Consider the same situation as in Exercise E10C.4(a). Find the irreducible representations spanned by the combinations \(\mathrm{p}_{y}(\mathrm{~A})+\mathrm{p}_{y}(\mathrm{~B})\) and \(\mathrm{p}_{y}(\mathrm{~A})-\mathrm{p}_{y}(\mathrm{~B})\). Are there any valence orbitals of the central O atom that can have a non-zero overlap with these combinations of F orbitals?
Text Transcription:
p_yA+p_yB
p_yA-p_yB
Chapter 5 Tuesday, April 05, 2016 1:16 PM Oxidation Reduction (redox) reactions Redox Reactions o Transfer or exchange of electrons between two species o To show both components occurring together o Oxidation- lose electrons OiL o Reduction- gain electrons RiG o Oxidation and reduction must occur together o No net change in the number of electrons in a redox reaction (both sides of the reaction must have same number of atoms and charge) o Reducing agent- species or substance that donates electrons o Oxidizing agent- species or substances that accept the electron Oxidation numbers o Number that is assigned to an element in a molecule or ion to reflect qualitatively its state of oxidation o Batteries, metabolism of food, combustion, bleach o Method of bookkeeping to track electrons o Change in oxidation number of an element shows that a redox reaction has occurred o Rules Sum of oxidation number in a neutral species is 0 Atoms of free elements have ON of 0 ON of metal ions in groups 1A 2A and Al have +1, +2, +3 respectively If a transition metal, () determines the oxidation number Nonmetals have negative numbers Bonded with nonmetal, oxygen is +1 Bonded with metal, oxygen is -1 Fluorine is -1
