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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

The \(\mathrm{O}-\mathrm{H}\) bond lengths in the water molecule \(\left(\mathrm{H}_{2} \mathrm{O}\right)\) are\(0.96 \mathrm{A},\) and the \(\mathrm{H}-\mathrm{O}-\mathrm{H}\) angle is \(104.5^{\circ} .\) The dipole moment of the water molecule is 1.85 \(\mathrm{D}\) . (a) In what directions do the bond dipoles of the \(\mathrm{O}-\mathrm{H}\) bonds point? In what direction does the dipole moment vector of the water molecule point? (b) Calculate the magnitude of the bond dipole-of the \(\mathrm{O}-\mathrm{H}\) bonds. (Note: You will need to use vector addition to do this. \((\mathbf{c})\) Compare your answer from part (b) to the dipole moments of the hydrogen halides (Table 8.3\() .\) Is your answer in accord with the relative electronegativity of oxygen?

(a) Is the molecule BF \(_{3}\) polar or nonpolar? (b) If you react BF \(_{3}\) to make the ion \(\mathrm{BF}_{3}^{2-}\) , is this ion planar? (c) Does the molecule BF\(_{2}\)Cl have a dipole moment?

In the formate ion, \(\mathrm{HCO}_{2}^{-}\) , the carbon atom is the central atom with the other three atoms attached to it. (a) Draw a Lewis structure for the formate ion. (b) What hybridization is exhibited by the C atom? (c) Are there multiple equivalent resonance structures for the ion? (d) How many electrons are in the \(\pi\) system of the ion?

Which of the following statements about hybrid orbitals is or are true? (i) After an atom undergoes sp hybridization, there is one unhybridized \(p\) orbital on the atom, (ii) Under \(s p^{2}\) hybridization, the large lobes point to the vertices of an equilateral triangle, and (iii) The angle between the large lobes of \(s p^{3}\) hybrids is \(109.5^{\circ} .\)

Consider the molecule \(\mathrm{BF}_{3}\). (a) What is the electron configuration of an isolated B atom? (b) What is the electron configuration of an isolated F atom? (c) What hybrid orbitals should be constructed on the B atom to make the B鈥揊 bonds in \(\mathrm{B} \mathrm{F}_{3}\)?(d) What valence orbitals, if any, remain unhybridized on the B atom in \(\mathrm{BF}_{3} ?\)
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