1) Explain the main concept behind the VSEPR theory of molecular
shape. How do both number and type of electron pairs influence the
shape of a molecule?
2) Explain how you were able to determine molecular polarity.
What two factors did you need to consider?
3) Although PH3 and BH3 both contain bonds of similar polarity,
one molecule is polar while the other is nonpolar
Which statement is true regarding the molecular shapes
A. Molecular shape can be predicted by the number of electrons
around an atom
B. Molecular shape can be predicted by the number of bonds
around an atom
C. Molecular shape can be predicted by the number of electron
pairs around an atom
D. Molecular shapes cannot be predicted by the number of
electrons around an atom
E. Both (B) and (C)
Give the electron geometry (eg), molecular geometry (mg), and
hybridization for PF3.
A) eg=tetrahedral, mg=trigonal planar, sp2
B) eg=trigonal pyramidal, mg=trigonal pyramidal, sp3
C) eg=tetrahedral, mg=trigonal pyramidal, sp3
D) eg=trigonal pyramidal, mg=tetrahedral, sp3
E) eg=trigonal planar, mg=trigonal planar, sp2
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...
Ethane (C2H6), ethylene (C2H4), acetylene (C2H2). Give the lewis
structure, VSEPR shape, bond angles, molecular dipole, valence bond
sketch, hybridization of each carbon atom, sigma and pi bonds for
each of the three substances above.