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The 31 pages that link to Pi bond, each with the reason it gives.

• AromaticityRelated: Its electrons contribute to the delocalized circuits used in aromaticity tests.

• AlkeneBroader topic: The alkene double bond contains a pi bond that reacts more readily than its sigma bond.

• Carbonyl groupRelated: Its second bond component gives C=O the geometry and reactivity of a double bond.

• Conjugated systemBroader topic: Its p orbitals overlap along a conjugated chain, spreading π electrons across multiple atoms.

• Cis–trans isomerismBroader topic: Breaking its orbital overlap is required for unrestricted rotation around an alkene double bond.

• ChromophoreBroader topic: Pi electrons in many chromophores participate in light-driven electronic transitions.

• Nucleophilic additionRelated: The pi component of the multiple bond is displaced as the new sigma bond forms.

• Electrophilic additionBroader topic: Its exposed electron density makes it more accessible to electrophiles than a sigma bond.

• AlkyneRelated: Two pi bonds accompany the sigma bond in an alkyne’s triple bond.

• Sigma bondCompared with: Unlike sigma bonds, pi bonds restrict rotation and accompany a sigma bond in multiple bonds.

• Carbon–carbon bondBroader topic: Double and triple carbon–carbon bonds add one or two pi bonds.

• Geometric isomerismRelated: Rotating an alkene would disrupt the pi bond and requires substantial energy.

• HyperconjugationCompared with: Its delocalization with adjacent pi bonds is ordinary conjugation, distinct from sigma donation.

• Aromatic compoundRelated: Overlapping p orbitals create the π system that can delocalize around a ring.

• PyrroleRelated: Delocalized π bonding connects pyrrole’s ring atoms and contributes to its aromatic character.

• Electrocyclic reactionRelated: The reaction reorganizes π bonding as a new σ bond forms or disappears.

• EtheneBroader topic: Its π bond makes ethene's double bond reactive toward addition.

• CycloadditionNarrower topic: Cycloaddition reorganizes π bonds as new σ bonds form.

• p orbitalRelated: Side-on overlap between p orbitals is the usual source of a π bond.

• FuranRelated: Delocalized π bonding gives furan its aromatic character.

• sp² hybridizationRelated: The remaining unhybridized p orbital can overlap sideways to create this bond.

• CyclobutadieneRelated: Each carbon contributes a p orbital whose overlap builds the ring’s π system.

• Cyclopentadienyl anionRelated: The ring’s conjugated π system arises from overlapping p orbitals.

• Aromatic hydrocarbonRelated: Overlapping p orbitals form the π system responsible for delocalization.

• Addition reactionRelated: Addition commonly replaces a π bond with two new sigma bonds.

• Double bondRelated: The second electron pair in a typical double bond forms this bond.

• AntiaromaticityRelated: π bonds supply the electrons counted when assessing antiaromaticity.

• Triple bondRelated: The two additional components of a triple bond are pi bonds.

• CyclopropeneRelated: The carbon–carbon double bond contains a pi component constrained by the small ring.

• PropadieneBroader topic: Each of propadiene’s two carbon–carbon double bonds contains a pi bond.

• Double bond ruleBroader topic: Weak sideways overlap is the rule’s central explanation for unstable heavier-element multiple bonds.