1 Shapes of Molecules Determined by number of valence electrons of the central atom 3-D shape a result of bonded pairs and lone pairs of electrons Use.

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Presentation transcript:

1 Shapes of Molecules Determined by number of valence electrons of the central atom 3-D shape a result of bonded pairs and lone pairs of electrons Use VSEPR theory (valence-shell-electron-pair repulsion

2 Using the VSEPR Model 1. Draw the electron-dot structure 2.Identify the central atom 3.Count the total number of electron pairs around central atom 4.Predict the electron shape 5.Predict the shape of the molecule using the bonding atoms

3 Shapes of Molecules Number of electron pairs2 (= negative charge clouds) Number of bonded atoms 2 Angle180° Name of shape linear

4 BeCl 2 Be 2 valence electrons.... : Cl : Be : Cl :.... : Cl Be Cl : linear, 180°....

5 More Electron Pairs Electron AngleBonded Name of PairsAtomsShape 3120° 3trigonal planar 3120° 2angular

6 Electron Shape with 3 Pairs

7 BF 3 B has 3 valence electrons 120° Ftrigonal planar B F

8 SO 2 S has 2 bonded atoms, 1 lone pair (electron cloud) 120°, angular : O :: S : O : S.. O

9 More Electron Pairs Electron AngleBonded Name of PairsAtomsShape 4109° 4tetrahedral 4109° 3pyramidal 4109° 2bent, angular

10 Tetrahedral CH 4 4 electron Pairs, 4 bonded atoms, 109° H H C H C H H H H H

11 NH 3 Pyramidal N has 4 electron pairs, 3 bonded H atoms Shape is called pyramidal.. H : N : H N.. HH H H..

12 H 2 O Bent or Angular O has 4 electron pairs, 2 bonded H atoms Shape is called bent or angular, 109°.. : O : H O.. H H H..

13 Learning Check Determine the molecular geometry of each of the following: A. CCl 4 1) tetrahedral 2) pyramidal3) angular B. SO 3 1) trigonal planar 2) pyramidal3) angular C. PCl 3 1) trigonal planar 2) pyramidal3) angular

14 Solution Determine the molecular geometry of each of the following: A. CCl 4 1) tetrahedral B. SO 3 1) trigonal planar C. PCl 3 2) pyramidal