A pi-bond may be formed between two p_x-orbit | vedclass

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Question

(C) $\pi$-bond is formed by the lateral or side-by-side overlapping of atomic orbitals.For $p_x$-orbitals,the electron density is concentrated along t

Vedclass · Accepted Answer

$z$-axis

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(C) $\pi$-bond is formed by the lateral or side-by-side overlapping of atomic orbitals.For $p_x$-orbitals,the electron density is concentrated along the $x$-axis.If the orbitals approach along the $x$-axis,they undergo head-on overlapping,which results in the formation of a $\sigma$-bond.If the $p_x$-orbitals approach each other along the $y$-axis or $z$-axis,they will overlap laterally (side-by-side),resulting in the formation of a $\pi$-bond.Therefore,the correct axis for $\pi$-bond formation between $p_x$-orbitals is the $y$-axis or $z$-axis.

$A$ $\pi$-bond may be formed between two $p_x$-orbitals containing one unpaired electron each when they approach each other appropriately along:

Similar Questions

The number of sigma $(\sigma)$ and pi $(\pi)$ bonds present in benzene respectively are:

Determine the number of $\sigma$ and $\pi$ bonds in the following molecules:
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$(ii)$ $N_2$
$(iii)$ $C_6H_6$ (Benzene)
$(iv)$ $O_3$ (Ozone)

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

Which type of overlapping results in the formation of a $\pi$ bond?

Which type of bond is formed by the linear overlap of two hybrid orbitals,each containing one electron,associated with two different atoms?

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