Which of the following molecules has a centra | vedclass

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(B) To determine the hybridization of the central atom,we use the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is the number of valence electro

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$SO_2$

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(B) To determine the hybridization of the central atom,we use the formula: $H = \frac{1}{2}(V + M - C + A)$,where $V$ is the number of valence electrons,$M$ is the number of monovalent atoms,$C$ is the cationic charge,and $A$ is the anionic charge.For $CO_2$: $H = \frac{1}{2}(4 + 0) = 2$ ($sp$ hybridization).For $SO_2$: The central $S$ atom has $6$ valence electrons. It forms two double bonds with $O$ atoms and has one lone pair. $H = \frac{1}{2}(6 + 0) = 3$ ($sp^2$ hybridization).For $N_2O$: The central $N$ atom is $sp$ hybridized.For $CO$: The central $C$ atom is $sp$ hybridized.Thus,$SO_2$ is the correct answer.

List-$I$	List-$II$
$(a)$ $SF_6$	$(i)$ $sp^3d^2$
$(b)$ $PCl_5$	(ii) $sp^3d$
$(c)$ $XeF_4$	(iii) $sp^3d^3$
$(d)$ $IF_7$	(iv) $sp^3d^2$

Which of the following molecules has a central atom with $sp^2$ hybridization?

Similar Questions

Which bonds are formed by a carbon atom with $sp^{2}$-hybridisation?

Which of the following statements are true about the $S_8$ molecule?
$I.$ There are no $p_{\pi}-p_{\pi}$ bonds present in the molecule.
$II.$ There are eight lone pairs of electrons in total.
$III.$ Each $S$ atom is $sp^3$ hybridized.

Match the following:
List-$I$ List-$II$
$(a)$ $SF_6$ $(i)$ $sp^3d^2$
$(b)$ $PCl_5$ (ii) $sp^3d$
$(c)$ $XeF_4$ (iii) $sp^3d^3$
$(d)$ $IF_7$ (iv) $sp^3d^2$

The correct answer is:

The type of hybrid orbitals used by the chlorine atom in $ClO_2^-$ is

The states of hybridization of boron and oxygen atoms in boric acid $(H_3BO_3)$ are respectively

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