A. Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (a)'s geometry.  B. Give the number of total electron groups, the number of bonding...

 


A. Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (a)'s geometry. 

B. Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (b)'s geometry. 

C. Give the number of total electron groups, the number of bonding groups, and the number of lone pairs for (c)'s geometry.

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This question requires using Valence Shell Electron Pair Repulsion or VSEPR theory to explain the shapes of molecules. According to VSEPR theory molecules take on the shapes in which valence electron pairs have the maximum separation. It's necessary to consider both bonding and lone (non-bonding) pairs because both influence the shape of the molecule by repelling other electron pairs. 

A. This molecule has six atoms bonded around a central atom. It has six electron pairs, six bonding pairs and no lone pairs. The molecular geometry is octahedral with sp3d2 hybridization, meaning that the bonding orbitals are blends of an s, three p and two d orbitals. The six hybrid orbitals are equal in energy. The octahedron shape is the maximum separation of all six electron pairs. 

B. This molecule also has sp3d2 hybridization with a total of six electron pairs. It has 4 bonding pairs and 2 lone pairs. The molecular geometry is square planar.

The four atoms bonded to the central atom don't have...

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