Considering the X-axis as the internuclear ax | vedclass

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(C) sigma $(\sigma)$ bond is formed by the head-on (axial) overlap of atomic orbitals along the internuclear axis.If the $X$-axis is the internuclear

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$2p_y$ and $2p_y$

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(C) sigma $(\sigma)$ bond is formed by the head-on (axial) overlap of atomic orbitals along the internuclear axis.If the $X$-axis is the internuclear axis,$2p_y$ orbitals (which are oriented along the $Y$-axis) are perpendicular to the internuclear axis.Their lateral (sideways) overlap results in the formation of a pi $(\pi)$ bond,not a sigma $(\sigma)$ bond.On the other hand,$s-s$ and $s-p_x$ overlaps along the $X$-axis are axial and form $\sigma$ bonds.

Considering the $X$-axis as the internuclear axis,which of the following will not form a sigma $(\sigma)$ bond and why?

Similar Questions

Which of the following would result in the formation of the strongest $\pi-$ bond if the molecular axis is the $x-$axis?

The total number of sigma $(\sigma)$ and pi $(\pi)$ bonds in an ethylene molecule are

Which of the following is correct for the $N_2$ triple bond?

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

How many $\sigma$ and $\pi$ bonds are present in each of the following molecules?
$(a)$ $HC \equiv C-CH=CH-CH_3$
$(b)$ $CH_2=C=CH-CH_3$

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