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(D) In a diatomic molecule,if the internuclear axis is the $z$-axis,then the $p_z$ orbitals undergo head-on overlap to form a $\sigma$ bond. The $p_x$

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no bond formation

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(D) In a diatomic molecule,if the internuclear axis is the $z$-axis,then the $p_z$ orbitals undergo head-on overlap to form a $\sigma$ bond. The $p_x$ and $p_y$ orbitals are oriented perpendicular to the $z$-axis. Since $p_x$ and $p_y$ orbitals are orthogonal to each other and to the $z$-axis,they cannot overlap effectively to form a bond. Therefore,the overlap of $p_x$ and $p_y$ orbitals results in no bond formation.

If the internuclear axis of a diatomic molecule is $z$,then the overlap of $p_x$ and $p_y$ orbitals results in the formation of ........

Similar Questions

If the internuclear axis is $z$,then which of the following overlapping gives a $\sigma$ bond?

Which of the following orbital overlaps leads to bonding?

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

In which of the following ions is $p\pi - d\pi$ overlap present?

In a $\sigma$ bond,

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