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Question: The ion \[CIF_{2}^{-}~\] is linear, but the ion \[CIF_{2}^{+}~\]​ is bent. Hybridization schemes for...

The ion CIF2− CIF_{2}^{-}~ is linear, but the ion CIF2+ CIF_{2}^{+}~​ is bent. Hybridization schemes for the central ClCl atom to account for this difference in structure.
A. ClF2−−sp3dClF_{2}^{-}-s{{p}^{3}}d
B. ClF2+−sp3ClF_{2}^{+}-s{{p}^{3}}
C. ClF2+−sp3dClF_{2}^{+}-s{{p}^{3}}d
D. ClF2−−sp3ClF_{2}^{-}-s{{p}^{3}}

Explanation

Solution

To find the shape of a molecule, we need to identify the Lewis structure of the ion, and using the Lewis structure finds the steric number. Then using the VSEPR theory we can infer the shape, and hybridisation of the molecular structure of the given compound from its steric number. We also know that the Steric number is given by, SN=SN= (number of lone pair of electrons on the central atom) ++ (number of atoms bonded to the central atom)

Complete step by step answer:
We know that both fluorine and chlorine are elements of the halogen group from the periodic table. They are monovalent ions with 77 valence electrons in its outermost orbit. Since all the three constituting elements are halogens with similar valency, the heaviest and the element with least electronegativity will be the central atom. Hence in this case, is the central atom while the fluorine atoms form single bonds (due to its mono-valency), Drawing the Lewis structure, we get, Valence electrons on chlorine and fluorine =7=7 so, the total number of electrons on the given ion will be, 7+7(2)+1=227+7(2)+1=22

We know that each element forming a bond must have an octet electron exactly. Here we can see that the chlorine has more electrons than an octet, this is because the halogens can expand their octet while bonding among themselves. Now we can see that the central atom Chlorine has 3 lone pairs of electrons while it is bonded to two other fluorine atoms. Steric number; SN=3+2=5.SN=3+2=5.
We now know from the Lewis structure the steric number of the ion given is 5.5. Using the VSEPR theory we can find the hybridisation of the ion to be,sp3ds{{p}^{3}}d From the hybridisation structures of sp3ds{{p}^{3}}d we know if a compound has 33 lone pairs and 22 bond pairs then it forms a linear structure with 180o{{180}^{o}} . Similarly for CIF2+ CIF_{2}^{+}~ ion is bent and its sp3.s{{p}^{3}}.

So, the correct answer is Option A,B.

Note: The hybridisation is related to the geometries of molecules. It should be founded judiciously. Alternate method: We know that the central atom will be chlorine and it holds seven valence electrons and also holds an extra electron, hence eight electrons.