Final answer:
Each ion is matched to its molecular geometry by considering the number of electron pairs around the central atom. C2O42- displays tetrahedral, PS33- has trigonal pyramidal, and SiO32- is trigonal planar molecular geometries.
Step-by-step explanation:
To match the ions with their correct molecular geometry, one must look at the number of electron pairs, including both bonding pairs and lone pairs, around the central atom. This is dictated by the VSEPR theory:
C2O42- (Oxalate ion): This ion has a central carbon atom with two oxygen atoms double-bonded and two oxygens single-bonded, creating a total of four regions of electron density. This results in a tetrahedral electron-pair geometry, but since there are no lone pairs on the carbon atom, the molecular structure is also tetrahedral.
PS33- (Phosphite ion): This ion has four regions of electron density around the central phosphorus atom (three bonding pairs and one lone pair), leading to a tetrahedral electron-pair geometry, but with the lone pair, the molecular structure becomes trigonal pyramidal.
SiO32- (Silicate ion): With three oxygen atoms bonded to the central silicon and no lone pairs, this ion has three regions of electron density, resulting in a trigonal planar electron-pair geometry and molecular structure.
Therefore, the correct matches are:
C2O42-: Tetrahedral
PS33-: Trigonal Pyramidal
SiO32-: Trigonal Planar