1) What are the bond angles in the molecular model of SI6?
2) What is the bond angle in the following molecular model of H2Te?
3) What is the geometry around the central atom in the following molecular model of BF3?
To create a molecular model, a student will use blue spheres to represent nitrogen (N) and white spheres to represent hydrogen (H). Which option correctly describes a model of ammonia, NH3?(1 point)
Responses
three blue spheres and one white sphere
three blue spheres and one white sphere
one blue sphere and one white sphere
one blue sphere and one white sphere
three blue spheres and three white spheres
three blue spheres and three white spheres
one blue sphere and three white spheres
one blue sphere and three white spheres
To determine the bond angles and geometry in molecular models, you need to know the electron geometry and the number of bonded and lone pairs around the central atom.
1) To determine the bond angles in the molecular model of SI6, we first need to know the electron geometry. In SI6, there are six bonding pairs and no lone pairs around the central atom. Since all the bonding pairs repel each other equally, the electron geometry is octahedral.
In an octahedral geometry, the bond angles between any two adjacent bonds are 90 degrees. Therefore, the bond angle in SI6 is 90 degrees.
2) For the molecular model of H2Te, we need to know the electron geometry and the number of bonded and lone pairs. In H2Te, there are two bonding pairs and two lone pairs around the central atom.
The electron geometry of H2Te is tetrahedral, which has bond angles of approximately 109.5 degrees. However, the presence of two lone pairs affects the bond angles in the molecule. Lone pairs exert greater repulsion compared to bonding pairs, causing the bond angle to deviate slightly from the ideal tetrahedral angle. Therefore, the bond angle in H2Te would be slightly less than 109.5 degrees.
3) To determine the geometry around the central atom in the molecular model of BF3, we again need to know the electron geometry and the number of bonded and lone pairs. In BF3, there are three bonding pairs and no lone pairs around the central atom.
The electron geometry of BF3 is trigonal planar, which has bond angles of 120 degrees between any two adjacent bonds. Therefore, the geometry around the central atom in BF3 is trigonal planar with bond angles of 120 degrees.