Question

Which bond in Figure P5.45 has $\mu=0 ?$

   Which bond in Figure P5.45 has $\mu=0 ?$

Chemistry: An Atoms-Focused Approach

Chemistry: An Atoms-Focused Approach

Thomas R. Gilbert,… 2nd Edition

Chapter 5, Problem 46

Instant Answer

Solved by Expert David Collins

09/08/2020

Step 1

A dipole moment, denoted by $\mu$, is a measure of the polarity of a chemical bond within a molecule. It arises from the difference in electronegativity between the two atoms involved in the bond. If the atoms have the same electronegativity, the bond is nonpolar Show more…

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Which bond in Figure P5.45 has $\mu=0 ?$

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Key Concepts

Dipole Moment

The dipole moment quantifies the separation of positive and negative charges in a bond. A bond with zero dipole moment indicates that there is no net separation of charge, meaning any individual bond dipoles (if present) are either absent or cancel out due to symmetry.

Molecular Symmetry

Molecular symmetry involves the spatial arrangement of atoms within a molecule. Even if some bonds within the molecule are polar, the overall dipole moment can be zero if the molecular geometry allows the individual bond dipoles to cancel each other out.

Bond Polarity

Bond polarity is based on the difference in electronegativity between two bonded atoms. When the electronegativity values are similar or identical, the electrons are distributed nearly equally between the atoms, resulting in a nonpolar bond with a dipole moment of zero.

Electronegativity

Electronegativity is the measure of an atom's ability to attract shared electrons in a bond. If two bonded atoms have the same or nearly the same electronegativity, the bond will have no distinct dipole as there is no significant charge separation.

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