What is the type of chemical covalent bond be | vedclass

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(A) In $C_2H_4$ (ethene),each carbon atom is $sp^2$ hybridized.The carbon-carbon double bond consists of one $\sigma$ bond and one $\pi$ bond.The $\si

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$sp^2-sp^2$ $\sigma$ bond,$2p\pi -2p\pi$ bond

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(A) In $C_2H_4$ (ethene),each carbon atom is $sp^2$ hybridized.The carbon-carbon double bond consists of one $\sigma$ bond and one $\pi$ bond.The $\sigma$ bond is formed by the head-on overlap of $sp^2$ hybrid orbitals from each carbon atom,denoted as $sp^2-sp^2$ $\sigma$ bond.The $\pi$ bond is formed by the lateral (sideways) overlap of the unhybridized $2p$ orbitals on each carbon atom,denoted as $2p\pi -2p\pi$ bond.

List-$I$	List-$II$
$(1)$ $SF_4$	$(A)$ $sp^3d^2$
$(2)$ $IF_5$	$(B)$ $d^2sp^3$
$(3)$ $NO_2^+$	$(C)$ $sp^3d$
$(4)$ $NH_4^+$	$(D)$ $sp^3$
	$(E)$ $sp$

What is the type of chemical covalent bond between the carbon-carbon atoms in $C_2H_4$?

Similar Questions

Which one of the following has the maximum number of hybrid orbitals?

Match the species in List-$I$ with their correct hybrid orbitals in List-$II$.

List-$I$ List-$II$

$(1)$ $SF_4$ $(A)$ $sp^3d^2$

$(2)$ $IF_5$ $(B)$ $d^2sp^3$

$(3)$ $NO_2^+$ $(C)$ $sp^3d$

$(4)$ $NH_4^+$ $(D)$ $sp^3$

$(E)$ $sp$

The structure of $IF_{7}$ is

The hybridisations of the atomic orbitals of nitrogen in $NO_{2}^{-}$,$NO_{2}^{+}$ and $NH_{4}^{+}$ respectively are.

What is the hybridization of $Xe$ in $XeF_2$?

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