Final answer:
The molecular geometries of SF6, BCl3, NI3, H3O+, S3, CH3F, SCN, HCl, CS2, and H2S are octahedral, trigonal planar, trigonal pyramidal, trigonal pyramidal, bent, tetrahedral, linear, linear, linear, and bent, respectively. These geometries are determined according to the VSEPR theory, considering both bonding and nonbonding electron pairs.
Step-by-step explanation:
Predicting the molecular geometry for the given compounds involves considering the electron pair geometry and the molecular structure for each compound based on VSEPR theory. The molecular geometry is determined by the arrangement of electron pairs around the central atom to minimize repulsion. Here are the molecular geometries of the given compounds:
- (a) SF6: Octahedral molecular geometry.
- (b) BCl3: Trigonal planar molecular geometry.
- (c) NI3: Trigonal pyramidal molecular geometry.
- (d) H3O+: Trigonal pyramidal molecular geometry.
- (e) S3: Bent molecular geometry (assuming it's the S3 radical with a V-shaped structure).
- (f) CH3F: Tetrahedral molecular geometry.
- (g) SCN: Linear molecular geometry.
- (h) HCl: Linear molecular geometry.
- (i) CS2: Linear molecular geometry.
- (j) H2S: Bent molecular geometry.
It's important to note that electron pair geometries account for both bonding and nonbonding electron pairs, while molecular geometries describe the spatial arrangement of only the atoms in a molecule.