Slide No. 1Chapter 10: Shapes of MoleculesWhat's The Point?We learn how atomic orbitals combine to give molecules their observed structure.Lewis Dot StructuresDrawing Lewis Dot Structures of Molecular Compounds ResonanceFormal ChargeEstimating Bond Enthalpies from Bond EnergiesVSEPRMolecule PolarityReading:Entire ChapterHomework Problems:5(6), 9(10a),11(12a), 13(14a), 15(16b), 17(18), 19(20a,b), 21(22b), 26(24), 30(31), 43(44), 45(46), 49(50a,b,d), 51(52), 64(65)Lecture OutlineSlide No. 210.1 Lewis Dot Structures of Molecules Gilbert N. Lewis, American chemist (1875-1946)Lewis StructuresPredict atom connectivity and bond order in moleculesPredict three-dimensional molecular structure1)Determine total number of VEs in each atom (ns and np orbitals only).Add electrons for anions, subtract for cations. 2)Draw a molecular structure with single bonds between atoms H is always terminal (it can only form 1 bond)Least electronegative atom is usually the central atom and is often the first atom in the chemical formula (SO2, ClO4–)Each single bond that you drew uses up 2 (shared) electrons3)Determine # of remaining VEs (subtract 2 x bonds from total)4)Fill in the octets around the terminalatoms (except H) and again calculate the number of VEs remaining5)Place remaining electrons around central atomLewisin 1923Guidelines for Lewis Diagrams
has intentionally blurred sections.
Sign up to view the full version.