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Enhanced PromptMolecular geometry chart based on VSEPR theory, detailing electron pair arrangements and corresponding shapes, including linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral geometries, with bond angles and examples of molecules for each shape, showcasing the relationship between electron pairs and molecular structure, a comprehensive chart including the following information:
Linear: 2 electron pairs, 180-degree bond angle, examples include CO2 and HCN
Trigonal Planar: 3 electron pairs, 120-degree bond angle, examples include CO3^2- and NO3^-
Tetrahedral: 4 electron pairs, 109.5-degree bond angle, examples include CH4 and NH4^+
Trigonal Bipyramidal: 5 electron pairs, 90-degree and 120-degree bond angles, examples include PCl5 and SF4
Octahedral: 6 electron pairs, 90-degree bond angle, examples include SF6 and XeF4
Bent or V-shape: 2 electron pairs and 1 lone pair, 104.5-degree bond angle, examples include H2O and SO2
Trigonal Pyramidal: 3 electron pairs and 1 lone pair, 107-degree bond angle, examples include NH3 and PCl3
T-shaped: 3 electron pairs and 2 lone pairs, 90-degree bond angle, examples include ClF3 and ICl3
Seesaw: 4 electron pairs and 1 lone pair, 90-degree and 120-degree bond angles, examples include SF4 and TeCl4
Square Pyramidal: 5 electron pairs and 1 lone pair, 90-degree bond angle, examples include BrF5 and XeOF4
Square Planar: 4 electron pairs and 2 lone pairs, 90-degree bond angle, examples include XeF4 and PtCl4^2-
Octahedral with one lone pair: 5 electron pairs and 1 lone pair, 90-degree bond angle, examples include XeOF4 and OsF6
Molecular structures depicted using ball-and-stick models, with electron pairs represented by lines and lone pairs shown as dots, highlighting the importance of VSEPR theory in predicting molecular geometry, a fundamental concept in chemistry and physics.
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