Octahedral arrangement hybrid orbitals

We need six orbitals to accommodate six electron pairs around an atom in an octahedral arrangement, as in SF6 and XeF4, and so we need to use two d-orbitals in addition to the valence s- and p-orbitals to form six sp3d2 hybrid orbitals (Fig. 3.18). These identical orbitals point toward the six corners of a regular octahedron. 

A molecule with a steric number of 6 requires six hybrid orbitals arranged in octahedral geometry. In Chapter 9, sulfur hexafluoride appears as the primary example of a molecule with a steric number of 6 (Figure ). Six equivalent orbitals for sulfur can be constmcted for the inner sulfur atom by combining the 3. S, the three 3 p,... 

This requires an octahedral arrangement of pairs and, in turn, an octahedral set of six hybrid orbitals. This leads to d2sp3 hybridization, in which two d orbitals, one s orbital, and three p orbitals are combined (see Fig. 14.23). Note that six electron pairs around an atom are always arranged octabedrally, requiring d2sp3 hybridization of the atom. Each d2sp3 orbital on the sulfur atom is used to bond to a fluorine atom. Since there are four pairs on each fluorine atom, the fluorine atoms are assumed to be sp3 hybridized. 

The hybrid orbitals used by the metal ion depend on the number and arrangement of the ligands. For example, accommodating the lone pair from each ammonia molecule in the octahedral Co(NH5)63+ ion requires a set of six empty hybrid atomic orbitals with an octahedral arrangement. Recall that an octahedral set of orbitals is formed by the hybridization of two d, one s, and three p orbitals to give six dfsp orbitals (see Fig. 20.19). 

Although the spatial arrangement of six electron pairs round I-atom is octahedral, due to the presence of two lone pairs of electrons in the axial hybrid orbitals, the shape of IC14- ion gets distorted and becomes square planar as shown in Fig. 

The octahedral [SiF6]2 molecular ion, and a simple valence bond approach to explaining its formation. Overlap of a p orbital containing two electrons on each of the six fluoride anions with one of six empty hybrid orbitals on the Si(IV) cation, arranged in an octahedral array, generates the octahedral shape with six equivalent covalent a bonds. 

The extended valence bond description of inner shell and outer shell bonding for octahedral cobalt(III) complexes, required as a result of different d-electron arrangements on the metal. The six empty hybridized orbitals can in each case accommodate six bonding lone pairs from six ligand donor atoms. 

Hybridization of v, p,., Py, p, d i and d,.i yi atomic orbitals gives six sp d hybrid orbitals corresponding to an octahedral arrangement. The bonding in M0F5 can be described in terms of sp d hybridization of the central atom. If we remove the z-components from this set (i.e. p and d i) and hybridize only the s, Px, Py and d i yi atomic orbitals, the resultant set of four sp d hybrid orbitals corresponds to a square planar arrangement, e.g. [PtCLi]. ... 

With the six metal electrons placed in this way, the hybrid orbitals are empty. Each of these interacts with the doubly occupied orbital of the ligand L towards which it points, thereby forming six bonds in an octahedral arrangement (5-5). 

The aiTangement of hybrid orbitals is octahedral and the bond angles are 90°. 9.5B One of the 2s electrons in Be is promoted to an empty p orbital. The. 5 orbital and one p orbital hydridize to form two sp hybrid orbitals. Each hybrid orbital contains one electron and overlaps with a singly occupied 2p orbital on an F atom. The arrangement is linear with a bond angle of 180°. 9.6A 16 tr bonds and 4 tt bonds. 9.6B 17 rr bonds and 5 ir bonds. 9.7A C and N atoms are sp-hybridized. The triple bond between C and N is composed of one sigma bond (from overlap of hydrid orbitals) and two pi bonds (from interaction of remaining p orbitals). 

FIGURE 3.18 One of the six sp d1 hybrid "S-orbitals, and their six directions, that may be formed when el-orbitals are available 2 and we need to account for an octahedral o arrangement of electron pairs. 

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