Fluoromethane (CH 3 F, µ=1.81 D) has a smaller dipole moment than chloromethane (CH 3 Cl, 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 -30 C.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 (CH 3 F, µ=1.81 D) has a smaller dipole moment than chloromethane (CH 3 Cl, µ=1.87 D) even though fluorine is more electronegative than chlorine.

Question

Draw the major producrs of this SN1 reaction. Ignore any inorganic byproducts. Use a dash or wedge bond to indicate the sereochemistry of substituents on asymmetric centers where appllicable.

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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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