Chem 113 1st Edition Lecture 39 Outline of Last Lecture I. The relationship between Ksp and solubility at 25CII. Effect of pH on solubilityIII. Predicting the formation of a precipitateOutline of Current Lecture IV. Lewis acids and basesV. Transition metals as Lewis AcidsVI. ElectrochemistryCurrent LectureI. Lewis acids and basesa. Lewis acids accept a pair of electronsi. Have empty orbitals that can accept a pair of electronsii. Examples: H+, BH3, O=C bondsb. Lewis bases donate a pair of electronsi. Lone pair of electrons on one atomii. Examples: NH3, H2O, Cl-II. Transition metals as Lewis Acidsa. Each H2O is acting as a Lewis base or ligandb. Donate into empty d-orbitals of the metalc. The ability of transition metals to act as Lewis acids enables complex ion formationd. In acidic solutions, they are more solublee. In basic solutions, more soluble because it forms the complex ionThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.f. Slightly soluble ionic species are more soluble in solutions that enable complex ion formationIII. Electrochemistrya. Redox chemistry or the “stealing of electrons”b. Oxidation is loss of electronsc. Reduction is gain of
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