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Chapter 8: Problem 33

Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those that are incorrect. a. \(\delta^{+} \mathrm{H}-\mathrm{F}^{\delta-}\) d. \(^{\delta+} \mathrm{Br}-\mathrm{Br}^{\delta-}\) b. \(^{\delta+} \mathrm{Cl}-\mathrm{I}^{\delta-}\) e. \(^{\delta+} \mathrm{O}-\mathrm{P}^{\delta-}\) c. \(\delta+\mathrm{Si}-\mathrm{S}^{\delta-}\)

Short Answer

Expert verified
The incorrect bond polarity representations are: d. \(\delta^{+} \mathrm{Br}-\mathrm{Br}^{\delta-}\) (Corrected to Br-Br) e. \(^{\delta+} \mathrm{O}-\mathrm{P}^{\delta-}\) (Corrected to \(\delta^{-}\mathrm{O}-\mathrm{P}^{\delta+}\)) b. \(^{\delta+} \mathrm{Cl}-\mathrm{I}^{\delta-}\) (Corrected to \(\delta^{-}\mathrm{Cl}-\mathrm{I}^{\delta+}\))

Step by step solution

01

Analyze Each Bond Individually

In order to determine if the bond polarity is represented correctly or not, we will analyze each bond one by one.
02

Analyze Bond a.

a. \(\delta^{+} \mathrm{H}-\mathrm{F}^{\delta-}\) Fluorine (F) is more electronegative than Hydrogen (H), so this bond polarity representation is correct.
03

Analyze Bond d.

d. \(^{\delta+} \mathrm{Br}-\mathrm{Br}^{\delta-}\) In this case, Br (Bromine) atoms have the same electronegativity, and thus there is no difference in electronegativity between the two bonded atoms. Therefore, this bond is nonpolar, and the representation is incorrect. The correct representation for a nonpolar bond between two Br atoms is: Br-Br
04

Analyze Bond b.

b. \(^{\delta+} \mathrm{Cl}-\mathrm{I}^{\delta-}\) In this case, Cl (Chlorine) is more electronegative than I (Iodine), which means that the bond polarity representation is incorrect. The correct representation should be: \(\delta^{-}\mathrm{Cl}-\mathrm{I}^{\delta+}\)
05

Analyze Bond e.

e. \(^{\delta+} \mathrm{O}-\mathrm{P}^{\delta-}\) Oxygen (O) is more electronegative than Phosphorus (P) in this bond, so the bond polarity representation is incorrect. The correct representation should be: \(\delta^{-}\mathrm{O}-\mathrm{P}^{\delta+}\)
06

Analyze Bond c.

c. \(\delta+\mathrm{Si}-\mathrm{S}^{\delta-}\) Silicon (Si) is less electronegative than Sulfur (S), so this bond polarity representation is correct.
07

Present the Corrected Bond Polarity Representations

Here are the corrected bond polarity representations: a. \(\delta^{+} \mathrm{H}-\mathrm{F}^{\delta-}\) (Correct as given) d. Br-Br (Corrected) b. \(\delta^{-}\mathrm{Cl}-\mathrm{I}^{\delta+}\) (Corrected) e. \(\delta^{-}\mathrm{O}-\mathrm{P}^{\delta+}\) (Corrected) c. \(\delta+\mathrm{Si}-\mathrm{S}^{\delta-}\) (Correct as given)

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Most popular questions from this chapter

Which of the following compounds or ions exhibit resonance? a. \(\mathrm{O}_{3}\) b. \(\mathrm{CNO}^{-}\) c. AsI \(_{3}\) d. \(\mathrm{CO}_{3}^{2-}\) e. \(\mathrm{AsF}_{3}\)

Write Lewis structures that obey the octet rule for each of the following molecules and ions. (In each case the first atom listed is the central atom.) a. \(\mathrm{POCl}_{3}, \mathrm{SO}_{4}^{2-}, \mathrm{XeO}_{4}, \mathrm{PO}_{4}^{3-}, \mathrm{ClO}_{4}^{-}\) b. \(\mathrm{NF}_{3}, \mathrm{SO}_{3}{ }^{2-}, \mathrm{PO}_{3}{ }^{3-}, \mathrm{ClO}_{3}^{-}\) c. \(\mathrm{ClO}_{2}^{-}, \mathrm{SCl}_{2}, \mathrm{PCl}_{2}^{-}\) d. Considering your answers to parts \(\mathrm{a}, \mathrm{b}\), and \(\mathrm{c}\), what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons?

Predict the molecular structure (including bond angles) for each of the following. a. \(\mathrm{SeO}_{3}\) b. \(\mathrm{SeO}_{2}\)

List all the possible bonds that can occur between the elements \(\mathrm{P}, \mathrm{Cs}, \mathrm{O}\), and \(\mathrm{H}\). Predict the type of bond (ionic, covalent, or polar covalent) one would expect to form for each bond.

List the bonds \(\mathrm{P}-\mathrm{Cl}, \mathrm{P}-\mathrm{F}, \mathrm{O}-\mathrm{F}\), and \(\mathrm{Si}-\mathrm{F}\) from least polar to most polar.
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