(Polar molecules, Non-polar molecules, etc.)
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T-Shapes you mention here might refer to trigonal bipyramidal without two equilateral lone pairs. Trigonal bipyramidal and octehedra are the two shapes with 90 degree bond angles, and T-shape can never happen to octehedra because it would be very unstable. Thus, Trigonal bipyramidal without two equilateral lone pairs is the only plausible option by far we covered in this course.
T-shape refers to the shape molecules with 5 regions of electron density with 3 bonding pairs of electrons and 2 lone pairs, or the shape of molecules with 6 regions of electron density with 3 bonding pairs of electrons and 3 lone pairs.
T shaped is when the electron geometry is trigonal bipyrimidal because there are 5 regions of electron density around the CE and the Molecular shape is t-shaped because 3/5 of the regions of electron density are atoms and 2/5 are lone pairs.
T shaped molecules have 3 bonded atoms and 2 lone pairs. The 5 regions of electron density have trigonal bipyramidal geometry, and the two lone pairs are placed equatorially to maximize distance; this forms a T shaped molecule.
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