In which of the following molecules are pi- e | vedclass

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(C) Delocalization of $\pi-$ electrons requires a conjugated system where $p-$ orbitals overlap across adjacent atoms.$1$. In the pyrrole cation,the n

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$H_2C=C=CH_2$

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(C) Delocalization of $\pi-$ electrons requires a conjugated system where $p-$ orbitals overlap across adjacent atoms.$1$. In the pyrrole cation,the nitrogen atom is part of a cyclic system with $4n+2$ $\pi-$ electrons,allowing for delocalization.$2$. In the anilinium ion $(C_6H_5NH_3^+)$,the $\pi-$ electrons within the benzene ring remain delocalized.$3$. In $H_2C=C=CH_2$ (allene),the central carbon is $sp$ hybridized. The two $\pi-$ bonds are perpendicular to each other,preventing continuous $p-$ orbital overlap across the entire molecule. Thus,the $\pi-$ electrons are localized in their respective $\pi-$ bonds.$4$. In the borirene derivative,the boron atom has an empty $p-$ orbital,which allows for delocalization of the $\pi-$ electrons from the double bond into the boron $p-$ orbital.Therefore,the molecule where $\pi-$ electrons are not delocalized across the entire system is allene $(H_2C=C=CH_2)$.

$Bond$	$E_{diss} (kJ \ mol^{-1})$
$C-A$	$240$
$C-B$	$328$
$C-C$	$276$
$C-D$	$485$

In which of the following molecules are $\pi-$ electrons not delocalized?

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The table shown below gives the bond dissociation energies $E_{diss}$ for single covalent bonds of carbon $C$ atoms with elements $A, B, C$ and $D.$ Which element has the smallest atoms?

$Bond$ $E_{diss} (kJ \ mol^{-1})$

$C-A$ $240$

$C-B$ $328$

$C-C$ $276$

$C-D$ $485$

Which of the following has the least covalent $P-H$ bond?

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