In the thiocyanate ion, $${\text{SC}}{{\text{N}}^ - }$$ , three resonance structures are consistent with the electron-dot method. Structure A has only one negative formal charge on the nitrogen atom, the most electron negative atom in the ion. Structure B has a single negative charge on the S, which is less electronegative than N. Structure C has charges of −2 on N and +1 on S, consistent with the relative electronegativities of the atom s but with a larger charger and greater charge separation than the first.Predict the hybridization of an atom which is bonded with H in the structure of $${\text{HNCS}}$$ .\n \n \n \n \n A.$${\text{sp}}$$B.$${\text{s}}{{\text{p}}^2}$$C.$${\text{s}}{{\text{p}}^3}$$D.No hybridization

Question

In the thiocyanate ion, $${\text{SC}}{{\text{N}}^ - }$$ , three resonance structures are consistent with the electron-dot method. Structure A has only one negative formal charge on the nitrogen atom, the most electron negative atom in the ion. Structure B has a single negative charge on the S, which is less electronegative than N. Structure C has charges of −2 on N and +1 on S, consistent with the relative electronegativities of the atom s but with a larger charger and greater charge separation than the first.Predict the hybridization of an atom which is bonded with H in the structure of $${\text{HNCS}}$$ .\n    \n    \n    \n    \n  A.$${\text{sp}}$$B.$${\text{s}}{{\text{p}}^2}$$C.$${\text{s}}{{\text{p}}^3}$$D.No hybridization

Vedantu Content Team · Accepted Answer

Hint: If the hydrogen gets attached to the double bond then the hybridisation will be $${\text{s}}{{\text{p}}^2}$$ hybridisation. If the hydrogen gets attached to an atom which is under resonance then also the hybridisation of that atom will be $${\text{s}}{{\text{p}}^2}$$ .Complete step-by-step answer:Hydrogen has the atomic number 1. It requires one more electron to complete its out electronic configuration. So it will attach to that carbon which is electron rich and has more electron density in order to gain stability.\n    \n    \n    \n    \n  In case A as we can see that nitrogen has a negative charge and sulphur has only lone pair of electron. A negative charge has more tendencies to donate electron and hence the hydrogen will attach to the nitrogen instead of sulphur. The valency of carbon is satisfied and hence hydrogen will not attach there. Also the nitrogen is attached with double bond and hence the hybridisation will be $${\text{s}}{{\text{p}}^2}$$ .\n    \n    \n    \n    \n  In case B the hydrogen will attach to the sulphur due to the presence of negative charge. As we can see that lone pair is in resonance with the double bond. So the hybridisation will also be $${\text{s}}{{\text{p}}^2}$$ .\n    \n    \n    \n    \n  In case C, sulphur has a positive charge and hence can never attract hydrogen. The hydrogen will go towards the nitrogen. The nitrogen has adjacent pi bonds and has lone pairs of electrons too. The nitrogen is in resonance and so the hybridisation will be $${\text{s}}{{\text{p}}^2}$$ . Thus, the correct option is B.Note:When a single Lewis structure cannot explain all the properties of an element then we have to draw various structures to explain all the properties. These various structures are known as resonating structures.

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