**Hybridization of SbPh5**

The hybridization of SbPh5 can be determined by considering the electronic configuration and bonding in the molecule. SbPh5 is the chemical formula for penta-phenyl antimony, which consists of one antimony atom bonded to five phenyl groups.

**Electronic Configuration of Antimony (Sb)**

Antimony (Sb) belongs to Group 15 (Group V) of the periodic table. Its atomic number is 51, and its electronic configuration is [Kr] 4d10 5s2 5p3. In the ground state, the antimony atom has three unpaired electrons in its valence shell.

**Valence Bond Theory**

According to valence bond theory, atoms form bonds by overlapping their atomic orbitals. Hybridization occurs when atomic orbitals mix to form new hybrid orbitals, which then participate in bonding. The type and number of hybrid orbitals formed depend on the number of electron pairs and the geometry of the molecule.

**Hybridization in SbPh5**

In SbPh5, antimony forms five bonds with the phenyl groups. To accommodate this, the three 5p orbitals of antimony hybridize with two of its 5s orbitals and form five sp3d hybrid orbitals. These hybrid orbitals are directed towards the corners of a trigonal bipyramidal geometry.

**Trigonal Bipyramidal Geometry**

In a trigonal bipyramidal geometry, the central atom (antimony) is surrounded by five groups (phenyl groups). Three of these groups lie in a trigonal plane, while the remaining two groups are axial and perpendicular to the plane. The axial and equatorial positions are occupied by the phenyl groups in SbPh5.

**Summary**

In summary, the hybridization of SbPh5 is sp3d. The antimony atom forms five sp3d hybrid orbitals by mixing its three 5p orbitals with two of its 5s orbitals. These hybrid orbitals are directed towards the corners of a trigonal bipyramidal geometry, allowing the antimony atom to form five bonds with the phenyl groups in SbPh5.