. ClO3- has one double-bonded O and two one-bonded O surrounding Cl with one lone pair.
03

Applying the AXE notation

This notation helps to predict the geometry of a molecule. The 'A' stands for the central atom, 'X' represents the number of atoms attached to A and 'E' is the number of lone electron pairs. For OSF2, A=S, X=3, E=2 (AX3E2). For O2SF2, A=S, X=4, E=0 (AX4E0). For SF5-, A=S, X=5, E=1 (AX5E1). For ClO4-, A=Cl, X=4, E=0 (AX4E0). For ClO3-, A=Cl, X=3, E=1 (AX3E1).
04

Predicting the shape

Now you can use the AXE notation to predict the shape of the molecules and ions. For OSF2 (AX3E2), it is a T-Shaped. For O2SF2 (AX4E0), it's Tetrahedral. For SF5- (AX5E1), it's a square pyramidal. For ClO4- (AX4E0), it's also Tetrahedral. For ClO3- (AX3E1), it's a Trigonal Pyramid.

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Most popular questions from this chapter

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

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable: (a) \(\mathrm{HCO}_{2}=\) (b) \(\mathrm{HCO}_{3}^{-}\) (c) \(\mathrm{FSO}_{3}^{-}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}^{2-}\) (the nitrogen atoms are joined centrally with one oxygen atom on one \(\mathrm{N}\) and two on the other)

The molecule \(\mathrm{H}_{2} \mathrm{O}_{2}\) has a resultant dipole moment of 2.2 D. Can this molecule be linear? If not, describe a shape that might account for this dipole moment.

Write plausible Lewis structures for the following free radicals: (a) \(\cdot \mathrm{C}_{2} \mathrm{H}_{5} ;\) (b) \(\mathrm{HO}_{2}\) "; (c) ClO?.

In which of the following molecules would you expect the oxygen-to-oxygen bond to be the shortest: (a) \(\mathrm{H}_{2} \mathrm{O}_{2},\) (b) \(\mathrm{O}_{2},\) (c) \(\mathrm{O}_{3} ?\) Explain.
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