Describe the molecular geometry of: (a) GeH4 (b) NH3 (c) H2S

Question

Accepted Answer

Step 1: Determine the central atom and count the total number of valence electrons for each molecule. For GeH4, Ge is the central atom with 4 valence electrons, and each H contributes 1 electron, totaling 8 valence electrons. For NH3, N is the central atom with 5 valence electrons, and each H contributes 1 electron, totaling 8 valence electrons. For H2S, S is the central atom with 6 valence electrons, and each H contributes 1 electron, totaling 8 valence electrons.. Step 2: Draw the Lewis structure for each molecule. For GeH4, place Ge in the center and arrange the 4 H atoms around it, forming single bonds. For NH3, place N in the center with 3 H atoms bonded to it and a lone pair on N. For H2S, place S in the center with 2 H atoms bonded to it and 2 lone pairs on S.. Step 3: Apply the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. For GeH4, with 4 bonding pairs and no lone pairs, the geometry is tetrahedral. For NH3, with 3 bonding pairs and 1 lone pair, the geometry is trigonal pyramidal. For H2S, with 2 bonding pairs and 2 lone pairs, the geometry is bent.. Step 4: Describe the bond angles based on the molecular geometry. In a tetrahedral geometry like GeH4, the bond angles are approximately 109.5°. In a trigonal pyramidal geometry like NH3, the bond angles are slightly less than 109.5° due to the lone pair repulsion. In a bent geometry like H2S, the bond angles are even smaller, typically around 104.5°.. Step 5: Summarize the molecular geometries: (a) GeH4 is tetrahedral, (b) NH3 is trigonal pyramidal, and (c) H2S is bent. These geometries are determined by the number of bonding pairs and lone pairs around the central atom, as predicted by VSEPR theory.

Describe the molecular geometry of: (a) GeH4 (b) NH3 (c) H2S

주요 개념

VSEPR Theory

Hybridization

Molecular Geometry