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

$A$ carbon-carbon triple bond in ethyne $(HC \equiv CH)$ consists of:

Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in $C_2H_4$ and $C_2H_2$ molecules.

Which of the following statements is incorrect for sigma and $\pi$-bonds formed between two carbon atoms?

Assertion : Sigma $(\sigma)$ is a strong bond,while pi $(\pi)$ is a weak bond.
Reason : Atoms rotate freely about pi $(\pi)$ bond.

Which of the following combinations forms the strongest bond by head-on overlapping?

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