To devise a Lewis formula for SbCl5, we first need to consider the elements involved. Antimony (Sb) is the central atom, and it is surrounded by five chlorine (Cl) atoms.
1. **Counting Valence Electrons**: Antimony has 5 valence electrons (from group 15), and each chlorine has 7 valence electrons. So the total number of valence electrons is:
- 5 (Sb) + 5 × 7 (Cl) = 5 + 35 = 40 valence electrons
2. **Drawing the Lewis Structure**: In the Lewis structure for SbCl5, we place Sb in the center and surround it with five Cl atoms. Each Cl atom forms a single bond with Sb, using two electrons. So, we use 10 electrons for the five bonds, leaving us with 30 valence electrons to distribute around the chlorine atoms. Each chlorine atom will receive 3 lone pairs of electrons after forming the bond, completing their octet:
- Lewis structure:
3. **Hybridization**: The antimony atom in SbCl5 undergoes hybridization to accommodate five bonding pairs of electrons. The hybridization of Sb in this case is sp3d because it incorporates one s, three p, and one d orbital from the valence shell.
4. **Molecular Shape**: With five bonding pairs and no lone pairs, SbCl5 adopts a trigonal bipyramidal shape. In this geometry, three chlorine atoms occupy the equatorial positions, while the other two are in the axial positions, creating a symmetric arrangement that minimizes repulsion between the bonded pairs.
In summary, the Lewis formula for SbCl5 displays antimony in the center bonded to five chlorines, with an sp3d hybridization and a trigonal bipyramidal shape.