Chem 105 Friday, 5 Nov 2010
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1 Chem 105 riday, 5 Nov 2010 Lewis formula practice Sub-octet and expanded-octet molecules Molecular geometry Electron pair geometry vs. molecular geometry 11/5/2010 1
2 The preferred Lewis formula for CN contains how many single bonds? (int: ollow the procedure we discussed.) /5/2010 2
3 C N Answer: 2 (1 single bond) C N C N C N C N C N Not so good: + charge on, and charge separation is not necessary. This isocyanic acid, liquid bp 24 C. irst discovered in 1830 by rederick Wohler. ne of 129 interstellar molecules identified by rotational and vibrational spectroscopy. The 129 reported interstellar and circumstellar molecules 11/5/
4 Sub-octet (electron-deficient) atoms Be? ( No ) Be Do atoms donate electrons to give Be an octet? (No: the Be- bonds are single due to the high electronegativity of.) Compare bond lengths: =C= has = bonds (short). Be has bonds. (longer) 1.18 Å 1.40 Å 11/5/2010 4
5 Expanded octet atoms (3 rd, 4 th, 5 th period) can accommodate more than 8 valence electrons due to greater size. 10 valence electrons (5 bonds/non-bonding pairs) 12 valence electrons (6 bonds/non-bonding pairs) Cl P Chlorine pentafluoride Cl 5 Phosphorus pentafluoride P 5 11/5/2010 5
6 Molecular geometry is controlled by valence electron status VSEPR Valence Shell Electron Pair Repulsion 1. Valence electron pairs occupy orbitals look like balloons. 2. When attached to an atom, they repel each other due to negative charges. Very approximately, SINGLE, DUBLE, TRIPLE, & NN-BNDING PAIRS all look 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 3 balloons: Trigonal planar 4 balloons: Tetrahedral 180 B 11/5/ S 2-
7 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. 11/5/2010 7
8 Non-bonding electron pairs occupy one balloon. Therefore, a molecule may have DIERENT Electron Pair and Molecular (or ionic ) geometries. X B Trigonal-planar electron pair geom; Trigonal-planar molecular geometry 11/5/2010 8
9 X Trigonal-planar electron pair geom; Bent molecular geometry 11/5/2010 9
10 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 geom; Trigonal pyramidal molecular geometry Tetrahedral electron pair geom; Bent molecular geometry 11/5/
11 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) 11/5/
12 ig. 8-6, p. 371
13 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.) 11/5/
14 5 Electron Pairs Trigonal Bipyramidal ig. 8-8, p. 372
15 ig. 8-8, p. 372
16 Trigonal bipyramidal 11/5/
17 Yes, you do need to know the standard electron pair and molecular geometries. 11/5/
18 Expanded ctets: The electron pair geometry of atoms with IVE electron pairs is triangular bipyramid P Phosphorus pentafluoride P 5 S Sulfur tetrafluoride has one lone pair See-saw molecular shape 11/5/
19 The non-bonded pair does not occupy an apical position. The apical positions are more crowded than the equatorial positions. Lone pair orbitals are more diffuse than single bond orbitals. They prefer the roomier equatorial position. 11/5/
20 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 11/5/
21 In Cl 5 the smallest -Cl- bond angle is about /5/
22 90 Cl /5/
23 WL JK pasted trigonal pyramidal rather than trigonal bipyramidal. The former is a geometry derived from tetrahedral electron pair geometry. Trigonal bipyramidal geometry is derived from the trigonal bipyramidal electron pair geometry, which S 4 is. Use a text file ctrl-c file linear trigonal planar tetrahedral trigonal bipyramidal octahedral bent trigonal pyramidal seesaw t-shaped square pyramidal square planar 6+6+4(7)=40 11/5/ S = 30 = 3 nonbonding pairs on 5 atoms
24 The End 11/5/
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