Why are most organic compounds nonconducting and insoluble in water?
2 answers:
Explanation:
It is known that like dissolves like which means that polar substances are able to dissolve only in polar solvents.
Whereas non-polar substances are able to dissolve only in non-polar solvents.
As all organic compounds are non-polar in nature so, they are only soluble in non-polar solvents.
On the other hand, water is a polar solvent and its dissolves substances like NaCl, etc that are also polar in nature.
Also, for a solution to conduct electricity it is necessary that there must be flow of ions from one place to another. But a non-polar or organic substance do not dissociate into ions when dissolved in water.
Hence, it is unable to conduct electricity.
Thus, we can conclude that most organic compounds are non-conducting and insoluble in water because:
- Most organic compounds don't dissolve in water because they are nonpolar.
- They don't conduct electricity because they are covalent, not ionic.
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Answer:
Here's what I get
Explanation:
(a) Intermediates
The three structures below represent one contributor to the resonance-stabilized intermediate, in which the lone pair electrons on the heteroatom are participating (the + charge on the heteroatoms do not show up very well).
(b) Relative Stabilities
The relative stabilities decrease in the order shown.
N is more basic than O, so NH₂ is the best electron donating group (EDG) and will best stabilize the positive charge in the ring. However, the lone pair electrons on the N in acetanilide are also involved in resonance with the carbonyl group, so they are not as available for stabilization of the ring.
(c) Relative reactivities
The relative reactivities would be
C₆H₅-NH₂ > C₆H₅-OCH₃ > C₆H₅-NHCOCH₃
