Describe the shape of each of the following molecules or ions, and tell which hybrid orbitals are used by the central atom. (a) GeBr4 (b) CO2 (c) CO32- (d) SnCl3-

Verified step by step guidance

1. Step 1: Determine the central atom and count the total number of valence electrons for each molecule or ion. For example, in GeBr4, the central atom is Ge, and you need to consider the valence electrons from Ge and Br atoms.
2. Step 2: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. For GeBr4, with four bonding pairs and no lone pairs on the central atom, the shape is tetrahedral.
3. Step 3: Identify the hybridization of the central atom based on the number of electron domains (bonding and lone pairs). For GeBr4, with four electron domains, the hybridization is sp3.
4. Step 4: Repeat the process for CO2. The central atom is C, with two double bonds to O atoms. According to VSEPR, the shape is linear, and the hybridization is sp.
5. Step 5: For CO32-, consider the resonance structures and the central atom C. With three bonding pairs and no lone pairs, the shape is trigonal planar, and the hybridization is sp2. For SnCl3-, the central atom Sn has three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape with sp3 hybridization.