![]() Thus, Chlorine Trifluoride (ClF 3 ) has 2 lone pairs and 3 bond repulsion units. ![]() There also exists an asymmetric charge distribution around the ClF 3 hybridization of the central atom. If two bonds of the trigonal bipyramidal basic geometry are changed into two lone pairs, therefore hybridization and shape of ClF 3 shape will be in “T” shape. If the central atoms contain 5 bond repulsion units and if it doesn’t contain a lone pair on the central atom, the molecule shape is trigonal bipyramidal having a bond angle of 175° F-Cl-F. Chlorine Trifluoride (ClF 3 ) represents a Trigonal bipyramidal geometry. Predicting molecular geometry and hybridization of ClF 3 can be done using some methods. Besides, here the two-hybrid orbitals will contain a pair of electrons, and three hybrid orbitals will contain unpaired electrons, which again will overlap with the 2p orbital of F to form the resultant single bonds. All in all, during the hybridization, one 3s orbital, three 3p orbitals, and one of the 3d orbitals participate in the process that leads to the formation of five sp 3 d hybrid orbitals. Here, one of the paired electrons of Cl present in the 3p subshell remains as either a lone pair or unpaired. Now, when the Cl needs to combine with Fluorine atoms to form ClF 3, it requires three unpaired electrons to bond with the three F-atoms. If we closely notice the valence electronic configuration of Chlorine (Cl), it is represented as 3px 2, 3s 2, 3py 2, 3pz 1, 3d. This atom holds 7 valence electrons while ClF 3 should consist of 2 lone-pairs and 3 bond-pairs. If we speak about the hybridization of chlorine trifluoride, we should consider its central atom, which is Chlorine (Cl).
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