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Chapter 9: Problem 35

What is the distinction between a bond dipole and a molecular dipole moment?

Short Answer

Expert verified
The distinction between a bond dipole and a molecular dipole moment lies in their scope and focus. A bond dipole moment refers specifically to the polarity of a single chemical bond between two atoms in a molecule, primarily determined by their electronegativity difference. In contrast, a molecular dipole moment represents the overall polarity of the entire molecule, determined by summing up the individual bond dipole moments and accounting for the molecular geometry.

Step by step solution

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1. Definition of Bond Dipole Moment

A bond dipole moment is a measure of the polarity of a chemical bond between two atoms within a molecule. It is a vector quantity, which means it has both magnitude and direction. The bond dipole moment is determined by the difference in electronegativity between the two atoms forming the bond and the distance between them. When electrons are shared unequally between atoms, it results in a polar bond, with a positive and negative end (called a dipole). The dipole moment can be represented by an arrow pointing from the positive end to the negative end (from less electronegative to more electronegative atom).
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2. Definition of Molecular Dipole Moment

A molecular dipole moment is the overall dipole moment for the entire molecule. It is a measure of the molecule's overall polarity and takes into consideration the bond dipoles of all the bonds in the molecule and the molecular geometry. To determine the molecular dipole moment, all the individual bond dipole moments in the molecule should be summed up, considering both their magnitudes and directions. The total vector sum of these bond dipoles will give the molecular dipole moment. For some molecules, bond dipoles may cancel each other due to their geometry, resulting in a nonpolar molecule with a net dipole moment of zero.
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3. Distinction between Bond Dipole and Molecular Dipole Moments

The distinction between a bond dipole and a molecular dipole moment lies in the scope and focus of the concepts. A bond dipole moment refers specifically to the polarity of a single chemical bond between two atoms in a molecule, while a molecular dipole moment represents the overall polarity of the entire molecule. In summary, - Bond dipole moment: Polarity of a single chemical bond between two atoms within a molecule, it is primarily determined by the difference in electronegativity between these two atoms. - Molecular dipole moment: Overall polarity of the whole molecule, determined by summing up the bond dipole moments of all the individual bonds while taking into account the geometry of the molecule.

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Most popular questions from this chapter

Sulfur tetrafluoride \(\left(\mathrm{SF}_{4}\right)\) reacts slowly with \(\mathrm{O}_{2}\) to form sulfur tetrafluoride monoxide (OSF_ \(_{4} )\) according to the following unbalanced reaction: \begin{equation}\mathrm{SF}_{4}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{OSF}_{4}(g) \end{equation} The O atom and the four \(\mathrm{F}\) atoms in OSF \(_{4}\) are bonded to a central \(\mathrm{S}\) atom. (a) Balance the equation. (b) Write a Lewis structure of OSF_ in which the formal charges of all atoms are zero.(c) Use average bond enthalpies (Table 8.3 ) to estimate the enthalpy of the reaction. Is it endothermic or exothermic? (d) Determine the electron-domain geometry of \(\mathrm{OSF}_{4}\), and write two possible molecular geometries for the molecule based on this electron-domain geometry. (e) For each of the molecules you drew in part (d), state how many fluorines are equatorial and how many are axial.

(a) If the valence atomic orbitals of an atom are sp hybridized, how many unhybridized \(p\) orbitals remain in the valence shell? How many \(\pi\) bonds can the atom form? (b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single \(\sigma\) bond or around a double \((\sigma\) plust (rotate) around a single \(\sigma\) bond same?

(a) What is the difference between a localized \(\pi\) bond and a delocalized one? (b) How can you determine whether a molecule or ion will exhibit delocalized \(\pi\) bonding? (c) Is the \(\pi\) bond in \(\mathrm{NO}_{2}^{-}\) localized or delocalized?

Give the electron-domain and molecular geometries of a molecule that has the following electron domains on its central atom: (a) four bonding domains and no nonbonding domains, (b) three bonding domains and two nonbonding domains, (c) five bonding domains and one nonbonding domain, (d) four bonding domains and two nonbonding domains.

The Lewis structure for allene is Make a sketch of the structure of this molecule that is analogous to Figure \(9.25 .\) In addition, answer the following three questions: (a) Is the molecule planar? (b) Does it have a nonzero dipole moment? (c) Would the bonding in allene be described as delocalized? Explain.
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