Question

The molecules BF₃ and SO₃ are both described as trigonal planar. Does this information completely define the bond angles of these molecules?

What is the difference between the electron-domain geometry and the molecular geometry of a molecule? Use ammonia molecule as an example in your discussion.

     c. Acetone, C₃H₆O, is commonly used as organic solvent that is the main component of some nail-polish removers. Its Lewis structure shows the following connectivity CH₃-CO-CH₃

                 i.      What is the total # of valence electrons in the acetone molecule?

   ii.   How many valence electrons are used to make sigma bonds in the molecule

  iii.     How many valence electrons are used to make pi bonds in the molecule?

iv.   How many valence electrons remain in non-bonding pairs in the molecule?

v.     What is the hybridization at the central carbon atom of the molecule?

Answer 1

A. Both BF3&SO3 have 120°

B. Electron geometry includes lone pair of electrons while molecular geometry excludes lone pair of electrons.

Electron pair geometry of NH3: tetrahedral

MOlecular geometry: Pyramidal

C. No of valency electrons in acetone: 24(3x4=12 for C, and 6 for O and 6 for 6H)

Valency electron in sigma bond= 18

No of electrons in pi bond= 2

No of non binding electrons: 4 on oxygen

Hybridization of central carbon :sp2