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(B) The strength of a covalent bond depends on the extent of overlapping of atomic orbitals. Axial overlapping is always stronger than sidewise overla

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$p-p$ (axial)

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(B) The strength of a covalent bond depends on the extent of overlapping of atomic orbitals. Axial overlapping is always stronger than sidewise overlapping. Among axial overlaps,the $p-p$ (axial) overlap is stronger than $s-p$ and $s-s$ overlaps because $p-$orbitals are more directional in nature,allowing for a greater extent of overlap compared to the spherical $s-$orbitals.

Which overlap results in the formation of the strongest bond?

Similar Questions

Which of the following statements is $NOT$ correct?

Which of the following combinations does not form a $\sigma$ bond?
$(i) \ 2p_y - 2p_y$
$(ii) \ 2p_z - 2p_z$
$(iii) \ 2s - 2p_x$
$(iv) \ 2p_x - 2p_x$

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

The ratio of the number of $\sigma$ and $\pi$ bonds in benzene is equal to:

The nodal plane in an ethylene $(C_2H_4)$ molecule is:

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