Hybridisition of So2
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Tge hybridization of SO2 is SP2
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Sulphur dioxide is SO2
The central sulphur atom is bonded to two oxygen atoms. The structure is like this: O=S=O
The sulphur atom forms one sigma and one pi bond with each oxygen atom and has one lone pair.
Sulphur in its ground state has first two shells completely filled and six electrons in the outermost shell. There are two paired electrons in the 3s orbital and four electrons in 3p orbital (Two paired electrons in 3px orbital and one unpaired electron each in 3py and 3pz orbitals). In order to form four bonds, it needs four unpaired electrons. Therefore, the formation of the excited state takes place: One 3px electron shifts to an empty 3d orbital. Now, there are four unpaired electrons (Three unpaired electrons in three 3p orbitals and one unpaired electron in one 3d orbital).
As the electrons forming sigma bonds (and the lone pair) need to be on the same energy level, hybridisation takes place. One 3s and two 3p orbitals get hybridised to form three equal sp2 hybrid orbitals. One hybrid orbital is occupied by the lone pair and other two orbitals have unpaired electrons, which participate in sigma bonding with the oxygen atoms. The remaining 3p and 3d orbitals remain unhybridised. The two unpaired electrons in the unhybridised orbitals take part in the formation of pi bonds.
Therefore, the hybridisation of the central sulphur atom in this compound is sp2.
P.S. The hybridisation of the two oxygen atoms is sp2 as well.
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Sulphur dioxide is SO2
The central sulphur atom is bonded to two oxygen atoms. The structure is like this: O=S=O
The sulphur atom forms one sigma and one pi bond with each oxygen atom and has one lone pair.
Sulphur in its ground state has first two shells completely filled and six electrons in the outermost shell. There are two paired electrons in the 3s orbital and four electrons in 3p orbital (Two paired electrons in 3px orbital and one unpaired electron each in 3py and 3pz orbitals). In order to form four bonds, it needs four unpaired electrons. Therefore, the formation of the excited state takes place: One 3px electron shifts to an empty 3d orbital. Now, there are four unpaired electrons (Three unpaired electrons in three 3p orbitals and one unpaired electron in one 3d orbital).
As the electrons forming sigma bonds (and the lone pair) need to be on the same energy level, hybridisation takes place. One 3s and two 3p orbitals get hybridised to form three equal sp2 hybrid orbitals. One hybrid orbital is occupied by the lone pair and other two orbitals have unpaired electrons, which participate in sigma bonding with the oxygen atoms. The remaining 3p and 3d orbitals remain unhybridised. The two unpaired electrons in the unhybridised orbitals take part in the formation of pi bonds.
Therefore, the hybridisation of the central sulphur atom in this compound is sp2.
P.S. The hybridisation of the two oxygen atoms is sp2 as well.
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