4. Construct an orbital interaction diagram for O2 and predict bond order for: O2, [O2]*, [O2], and [O2]*. Order the molecules from the shortest to longest O-O bond length.

a) Using Valence Bond Theory, NOT VSEPR, thoroughly show how silicon is able to form four identical atomic orbitals available for bonding in the compound SIF4. Be sure to discuss bond angles/shape. Then check part (b). Don't do part (b) stuff here.

a. Predict the molecular structure and bond angles for OC12. Approximate bond angles are sufficient. Molecular Structure = Bond Angles = b. Predict the molecular structure and bond angles for BeH2. Approximate bond angles are sufficient. Molecular Structure = Bond Angles

What orbital would the lone pair on the central oxygen of ozone (O3)be located?

10. Consider the peroxide ion, O22. Draw the molecular orbital diagram. Be sure to label your orbitals. Calculate the bond order. Is the peroxide ion attracted to magnetic fields or repulsed by magnetic fields? Briefly explain why or why not.

Platinum hexafluoride is an extremely strong oxidizing agent. It can even oxidize oxygen, its reaction with O2 giving O2+PtF6−.a. Sketch the molecular orbital energy level diagram for the O2+ ion.b. How many net σ and π bonds does the ion have?c. What is the O-O bond order?d. How has the bond order changed on taking away electrons from O2 to obtain O2+?e. Is the O2+ ion paramagnetic?

Question 15

1. Mark the following statements (A-E) as true or false A. The halogen bond dissociation energy decreases in the row Cl2 Br2 I2 because of repulsion between the electrons in the lower shells.  B. The melting points of the dihalogens increase down the group because the interactions between the dihalogen molecules get stronger C. The electronegativity of the halogens decreases down the group because of the decrease of the electron affinity and the increase of the ionization energy.   D. The unusually low bond dissociation energy of the F2 molecule is a direct result of the high electronegativity of fluorine   E.  The high reactivity of fluorine is in part due to the low bond dissociation energy of the F2 molecule

7. Draw Lewis structures for the following species. Indicate electron-pair geometry, idealized bond angles and hybridization for each central atom. Provide formal charges where appropriate. Write a resonance structure for NCO and predict the polarity of BrF3. NCO (central atom: C) PC33 BrF3

Xenon Tetrafluoride, XeF, Lewis Structure 3-D Molecular Structure Number of Valence Electrons Steric Number of Central Atom Electron Group Geometry/ Hybridization Molecular Geometry Bond Angle(s) Polar? (If yes, show dipole on 3-D structure)