IIIIII Molecular Geometry Molecular Structure. A. VSEPR Theory  Valence Shell Electron Pair Repulsion Theory  Electron pairs orient themselves so that.

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Presentation transcript:

IIIIII Molecular Geometry Molecular Structure

A. VSEPR Theory  Valence Shell Electron Pair Repulsion Theory  Electron pairs orient themselves so that valence electrons are as far apart as possible

A. VSEPR Theory  Types of e - Pairs  Bonding pairs - form bonds  Lone pairs - nonbonding e - Lone pairs repel more strongly than bonding pairs!!!

A. VSEPR Theory  Lone pairs reduce the bond angle between atoms. Bond Angle

 Draw the Lewis Diagram.  Count up e - pairs on central atom.  double/triple bonds = ONE pair (for shape purposes only!!)  Shape is determined by the # of bonding pairs and lone pairs. Know the 8 common shapes & their bond angles! B. Determining Molecular Shape

C. Common Molecular Shapes 2 total electron pairs *2 bonding pairs *0 lone pairs LINEAR 180° BeH 2 Note: Beryllium does not follow the octet rule. Beryllium is complete with 4 valence electrons

3 total electron pairs *3 bonding pairs *0 lone pairs TRIGONAL PLANAR 120° BF 3 C. Common Molecular Shapes Note: Boron is also an exception to the octet rule. Boron is complete with 6 valence electrons

C. Common Molecular Shapes 3 total pairs *2 bonding pairs *1 lone pair BENT <120° SO 2

4 total pairs *4 bonding pairs *0 lone pairs TETRAHEDRAL 109.5° CH 4 C. Common Molecular Shapes

4 total pairs *3 bonding pairs *1 lone pair TRIGONAL PYRAMIDAL 107° NH 3 C. Common Molecular Shapes

4 total pairs *2 bonding pairs *2 lone pairs BENT 104.5° H2OH2O C. Common Molecular Shapes

5 total pairs *5 bonding pairs *0 lone TRIGONAL BIPYRAMIDAL 120°/90° PCl 5 C. Common Molecular Shapes

6 total pairs *6 bonding pairs *0 lone pairs OCTAHEDRAL 90° SF 6 C. Common Molecular Shapes

PF 3 4 total 3 bond 1 lone TRIGONAL PYRAMIDAL 107° F P F F D. Examples

CO 2 O C O 2 total 2 bonding pairs 0 lone LINEAR 180° D. Examples

IIIIII Molecular Polarity Molecular Structure

Molecular Polarity Polar Molecule: Molecule that has a partially positive end and a partially negative end. (It has electrical poles) There is an uneven distribution of electrons in the molecule

A. Dipole Moment  Direction of the polar bond in a molecule.  Arrow points toward the more electronegative atom. H Cl ++ --

B. Determining Molecular Polarity  Depends on:  dipole moments  molecular shape

B. Determining Molecular Polarity  Nonpolar Molecules  Dipole moments are symmetrical and cancel out. BF 3 F F F B

B. Determining Molecular Polarity  Polar Molecules  Dipole moments are asymmetrical and don’t cancel. net dipole moment H2OH2O H H O....

B. Determining Molecular Polarity  Polar molecules have...  asymmetrical shape (lone pairs) or  asymmetrical atoms (attached atoms are different)

B. Determining Molecular Polarity  Nonpolar Molecules have…  No lone pairs  All attached atoms are the same