Manganese: [Ar]4s2 3d5. Mn in its +7 oxidation state (MnO4-) has a d0 configuration. Explain this situation if there are only 5 d electrons, it can lose 7 electrons to acquire the d0 configuration.

The halogen oxides and oxoanions are good oxidizing agents. For example, the reduction of bromate ion has an E value of 1.44 V in acid solution: 2BrO3(aq)+12H+(aq)+10eBr2(aq)+6H2O(l) Is it possible to oxidize aqueous 1.0 M Mn2+ to aqueous MnO4 with 1.0 M bromate ion?

There are only two geometric isomers of the tetraamminedichlorocobalt(III) ion, [Co(NH3)4Cl2]+. How many geometric isomers would be expected for this ion if it had a regular planar hexagonal geometry? Give drawings for them. Does this rule out a planar hexagonal geometry for [Co(NH3)4Cl2]+? Explain.

Give the oxidation state of the metal for each of the following oxides of [Hint: first transition series. (Hint: Oxides of formula M3O4 are examples of mixed valence compounds in which the metal ion is present in more than one oxidation state. It is possible to write these compound formulas in the equivalent format MO-M2O 3, to permit estimation of the metal’s two oxidation states.) (a) SC2O3. (b) TiO2. (C) V2O5. (d) CrO3. (e) MnO2. (f) Fe3O4. (g) CO3O4. (h) NiO. (i) CU2O

Basic solutions of Na4XeO6, are powerful oxidants. What mass of Mn(NO3)26H2O reacts with 125.0 mL of a 0.1717 M basic solution of Na4XeO6 that contains an excess of sodium hydroxide if the products include Xe and solution of sodium permanganate?

Using data in Appendix 1, estimate the temperature at which Fe2O3 can be reduced to iron, using hydrogen gas as a reducing agent (assume H2O(g) is the other product).