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?

Consider the molecule of nitrosopropane. Its Lewis structure is shown. H H H 411- C C H H H Which Oxygen orbitals are involved in pi bonding in nitrosopropane? 2p sp O sp³ O sp² H 2s

Draw the Lewis structure for NO3- including the resonance structures. Does this NO3- have delocalized p bonds?

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