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

Vedclass · Answer

(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

Indicate the $\sigma$ and $\pi$ bonds in the following molecules:
$C_{6}H_{6}, C_{6}H_{12}, CH_{2}Cl_{2}, CH_{2}=C=CH_{2}, CH_{3}NO_{2}, HCONHCH_{3}$

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 $(CH_2=CH-CH=CH_2)$

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

Explain $\sigma$ and $\pi$ bonds,and mention the orbital overlapping involved in their formation.

According to the $VB$ theory,when is a bond not formed between two atoms? Give examples.

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