For each pair of bonds, identify the more polar one and use δ+ or δ- to indicate the partial cha

Name: Problem 47, Chapter 8: Chemistry: The Molecular Science
Uploaded: 2021-05-27T17:39:55-08:00
Duration: 1 min 43 s
Channel: Lottie Adams
Description: For each pair of bonds, identify the more polar one and use δ+ or δ- to indicate the partial charge on each atom. (a) B-Cl and B-O (b) O-F and O-Se (c) S-Cl and B-F (d) N-H and N-F

step 1 are a class of chemical bonds where the valence electrons are shared between atoms. These are ty

Question

For each pair of bonds, identify the more polar one and use $\delta+$ or $\delta-$ to indicate the partial charge on each atom. (a) $\mathrm{B}-\mathrm{Cl}$ and $\mathrm{B}-\mathrm{O}$ (b) $\mathrm{O}-\mathrm{F}$ and $\mathrm{O}-\mathrm{Se}$ (c) $\mathrm{S}-\mathrm{Cl}$ and $\mathrm{B}-\mathrm{F}$ (d) $\mathrm{N}-\mathrm{H}$ and $\mathrm{N}-\mathrm{F}$

   For each pair of bonds, identify the more polar one and use $\delta+$ or $\delta-$ to indicate the partial charge on each atom.
(a) $\mathrm{B}-\mathrm{Cl}$ and $\mathrm{B}-\mathrm{O}$
(b) $\mathrm{O}-\mathrm{F}$ and $\mathrm{O}-\mathrm{Se}$
(c) $\mathrm{S}-\mathrm{Cl}$ and $\mathrm{B}-\mathrm{F}$
(d) $\mathrm{N}-\mathrm{H}$ and $\mathrm{N}-\mathrm{F}$

Chemistry: The Molecular Science

John W. Moore,… 3rd Edition

Chapter 8, Problem 47

Instant Answer

Solved by Expert Lottie Adams

05/27/2021

Step 1

Electronegativity values are as follows: B = 2.04, Cl = 3.16, and O = 3.44. The difference in electronegativity between B and Cl is 1.12, while the difference between B and O is 1.40. Since the difference is greater for the B-O bond, it is more polar. The partial Show more…

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For each pair of bonds, identify the more polar one and use $\delta+$ or $\delta-$ to indicate the partial charge on each atom. (a) $\mathrm{B}-\mathrm{Cl}$ and $\mathrm{B}-\mathrm{O}$ (b) $\mathrm{O}-\mathrm{F}$ and $\mathrm{O}-\mathrm{Se}$ (c) $\mathrm{S}-\mathrm{Cl}$ and $\mathrm{B}-\mathrm{F}$ (d) $\mathrm{N}-\mathrm{H}$ and $\mathrm{N}-\mathrm{F}$

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Key Concepts

Electronegativity

Electronegativity is a measure of an atom’s tendency to attract electron density towards itself when forming a chemical bond. It is a fundamental concept in understanding molecular structure as differences in electronegativity between bonded atoms lead to unequal sharing of electrons.

Bond Polarity

Bond polarity arises when there is a difference in electronegativity between two atoms forming a covalent bond. This difference results in an uneven distribution of electron density across the bond, creating a dipole moment where one end of the bond is partially negative (?-) and the other is partially positive (?+).

Partial Charge Distribution

Partial charges describe the small electrical charges that develop on atoms within a polar bond due to differences in electronegativity. These charges, typically denoted as ?+ and ?-, are essential for predicting molecular interactions, reactivity, and physical properties.

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