molecular geometry 3-d arrangement of molecules
TRANSCRIPT
Molecular Geometry
3-D arrangement of molecules
VSEPR Theory
Valence-shell, electron-pair repulsion
Def: repulsion b/ valence e- pairs around atom causes them to be as far apart as possible
Shapes
NO lone pairs on CENTRAL atom
Symmetrical Linear Trigonal-Planar Tetrahedral Trigonal-
bipyramidal Octahedral
WITH lone pairs on CENTRAL atom
Non-symmetrical Trigonal-pyramidal Bent (angular)
Shapes – NO lone pairs on central atom
1. Linear (AB2):
• A – central atom B-bonded atoms- 3 atom molecules CO2
- 2 atom molecules, O2, HCl, etc.
- bond angles: 180o
Shapes – NO lone pairs on central atom
2. Trigonal Planar (AB3):
- BCl3- bond angles: 120o
Shapes – NO lone pairs on central atom
3. Tetrahedral (AB4):
- CCl4- bond angles: 109.5o
Shapes – NO lone pairs on central atom
4. Trigonal-bipyramidal (AB5):
- PCl5- bond angles: 120o and 90o
Shapes – NO lone pairs on central atom
5. Octahedral (AB6):
- SF6
- bond angles: 90o
Shapes – WITH lone pairs on central atom
6. Trigonal-Pyramidal (AB3E):
• A – central atom B – bonded atoms E – lone pair- NH3
- triangular sides - bond angles: 107o
Shapes – WITH lone pairs on central atom
7. Bent or Angular (AB2E2):
- H2O
- bond angles: 105o
Molecular Polarity
Polarity of each bond Molecular polarity
Molecular Polarity
1. Has ALL bonds NONPOLAR nonpolar molecule
2. Has bonds nonpolar AND polar polar molecule
3. Has ALL bonds POLAR depends on shape
Symmetrical shape (linear - octahedral) NONPOLAR
Non-symmetrical shape (bent & trigonal pyramidal) POLAR
Molecular Polarity Examples
CCl4 PH3
CBr3H
Intermolecular Forces
Intermolecular Forces
“between molecule” forces Generally weaker than bonds b/
atoms Boiling point – good to measure
intermolecular forces
Dipole-Dipole Forces
Dipole- equal but opposite charges separated by a short distance
Video 124H Cl
Dipole-Dipole Forces
Induced Dipole: polar molecule makes a dipole on a nonpolar molecule
Ex: O2 dissolved in H2O Weaker than regular dipole forces
Hydrogen Bonding
Type of dipole-dipole force Def: H-atom bonded to highly e-neg
atom is attracted to lone pair of the e-neg atom in nearby molecule
Ex: HF, H2O, NH3
Hydrogen Bonding
London Dispersion Forces
Def: constant motion of e-s and creation instantaneous dipoles
Video 133