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all aromatic compounds have 1) delocalized pi electrons (usually in conjugated double bonds) 2) 4n+2 pi electrons to be shared on adjacent atoms... this is "Huckles" rule 3) a planar structure 4) rings.. aromatic compounds are cyclic
You can think of pi bonds in the terms of pi electrons as well which will become more important in terms of aromaticity. A Triple bond has 1 sigma bond & 2 pi bonds. There are 6 electrons in a triple bond; 2 sigma electrons and 4 pi electrons. The two unhybridized p orbitals on each atom on either side of the triple bond are perpendicular to each other. So, if you are trying to determine the number of pi electrons in an aromatic monocyclic compound and you have an uninterrupted combination of sp & sp2 orbitals (sp3 does not have p orbitals), whenever you come across a triple bond you would add 4 pi electrons and for a double bond you would add 2 pi electrons. The important thing to remember though is if the question asks for the number of electrons delocalized in the ring because of the aforementioned p orbitals in a triple bond being perpendicular only 2 of the 4 available pi electrons would delocalize in the ring. The really dirty trick is that Huckel's rule applies to electrons in the cloud, delocalized electrons.
Aromatic compounds, conjugated dienes, and compounds with extensive pi-electron systems often show UV absorption bands. These compounds have delocalized electrons that can undergo electronic transitions when exposed to ultraviolet light, leading to absorption of UV radiation.
Alkyl groups are electron donating because they have a lower electronegativity than the atoms in the pi system (such as carbon or nitrogen). The alkyl group donates electron density to the pi system through its sigma bonds, thereby increasing the electron density in the pi system. This electron donation stabilizes the pi system and can affect its reactivity.
pH has a vital role in formation of coacervates. pH changes the surface charge of the polymer in its solution. When two types of charges are present in the solution, the environment prefers binding and crosslinking. When this sort of aggregation develops, we see droplets of coacervates in the system. now How pH changes the surface charge density? The total charge of the polymer solution(system) is zero at its pI or isoelectric point which is fixed for a particular polyampholytic polymer like gelatin. However no pI exists for purely anionic and purely cationic polymers. For example, Agar is a polyanionic polymer. When the pH of solution is less than the PI, the positive charges get dominated over it and vice versa. These charges affect the binding property in the system and hence the coacervate formation. Answered by Shilpi Boral.
yes
Benzene has covalent bonds. Each of the six carbons in benzene is sp2 hybridized meaning the ring has both sigma bonds and pi bonds. Benzene is aromatic meaning its pi electrons are delocalized and form a pi system.
No, in aromatic compounds and some aliphatic compounds have deloclized pi bonds but in most of the alkenes and alkynes there are localized pi bonds.
Benzene has a property called resonance. Because of this, the three pi-bonds in benzene act as a rather delocalized single pi-structure. So, benzene does not actually have 3 distinct pi-bonds. This pi-structure is stable, which explains why benzene is more stable than it would be if it had 3 pi-bonds.
Electrons in SIGMA bonds remain localized between two atoms, Electrons in PI bonds can become delocalized between more than two atoms?
KMnO4 will add across the double bond of alkenes (or alkynes) resulting in the docolouring of KMnO4 but not an alkane such as ethane.
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all aromatic compounds have 1) delocalized pi electrons (usually in conjugated double bonds) 2) 4n+2 pi electrons to be shared on adjacent atoms... this is "Huckles" rule 3) a planar structure 4) rings.. aromatic compounds are cyclic
all aromatic compounds have 1) delocalized pi electrons (usually in conjugated double bonds) 2) 4n+2 pi electrons to be shared on adjacent atoms... this is "Huckles" rule 3) a planar structure 4) rings.. aromatic compounds are cyclic
one sigma and one and half pi bonds