How many absorptions would you expect to see in the infrared spectrum of the T-shaped ClF3...

How many absorptions would you expect to see in the infrared spectrum of the T-shaped ClF3 molecule? Explain why.

Expert Solution

ClF₃ has a non-symmetric XY₃ structure. It shows six strong absorptions in IR spectrum, and some of these also appear simultaneously in Ramana spectrum. Thus the molecule is neither planar nor pyramidal. The molecule has been found to have a T-shaped structure. XY₃ molecules with T-shaped structures (e.g. ClF₃) belong to the C_2v point group. For the C_2v molecules ClF₃, there are six normal modes of vibration, approximately described as equatorial stretch, symmetric axial stretch, asymmetric axial stretch and three deformation modes. All six modes are IR active.

The chlorine atom has five electron-pairs in its outer shell; three of these are in Cl-F bonds, two are non-bonding ("lone") pairs. These keep as far apart as possible, minimizing repulsion between each of the negatively charged clouds, by adopting a trigonal bipyramidal arrangement. The two lone pairs occupy equatorial positions at an angle of 120° to each other; this gives the lowest energy arrangement of the electron pairs in the molecule.

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queen_honey_blossom answered 2 years ago

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