Organic Chemistry
9th Edition
ISBN: 9781305080485
Author: John E. McMurry
Publisher: Cengage Learning
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Chapter 2.SE, Problem 33AP
Interpretation Introduction
Interpretation:
Fluoromethane (CH3F, µ=1.81 D) has a smaller dipole moment than chloromethane (CH3Cl, µ=1.87 D) even though fluorine is more electronegative than chlorine. This observation is to be explained.
Dipole moment is defined as, µ=Qxr
Where, Q=Magnitude of the charge developed at either end of the dipole.
R=The distance between the charges
It is expressed in Debyes (D). 1 D=3.336x10-30C.m.
Thus dipole moment values depend not only on the magnitude of charges developed on the dipole but also on the length of the bond.
To explain:
Why fluoromethane (CH3F, µ=1.81 D) has a smaller dipole moment than chloromethane (CH3Cl, µ=1.87 D) even though fluorine is more electronegative than chlorine.
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