A molecule (X) has (i) four sigma bonds forme | vedclass

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(D) In ethene $(C_2H_4)$,each carbon atom is $sp^2$ hybridized.Each carbon atom forms two $\sigma$ bonds with hydrogen atoms by the overlap of $sp^2$

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$C_2H_4$

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(D) In ethene $(C_2H_4)$,each carbon atom is $sp^2$ hybridized.Each carbon atom forms two $\sigma$ bonds with hydrogen atoms by the overlap of $sp^2$ and $s$ orbitals. Since there are two carbon atoms,there are $2 	imes 2 = 4$ such $\sigma$ bonds.The two carbon atoms are bonded to each other by a $\sigma$ bond formed by the overlap of $sp^2$ and $sp^2$ orbitals.Additionally,the unhybridized $p_z$ orbitals of the two carbon atoms overlap laterally to form one $\pi$ bond.Thus,the molecule $(X)$ is $C_2H_4$.

$A$ molecule $(X)$ has $(i)$ four sigma bonds formed by the overlap of $sp^2$ and $s$ orbitals,(ii) one sigma bond formed by $sp^2$ and $sp^2$ orbitals,and (iii) one $\pi$ bond formed by $p_z$ and $p_z$ orbitals. Which of the following is $X$?

Similar Questions

Which of the following orbital combinations form a sigma $(\sigma)$ bond? $1s-1s, 2s-2s, 1s-2s, 2p_x-2p_x, 2p_y-2p_y, 2p_z-2p_z$.

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

Where is the nodal plane of the $\pi$-bond in ethene located?

Considering the $x$-axis as the internuclear axis,which of the following will not form a sigma $(\sigma)$ bond and why?
$(a)$ $1s$ and $1s$
$(b)$ $1s$ and $2p_{x}$
$(c)$ $2p_{y}$ and $2p_{y}$
$(d)$ $1s$ and $2s$

How and when is a $\pi$-bond formed by the overlapping of orbitals?

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