Chemistry 111 1st Edition Exam # 2 Chapters 5-6Chapter 5 Bond AngleAngle (degrees) defined by lines joining the centers of two atoms to the center of a third atom to which they are covalently bondedVESPR TheoryA model predicting that the arrangement of valence electron pairs around a central atom minimizes repulsion to produce the lowest energy orientationElectron Pair Geometry3-dimensional arrangement of bonding e- pairs and lone pair electrons about a central atomMolecular Geometry3-dimensional arrangements of atoms in a moleculeTwo atoms bonded to central atom  linear (180 degrees)Three atoms bonded to a central atom  trigonal planar (120 degrees)4 atoms bonded to central atom  tetrahedral (109.5 degrees)5 atoms bonded to central atom trigonal bipyramidal (90 to 120 degrees)6 atoms bonded to central atom  octahedral (90 degrees)Bond DipoleSeparation of electrical charge created when atoms with different EN form a covalent bondPolar MoleculeSum of bond dipole vectors > zeroSigma BondCovalent bond having highest electron density between the two atoms along the bond axis. All bonds are sigma bonds. In a double or triple bond, one of the bonds is a sigma bond.Pi BondParallel p orbitals form pi bonds. A single bond is always a sigma bond, but a double bond has a sigma and a pi bondHybridizationMixing of atomic orbitals to generate new sets of equivalent orbitals that form covalent bonds with other atomsSp= 2 groups Sp2 = 3 groupsSp3= 4 groupsSp3d= 5 groupsSp3d2 = 6 groupsChapter 6Dispersion (London) ForcesIntermolecular force between nonpolar molecules caused by the presence of temporary dipolesin the molecules. (Nonpolar + Nonpolar molecules)  every bond has dispersion forcesTemporary Dipole (Induced Dipole)Separation of charge produced in an atom or molecule by a momentary uneven distribution of electronsPolarizabilityRelative ease with which the electron cloud in a molecule, ion, or atom can be distorted, inducing a temporary dipoleSize of Atoms/MoleculesLarger atoms/molecules more polarizable than smaller atoms/smaller. Dispersion increases withpolarizabilityShape of MoleculesIncreased surface area = increased interactions between molecules. Linear molecules have higher dispersion than branched molecules of similar molecular weightDipole-DipoleAttractive force between polar moleculesHydrogen BondStrongest dipole-dipole interaction. Occurs between H atom bonded to a small, highly electro negative element (F, O, N) and an atom of oxygen O or N in another moleculeIon-DipoleAttractive force between an ion and a molecule that has a permanent dipoleSphere of HydrationCluster of water molecules surrounding anion in aqueous medium. Sphere of solvation if solventother than H2O. Like Dissolves Like:Ionic/polar solutes will be soluble in polarsolvents.Nonpolar solutes will be soluble in