Chem111 Fall, 2005 51Enough of atoms! Let's see how they form molecules … Consider the molecules CO2and H2O OCOOHH•linear •bent •non-polar •quite polar •gas at room temp. •liquid at RT •two double bonds •two single bonds We could use the Schrödinger equation, approximations, lots of complicated mathematics, and a computer program and solve for the structures of our molecules. Ætoo expensive(both $$ and time) /Æwe will come up with "rough" methods, based upon concepts ☺Organizationof this part of the course •What are bonds? (Ionic bonds, covalent bonds, in-between) •Brief review of Lewis dot structures – electron bookkeeping •How can we predict (accurately) the shapes of molecules? (VESPR) •What does quantum mechanics tell us about bonding? (Molecular Orbitals) Lecture 13: Bonding and Molecules•Ionic and Covalent bonds •Electronegativity •Lewis Dot Structures •VESPRR (I)
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