The nodal plane in the pi-bond of ethene is l | vedclass

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(A) In ethene $(C_2H_4)$,the carbon atoms are $sp^2$ hybridized. The three $sp^2$ hybrid orbitals of each carbon atom lie in the same plane (the molec

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the molecular plane

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(A) In ethene $(C_2H_4)$,the carbon atoms are $sp^2$ hybridized. The three $sp^2$ hybrid orbitals of each carbon atom lie in the same plane (the molecular plane) and form $\sigma$ bonds with hydrogen atoms and the other carbon atom.The unhybridized $p_z$ orbitals are perpendicular to this molecular plane and overlap laterally to form the $\pi$ bond.$A$ nodal plane is a plane where the probability of finding an electron is zero.For a $\pi$ bond formed by the lateral overlap of $p$ orbitals,the molecular plane itself acts as the nodal plane because the electron density of the $\pi$ bond is concentrated above and below this plane,not within it.

The nodal plane in the $\pi-$bond of ethene is located in

Similar Questions

Which of the following statements is $NOT$ true regarding the sigma and pi bonds formed between two carbon atoms?

Calculate the ratio of $\sigma$ and $\pi$ bonds for the following compounds and determine the correct order:
$A$: Tetracyanomethane $(C(CN)_4)$
$B$: Carbon dioxide $(CO_2)$
$C$: Benzene $(C_6H_6)$
$D$: $1, 3$-Butadiene $(CH_2=CH-CH=CH_2)$

In an acetylene molecule,the bond between the carbon atoms consists of:

State the differences between sigma $(\sigma)$ and pi $(\pi)$ bonds.

In a $\sigma$ bond,

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