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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 relationship to molecular polarity. A bond dipole refers to the separation of charges within a single chemical bond due to differences in electronegativity between two atoms, while a molecular dipole moment is the vector sum of all the bond dipoles in a molecule, representing the overall polarity of the molecule. The presence of bond dipoles does not necessarily guarantee a molecular dipole moment, as bond dipoles can cancel each other out if they have opposite directions and equal magnitudes.

Step by step solution

01

Definition of Bond Dipole

A bond dipole occurs when there is a separation of charges between two atoms within a chemical bond. This is due to the difference in electronegativity between the two atoms. The more electronegative atom attracts the shared electrons, creating a partially negative charge on that atom, and leaving the other atom with a partially positive charge. The bond dipole is represented by an arrow pointing towards the more electronegative atom, with a cross at the tail representing the positive charge.
02

Definition of Molecular Dipole Moment

The molecular dipole moment is the vector sum of all the bond dipoles in a molecule. It represents the overall polarity of the molecule, accounting for the magnitude and direction of all bond dipoles. The molecular dipole moment is expressed in Debye units (D). A molecule with a net molecular dipole moment is said to be polar, whereas a molecule with no net molecular dipole moment (i.e., the bond dipoles cancel each other out) is considered nonpolar.
03

Comparing Bond Dipole and Molecular Dipole Moment

The distinction between bond dipole and molecular dipole moment lies in their scope and relationship to molecular polarity. A bond dipole considers the separation of charges within a single bond, while a molecular dipole moment takes into account the polarity of the entire molecule, accounting for the impact of all bond dipoles. It is important to note that the presence of bond dipoles does not necessarily guarantee a molecular dipole moment, as bond dipoles can cancel each other out if they have opposite directions and equal magnitudes.

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Most popular questions from this chapter

For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. (b) The greater the orbital overlap in a bond, the shorter the bond. \((\mathbf{c})\) To create a hybrid orbital, you could use the \(s\) orbital For each statement, indicate whether it is true or false. (a) The greater the orbital overlap in a bond, the weaker the bond. (b) The greater the orbital overlap in a bond, the shorter the bond. \((\mathbf{c})\) To create a hybrid orbital, you could use the \(s\) orbital

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