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Which one of the following statements is correct?
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The correct answer is:
Lateral overlap of $p$-orbitals or $p$ - and $d$-orbitals produces $\pi$-bonds
(a) Hybridised orbitals show only head on overlapping and thus form only $\sigma$ bonds. They never form $\pi$ bonds.
(c) Head on overlapping is stronger than lateral or sideways overlapping. Therefore, the strength of bonds follows the order
$$
\underbrace{\pi_{\rho-p}}_{\begin{array}{c}
\text { lateral } \\
\text { overlapping }
\end{array}} < \underbrace{\sigma_{s-s} < \sigma_{s-p} < \sigma_{\rho-p}}_{\text {head on overlapping of same shell }}
$$
(d) s-orbitals are spherically symmetrical and thus show only head on overlapping and form only $\sigma$ bonds.
(c) Head on overlapping is stronger than lateral or sideways overlapping. Therefore, the strength of bonds follows the order
$$
\underbrace{\pi_{\rho-p}}_{\begin{array}{c}
\text { lateral } \\
\text { overlapping }
\end{array}} < \underbrace{\sigma_{s-s} < \sigma_{s-p} < \sigma_{\rho-p}}_{\text {head on overlapping of same shell }}
$$
(d) s-orbitals are spherically symmetrical and thus show only head on overlapping and form only $\sigma$ bonds.
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