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VSEPR MODEL Valence Shell Electron Pair Repulsion Model A model for predicting the shapes of molecules and ions in which valence shell electron pairs are.

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Presentation on theme: "VSEPR MODEL Valence Shell Electron Pair Repulsion Model A model for predicting the shapes of molecules and ions in which valence shell electron pairs are."— Presentation transcript:

1 VSEPR MODEL Valence Shell Electron Pair Repulsion Model A model for predicting the shapes of molecules and ions in which valence shell electron pairs are arranged about each atom so that electron pair repulsion is minimized. ELECTRONIC GEOMETRY The general shape of a molecule determined by the number of electron pairs around the central atom occupying different quadrants. Gives starting point for bond angle. MOLECULAR GEOMETRY The general shape of a molecule determined by the relative positions of the atomic nuclei. The nonbonding electron pairs modifiy the geometry.

2 VSEPR MODEL I. Draw the Lewis dot structure. electronic geometry II. Determine the electronic geometry by counting the number of pairs of electrons around the central atom occupying different quadrants (top, bottom, left, right). This geometry gives the initial bond angle. Pairs of e- geometry bond angle 2 linear 180 o 3 trigonal planar 120 o 4 tetrahderal o

3 VSEPR MODEL III. Next, using the electronic geometry, determine the number of bonding and nonbonding electron pairs then arrange the electron pairs as far apart as possible. ___ nonbonding pairs require more space than bonding pairs. ___ multiple bonds require more space than single bonds. molecular geometry IV. The direction in space of the bonding pairs give the molecular geometry modified by the position of the nonbonding pairs.

4 Fig. 13-1, p. 369

5 Fig. 13-2, p. 369

6 Fig. 13-3, p. 370

7 Table describing Molecular Geometry VSPER Theory Number of electronic bonding nonbonding molecular e- pairs geometry e- pairs e- pairs geometry linear 2 linear 2 0 linear trigonal planar 3trigonal planar 3 0trigonal planar trigonal planar 3trigonal planar 2 1bent tetrahedral 4tetrahedral 4 0tetrahedral tetrahdral 4tetrahdral 3 1trigonal pyramidal tetrahedral 4tetrahedral 2 2bent

8 Fig. 13-4, p. 370

9 Fig. 13-5, p. 372

10 Table 13-2, p. 371

11 p. 374

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13 p. 375

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16 p. 376

17 Predict the Molecular Geometry for the following molecules. Predict the Molecular Geometry for the following molecules. 1. H 2 O tetrahedral BENT There are 4 pairs of electrons around the central atom so the electronic geometry is tetrahedral with a bond angle of o. Since 2 of the pairs of electrons are bonding and the other two pairs are nonbonding, the electronic geometry has been modified to a molecular geometry of BENT. 2. CO 2 LINEAR There are four pairs of electrons in two different quadrents (left & right) so the molecular geometry is LINEAR with a bond angle of 180 o..... : O = C = O :

18 Predict the Molecular Geometry for the following molecules. Predict the Molecular Geometry for the following molecules. 3. BH 3 trigonal planar There are 3 pairs of electrons around the central atom so the electronic geometry is trigonal planar with a bond angle of 120 o. Since all three pairs of electrons are bonding, the electronic geometry has not been modified. 4. NH 3 tetrahedral TRIGONAL PYRAMIDAL There are 4 pairs of electrons around the central atom so the electronic geometry is tetrahedral with a bond angle of o. Since 3 of the pairs of electrons are bonding and the other pair is nonbonding, the electronic geometry has been modified to a molecular geometry of TRIGONAL PYRAMIDAL.

19 Practice Problems Draw the Lewic structure for the following, then predict both the electronic & molecular geometry. Give the approximate bond angle. (See instructor for answers) a) GeH 2 b) AsF 3 c) AlF 3 d) SO 2 e) SO 3 f) SO 3 2- g) SiF 4 h) C 2 H 4 I) Cl 2 O

20 Group Study Problems Draw the Lewic structure for the following, then predict both the electronic & molecular geometry. Give the approximate bond angle. a) H 2 Sb) PH 3 c) CH 2 O d) NO 2 - e) H 3 PO 4 f) CBr 4 g) CH 2 FClh) C 2 H 2 I) O 3


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