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Chapter 10: Problem 61

Each of the following is either linear, angular (bent), planar, tetrahedral, or octahedral. Indicate the correct shape of (a) \(\mathrm{H}_{2} \mathrm{S} ;\) (b) \(\mathrm{N}_{2} \mathrm{O}_{4} ;\) (c) \(\mathrm{HCN} ;\) (d) \(\mathrm{SbCl}_{6}^{-}\); (e) \(\mathrm{BF}_{4}^{-}\)

Short Answer

Expert verified
(a) H2S is angular (bent), (b) N2O4 is planar, (c) HCN is linear, (d) SbCl6- is octahedral, (e) BF4- is tetrahedral.

Step by step solution

01

Analyze the Compound H2S

Sulfur (S) is the central atom. It has two bonds with Hydrogen (H) and two lone pairs of electrons. According to VSEPR theory, such an arrangement leads to a bent (or angular) molecular shape.
02

Analyze the Compound N2O4

The molecule N2O4 can be described as two NO2 molecules bonded together, with Nitrogen (N) being the central atom. Each Nitrogen forms two bonds with Oxygen (O) and has one lone pair, leading to a bent shape for each NO2. The overall shape of N2O4 is therefore described as planar.
03

Analyze the Compound HCN

Carbon (C) is the central atom in HCN, being bonded to both Hydrogen (H) and Nitrogen (N), with no lone pairs on the Carbon. This results in a linear molecular shape.
04

Analyze the Ion SbCl6-

Antimony (Sb) is the central atom in SbCl6-, surrounded by six Chlorine (Cl) atoms. There is no lone pair on the Antimony. According to VSEPR theory, this configuration results in an octahedral molecular shape.
05

Analyze the Ion BF4-

Boron (B) is the central atom in BF4-, surrounded by four Fluorine (F) atoms and no lone pairs. This results in a tetrahedral molecular shape.

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Most popular questions from this chapter

A \(0.325 \mathrm{g}\) sample of a gaseous hydrocarbon occupies a volume of \(193 \mathrm{mL}\) at \(749 \mathrm{mmHg}\) and \(26.1^{\circ} \mathrm{C}\). Determine the molecular mass, and write a plausible condensed structural formula for this hydrocarbon.

Give several examples for which the following statement proves to be incorrect. "All atoms in a Lewis structure have an octet of electrons in their valence shells."

Construct a concept map illustrating the connections between Lewis dot structures, the shapes of molecules, and polarity.

Explain why it is not necessary to find the Lewis structure with the smallest formal charges to make a successful prediction of molecular geometry in the VSEPR theory. For example, write Lewis structures for \(S O_{2}\) having different formal charges, and predict the molecular geometry based on these structures.

Which of the following species would you expect to be diamagnetic and which paramagnetic: (a) \(\mathrm{OH}^{-} ;\) (b) \(\mathrm{OH} ;(\mathrm{c}) \mathrm{NO}_{3} ;(\mathrm{d}) \mathrm{SO}_{3} ;(\mathrm{e}) \mathrm{SO}_{3}^{2-} ;(\mathrm{f}) \mathrm{HO}_{2} ?\)
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