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

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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 t

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$z$-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:

Which one is stronger,$\sigma$ bond or $\pi$ bond? Why?

The strongest bond is formed when atomic orbitals undergo:

Considering the $x$-axis as the internuclear axis,which of the following will not form a sigma $(\sigma)$ bond and why?
$(a)$ $1s$ and $1s$
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Number of $\sigma$ and $\pi$ bonds present in $CH_3-CH=CH-C\equiv CH$ are

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