Which of the following molecular geometries could describe a compound with a central atom that is dsp³ hybridized?

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11ecba2d_11cb_1899_a3bf_7d5a05036a66_MD0008_00 Hybrid orbitals form when two or more atomic orbitals (s, p, d, f) combine into new orbitals of different shape and spatial orientation. An atom's hybridization and electron geometry are dictated by the number of hybrid orbitals (electron-dense areas) formed around the atom. As the number of electron-dense areas increases, repulsion between orbitals increases. Electrons distribute themselves into specific configurations that minimize this repulsion. These electron distributions act as frames in which bonding may occur. The molecular geometry of a compound is determined only by the orientation of the bonds around the central atom, and nonbonding electron pairs are ignored. Two compounds may have the same number of electron-dense areas but different molecular geometries if they differ in number of lone electron pairs. Conservation of orbitals requires that the number of hybrid orbitals formed must equal the number of combined individual s, p, and d orbitals. Accordingly, compounds with a dsp³ hybridized central atom have five electron-dense areas, made from one d, one s, and three p orbitals. To minimize repulsion, three of the hybrid orbitals lie in the same plane, 120° apart, and the other two orbitals are 90° above and below the plane. Compounds with dsp³ hybridization and no lone pairs are trigonal bipyramidal. If a compound with dsp³ hybridization has either one or two lone pairs, it will have a see-saw or T-shaped geometry, respectively. (Choice A) Compounds with tetrahedral molecular geometry have four electron-dense areas around an sp³ hybridized central atom. (Choices B and D) Compounds with octahedral (no lone pairs) and square planar (two lone pairs) molecular geometries have six electron-dense areas around a d²sp³ hybridized central atom. Educational objective: Hybrid orbitals form when two or more atomic orbitals (s, p, d, f) combine into new orbitals. The number of hybrid orbitals (electron-dense areas) around an atom dictates its hybridization and electron geometry, whereas only the orientation of bonds around the central atom determines the molecular geometry (shape) of a molecule.

Which of the Following Molecular Geometries Could Describe a Compound