Answer
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Hint: In the trigonal planar arrangement, there is a central atom, bonded to three other atoms. These three other atoms are arranged like a triangle around the central atom, with a bond angle measuring ${ 120 }^{ \circ }{ C }$.
Complete step-by-step answer:
As we can see here that ${ CO }_{ 3 }^{ 2- }{ ,NO }_{ 3 }^{ - }{ ,SO }_{ 3 }$
has ${ sp }^{ 2 }$ and trigonal planar structure, so the correct option is B.
Additional Information:
-Hybridization is a process of mixing two or more atomic orbitals of an atom having comparable energy to form orbitals of equal energy known as hybrid orbitals.
-One s and three p orbitals of carbon mix/hybridize to give four ${ sp }^{ 3 }$ hybrid orbitals. The ${ sp }^{ 3 }$ hybrid orbitals are used by 4 hydrogen atoms for sigma bond formation.
-Trigonal planar is a subatomic geometry model with one molecule at the middle and three particles at the sides of a symmetrical triangle, called peripheral atoms, all in one plane.
- In an ideal trigonal planar species, every one of the three ligands are indistinguishable and all bond angles are ${ 120 }^{ \circ }{ C }$.
-When ${ sp }^{ 3 }$ orbitals are formed, they arrange themselves with the goal that they are as far separated as could be expected under the circumstances. That is a tetrahedral arrangement, with a point of ${ 109.5 }^{ \circ }{ C }$.
Note: The possibility to make a mistake is that you may choose option A. But in that ${ NCl }_{ 3 }$ is trigonal pyramidal, not trigonal planar due to the presence of lone pairs of electrons on nitrogen atoms.
Complete step-by-step answer:
As we can see here that ${ CO }_{ 3 }^{ 2- }{ ,NO }_{ 3 }^{ - }{ ,SO }_{ 3 }$
has ${ sp }^{ 2 }$ and trigonal planar structure, so the correct option is B.
Additional Information:
-Hybridization is a process of mixing two or more atomic orbitals of an atom having comparable energy to form orbitals of equal energy known as hybrid orbitals.
-One s and three p orbitals of carbon mix/hybridize to give four ${ sp }^{ 3 }$ hybrid orbitals. The ${ sp }^{ 3 }$ hybrid orbitals are used by 4 hydrogen atoms for sigma bond formation.
-Trigonal planar is a subatomic geometry model with one molecule at the middle and three particles at the sides of a symmetrical triangle, called peripheral atoms, all in one plane.
- In an ideal trigonal planar species, every one of the three ligands are indistinguishable and all bond angles are ${ 120 }^{ \circ }{ C }$.
-When ${ sp }^{ 3 }$ orbitals are formed, they arrange themselves with the goal that they are as far separated as could be expected under the circumstances. That is a tetrahedral arrangement, with a point of ${ 109.5 }^{ \circ }{ C }$.
Note: The possibility to make a mistake is that you may choose option A. But in that ${ NCl }_{ 3 }$ is trigonal pyramidal, not trigonal planar due to the presence of lone pairs of electrons on nitrogen atoms.