The electronegativities of the -C≡CH and -C≡N groups are the same, but the dipole moments of...

The electronegativities of the -C≡CH and -C≡N groups are the same, but the dipole moments of the CH3C≡CH and the CH3C≡N are 0.78 D and 3.92 D, respectively. Explain why the dipole moments are so different.

Expert Solution

Electrons are shared by atoms while forming a bond. If the electrons are shared unequally, then it creats small equal and opposite charge difference on the atoms. Often, when two atoms with different electronegativity share the electrons unequally, they form this small charge difference and due to this dipole moment is created. Which is a result of more electronegative atom pulling the shared electrons towards itself.

In terminal alkyne C triple bond C, the electronegativity difference in the two carbons is not much. Whereas, in C triple bond N (nitrile group) the electronegativity difference is large and so it shares the electrons unequally. This creats difference is small charges on C and N. Additionally, nitrogen has loan pair of electrons which adds to the magnitude of dipolemoment in nitrile group. So the dipole moment in nitrile is more as compared to alkyne C triple bond C.

Electronegativity of alkyne overall is same as nitrile because the positive inductive effect of nitrogen is doesnot pass much after the first carbon.

queen_honey_blossom answered 2 years ago

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