Draw the Lewis Dot Structure for oxalate (C2O4-2). Draw the Valence Bond orbital overlap diagram for the ion. Be sure to label all hybrid orbitals, all unhybridized orbitals, all bonds as
s or p, and any angles that are not apparent in your drawing.
Draw the Lewis Dot Structure for OCNH (the atoms occur in that order). Draw the Valence Bond orbital overlap diagram for the ion. Be sure to label all hybrid orbitals, all unhybridized orbitals, all bonds as
s or p , and any angles that are not apparent in your drawing. Are the lone pairs on the oxygen atom perpendicular or parallel to the H and lone pair on the nitrogen? Why?
Draw the Molecular Orbital Diagram for O2 (the "p" molecular orbitals appear in the logical order). What feature(s) of this structure justify the use of this theory (as opposed to Valence Bond theory or simple Lewis dot structures)? Be sure to explain not only the distinctive feature, but also the property or properties that relate to this structure, and how the property or properties can be observed, and why the property or properties exist.
Explain why the overlap of two atomic p orbitals can create
s , s *, p , and p * orbitals. Explaining may (should?) involve diagrams.
In first year chemistry, you probably heard about a sea of electrons that allowed metals to conduct. What do we really believe? Be complete in your answer.
Predict the structure, shape, bond polarity and molecular polarity for the following molecules:
sulfur hexafluoride (SF6)
Explain the reasoning behind the shapes of SF4 and IF3. In other words why do the lone pairs go where they do?