Chem 105 Friday 4 Nov 2011
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1 Chem 105 riday 4 Nov 2011 Chemical & Engineering News magazine Article on alogenated volatile organic compounds and groundwater pollution Valence Shell Electron Pair Repulsion (VSEPR) model Bond polarity and electronegativity
2 An excellent student question: how did I know this is the connection map of trichloroethylene? 1. It turns out that for this formula, there is only one map, or isomer, that satisfies octets of C s and Cl s. 2. The chemical name ethylene (or ethene ) refers to a C=C bond, so already I knew what the answer was nce you have that, there is only one way to install the Cl s. 3. We (i.e., you) will learn the ethene structure/name in Chap. 10. owever, for the present, I will either provide a map, or describe it. In this case, it might say, the two C s are connected, and one C has two Cl s attached. Lab # 9. Article on alogenated volatile organic compounds and groundwater pollution p. 32 Trichloroethylene C 2 Cl 3
3
4 Molecular geometry is controlled by valence electron arrangement. Why is the DNA phosphate P tetrahedral?? Why are the bases (A,G,C,T) flat? 11/2/2011 4
5 VSEPR Valence Shell Electron Pair Repulsion 1. Valence electron pairs occupy orbitals look like balloons. 2. When attached to an atom, they repeleach other due to negative charge. Veryapproximately, SINGLE, DUBLE, TRIPLE, & NN-BNDING PAIRS alllook like a balloon. 3. These lead to various Electron Pair Geometries: X 2 balloons: Linear X X -C N: S=C=N - Cl-Be-Cl balloons: Trigonal planar 4 balloons: Tetrahedral 11/2/ B S 2-
6 Actual balloons can be used to represent electron orbitals. Linear Trigonal planar Tetrahedral ne balloon can represent a single, double, or triple bond, or non-bonding pair. 11/2/ ig. 9.7, p.398
7 Non-bonding electron pairs occupy one balloon. Therefore, a molecule may have DIERENT Electron Pair and Molecular (or ionic ) geometries. X Trigonal-planar electron pair geometry; Bent molecular geometry (isocyanic acid) 11/4/2011 7
8 Non-bonding electron pairs occupy one balloon. Therefore, a molecule may have DIERENT Electron Pair and Molecular (or ionic ) geometries. X X Cl 3- anion - 2 S molecule Cl Cl S S Tetrahedral electron pair geometry; Trigonal pyramidal molecular geometry Tetrahedral electron pair geometry; Bent molecular geometry 11/4/2011 8
9 Methylamine C 3 N 2 N Bond angle ~ 109 o Central N has a tetrahedral electron pair geometry (4 electron pairs)......and trigonal pyramidal molecular geometry (3 bonds and 1 nb pair) 11/4/2011 9
10 The actualbond angle may differ by several degrees from the nominalbond angle. This is due to the slightly larger size of the lone pair electron cloud compared to a single bond. ig. 8-6, p. 371
11 Expanded octet electron pair geometries Trigonal bipyramidal ctahedral (all positions are equivalent in the octahedral geometry) ne balloon can represent a single, double, or triple bond, or non-bonding pair. (In 5-coordinate atoms, a non-bonding pair occupies the less-crowded equatorial position.) 11/4/
12 5 Electron Pairs Trigonal Bipyramidal ig. 8-8, p. 372
13 ig. 8-8, p. 372
14 Yes, you do need to know the standard electron pair and molecular geometries. 11 terms. 11/4/
15 Expanded ctets: The electron pair geometry of atoms with IVE electron pairs is trigonal bipyramidal P Phosphorus pentafluoride P 5 S Sulfur tetrafluoride has one lone pair Seesaw molecular shape 11/4/
16 The non-bonded pair does not occupy an apical position. The apical positions are more crowdedthan the equatorial positions. Lone pair orbitals are more diffusethan single bond orbitals. They prefer the roomier equatorial position. 11/4/
17 Expanded ctet: 6 e- pairs) ctahedral e- pair geometry S 6 1 non-bonding pair: square pyramidal Cl Chlorine pentafluoride has one lone pair Cl 5 ctahedral e- pr Square pyramidal molecular 11/4/
18 In Cl 5 the smallest-cl- bond angle is about
19 Cl 5 90 (nominal bond angles) 11/4/
20 Cl 5 85 (computed bond angles) /6-311+G(d,p) 11/4/
21 WL JK pasted trigonalpyramidal rather than trigonalbipyramidal. The former is a geometry derived from tetrahedralelectron pair geometry. Trigonal bipyramidal geometry is derived from the trigonal bipyramidalelectron pair geometry, which S 4 is. S 6+6+4(7)= = 30 = 3 nonbonding pairs on 5 atoms 11/4/
22 Polarity of Molecules Define electronegativity = the ability of an atom to pull bonding electrons toward itself. Electrons in covalent bonds between identical atoms are equally shared. Electrons in covalent bonds between nonidentical atoms are not equally shared. δ- C δ+ The more electronegative atom pulls bond electrons toward itself it becomes partially negative 11/8/
23 N C Cl S Br 11/8/
24 Increases (due to increasing effective nuclear charge) Increases 11/8/
25 The End 11/4/
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