Chemistry 105 Chemistry 105
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This 3 page Class Notes was uploaded by Emma Silverman on Sunday April 12, 2015. The Class Notes belongs to Chemistry 105 at Washington State University taught by Finnegan in Spring2015. Since its upload, it has received 103 views. For similar materials see Chem 105: Principles of Chemistry in Chemistry at Washington State University.
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Date Created: 04/12/15
4615 Exam 3 Chemistry 105 Thursday April 16th 2015 600700 PM Same place as the other exams Covers chapters 76106 quizzes 79 HW sets 912 lab experiments 4 5 10 Review Tuesday April 14th 700900PM da pit The AXE type of a compound can be found from a valid Lewis structure AXnEm n of bonding groups on the central atom m of lone pairs on the central atom Any type of bond single double or triple is one bonding group nm the number of electron groups on the central atom Valence Shell Electron Pair Repulsion Theory VSEPR Groups of valence electrons around an atom will tend to get as far apart from each other as possible The number of electron groups determines the Electron Geometry Geometry The electron geometry determines the ideal bond angles approximate bond angles Electron geometry and the number of lone pairs determines the Molecular Geometry Molecular Shape The Molecular Shape the bond polarities and the formal charge distribution determine the Molecular Polarity see table 101 on page 434 NOT GOING TO BE ON EXAM KNOW THEM Learning Catalytics A 2 Electron 1 Linear Groups B 3 Electron 2 Trigonal Planar Groups C 4 Electron 3 Tetrahedral Groups D 5 Electron 4 Trigonal Groups Bipyramidal E 6 Electron 5 Octahedral Groups What is the electron geometry around the central atom in I3quot Hnear trigonal planar bent tetrahedral trigonal pyramid trigonal bipyramidal seesaw Tshaped octahedral square pyramidal square planar 4815 The electron geometry determines the ideal bond angles approximate bond angles Lone pairs take up more space than bonding pairs see section 103 Double bonds take up more space than single bond see page 427 41015 Valence Bond THeory A covalent bond is produced by the overlap of orbitals in the region between the two atoms The greater overlap the stronger bond Problem THe atomic orbitals do not always point in the right directions to produce the shapes that we know that molecules have To explain this it is assumed that the atomic orbitals are mixed to produce hybrid orbitals that point in the correct direction Hybrid orbitals are named from the orbitals that contribute to them sp2 are a combination of one s and two p orbitals Note all of the orbitals that are mixed must come from the same shell same value of n The total number of orbitals is unchanged there will be two sp orbitals three sp2 orbitals four sp3 orbitals etc Each type of hybrid orbital is associated with a specific electron geometry 1What is the orbital hybridization on the central atom in SeOZ SP SP sp3 sp3d sp3d2 2 2What is the orbital hybridization on the central atom in PCI3 SID SID SP sp3d sp3d2 2 3 3What is the orbital hybridization on the central atom in 804239 SP SP sp3 sp3d sp3d2 2 Single bonds are formed by the overlap of orbitals in the region between the atoms Such bonds are called sigma 0 bonds Double and triple bonds also contain a 0 bond but the second and third bond cannot form directly between the atoms there is already a pair of electrons there The additional bonds are formed by unhybridized porbitals that overlap in the areas to either side of the 0 bond Such bonds are called pi 1T bonds How many sigma bonds and how many pi bonds are present in the following molecule SHE E GEN 39 orquot EEK HEH GH EH3 3 1 L 1H 125