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This is due to the resonation process that gives the allusion of all bond lengths being equal. In fact the bonds are in a state of constant flux and 'blend' into one. It is much like the apperance of a helicopters rotar blades i.e. in flight it appears as a blurr but whilst stationary it is clear that there are simply two blades
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The paragraph above is incorrect. Forget the fan blade and helicopter rotor analogies for resonance. There is NO evidence that bonds are jumping back and forth between a single bond and a double bond. That's just wrong. Resonance structures are simply an attempt at representing with Lewis structures something which really can't be represented with Lewis structures, that of a "partial" double bond.
In carbonate ion, all of the carbon-oxygen bonds are identical, and have a length somewhere between that of a single bond and a double bond. The bond order for the carbon-oxygen bond in carbonate is 1.33. The partial double bond comes from delocalized pi bonding.
In addition to the single bond between the central carbon and each oxygen, there is a delocalized pi bond between the central carbon and each of the oxygen atoms. There is overlap of the p-orbital on C with each of the p-orbitals on the oxygen atoms, but there are not enough electrons for three double bonds. It is this additional pi bonding which makes each of the carbon-oxygen bonds have a bond order of 1.33, and a bond length and bond strength between those of single and double carbon-oxygen bonds. ----- Pisgahchemist
What else can I help you with?
Draw resonance structure of benzene?
I can't draw images, but I can describe it. The resonance structure of benzene involves a delocalized ring of six carbons with alternating single and double bonds. The structure shows two resonance forms with the double bonds shifting around the ring to maintain stability and equal bond lengths.
Why does bromine react with hexene but not benzene?
Adding halogens to alkene groups (X2) requires that the product adopt an anti configuration. Hexene will also lose its double bond upon bromination. Benzene is energetically unfavorable when a reaction attempts to break its double bond. The resonance benzene has makes it very stable, and thus very hard to break.
How many resonance structure benzene have?
Benzene has two resonance structures. In the resonance hybrid, each carbon-carbon bond is a hybrid of a single bond and a double bond, resulting in a delocalized pi electron system. This delocalization gives benzene its unique stability and reactivity compared to typical alkenes.
Why are the bond lengths in no3- all identical and shorter than a nitrogen-oxygen single bond?
NO3- has three resonance structure. One double bond between N and O and another two N - O single bond. Since the double bond can be formed between N and any other O it is said that it has a resonance structure. This means that the true structure of NO3- is not any of this structure, but rather a hybrid of all three. Hence all 3 bond lengths would be identical AND shorter than single bond as it is basically an average between single and double bond. It is of course longer than a double bond
How many carbon atoms are there in the molecule hexane?
There are no double bonds in benzene. In a benzene molecule, every carbon is attached to another two carbon atoms and to a hydrogen atom. Then there is a free p-orbital to every carbon atom. All of these over lap to form delocalized orbitals. It is experimentally proved that C-C bond distance in benzene are all the same and liebetween the actual lengths of a C-C bond and a C=C bond. In the valence bond description of bonding there is resonance between two principal forms, each has 3 double bonds. The net effect of the resonance is very similar to the molecular orbital approach above.
Which compound contains a longer C-C bond benzene or ethene?
c-c bond length in benzene is 1.397 angston and that of ethene is 1.34 angston structure of benzene is a resonance hybrid, therefore all the c-c bond lengths are equal but different from those in alkanes,alkenes, and alkynes.
Why single and double bond length are same in benzene?
In reality, benzene does not contain alternating single and double bonds. It is more accurate to say that each carbon-carbon bond is in an intermediate state between a single and a double bond. Benzene therefore displays a property known as resonance.
Why is the circle with in a hexagon representation of a benzene molecule a better model than a hexagon with alternating double bonds?
The circle in a hexagon representation of a benzene molecule is a better model because it accurately represents the delocalized pi electrons in the benzene ring. This model explains the equal bond lengths and alternating single and double bonds seen in benzene ring, while the hexagon with alternating double bonds model implies unequal bond lengths and instability that contradict experimental observations.
Why c c bonds in benzene are intermediate in length between single and double c c bonds?
Because in benzene molecule the pi electrons are delocalized (continuously changing their position within the hexagonal ring), so there are no fixed single and double bonds but are in mid of single and double bond character.
Are all C-C bond distances the same in C6H6?
No, in benzene (C6H6), the C-C bond distances are not all the same. Benzene exhibits a hexagonal structure with alternating shorter and longer C-C bond lengths due to resonance delocalization of electrons in the π system.
Why c-c bond are equal in benzene due to resonance?
In benzene, the delocalization of electrons in the pi system creates a symmetric charge distribution around the ring, resulting in equal sharing of electron density between all carbon atoms. This leads to the concept of resonance, where the actual molecule is a hybrid of different resonance structures. As a result, the carbon-carbon bonds in benzene are equivalent and have partial double bond character.
Why in benzene c-c bond lengths is same?
In benzene, the carbon-carbon bond lengths are the same because of resonance. The pi electrons are delocalized throughout the ring structure, resulting in a continuous ring of electron density, which contributes to the stability of the molecule. This delocalization leads to a partial double bond character for all the C-C bonds in the ring, making them equivalent in length.
What is the bond order for the benzene molecule?
The bond order for the benzene molecule is 1.5. Benzene is a resonance hybrid of two possible structures, each involving alternating single and double bonds. This creates a partial double bond character for all the carbon-carbon bonds in benzene, resulting in a bond order of 1.5.
What is the unit used to define bond lengths?
Bond lengths are typically expressed in units of picometers (pm) or angstroms (Å), where 1 Å is equal to 100 pm. Bond lengths are a measure of the distance between the nuclei of two bonded atoms in a molecule.
Why does hydrogenation have no effect on benzene?
If you could add a pair of hydrogen ions to any double bond of the benzene ring it would not be benzene anymore, on the one hand.
Draw resonance structure of benzene?
I can't draw images, but I can describe it. The resonance structure of benzene involves a delocalized ring of six carbons with alternating single and double bonds. The structure shows two resonance forms with the double bonds shifting around the ring to maintain stability and equal bond lengths.
Why does bromine react with hexene but not benzene?
Adding halogens to alkene groups (X2) requires that the product adopt an anti configuration. Hexene will also lose its double bond upon bromination. Benzene is energetically unfavorable when a reaction attempts to break its double bond. The resonance benzene has makes it very stable, and thus very hard to break.
