Structure and Bonding - Chapter 4
- Created by: lindseyreidxo
- Created on: 04-04-17 14:43
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- Structure and Bonding
- London Dispersion Forces
- Weakest of all Van der Vaal forces
- The atom or molecule gets sightly charged ends known as a temporary dipole.
- This charge can then induce an opposite charge in a neighbouring atom or molecule called an induced dipole.
- The oppositely charged ands attract each other creating intermolecular bonds
- This charge can then induce an opposite charge in a neighbouring atom or molecule called an induced dipole.
- uneven distribution of electrons
- www.tutorhelpdesk.com
- Permanent Dipole Interactions
- a molecule which has permenantly charged ends.
- these forces are stronger than London dispersion forces.
- http://www.bbc.co.uk/bitesize/higher/chemistry/energy/bsp/revision/2/
- Polar Polar Molecules
- A polar molecule is a molecule which has a permanent slightly positive charge on one side and a permanent slightly negative on the other.
- The side with the higher the electro -negativity will be the side with the negative charge as it has a stronger pull on the electrons.
- When molecules have equal charges on each side it would be non-polar.
- http://users.stlcc.edu/gkrishnan/polar.html
- Hydrogen Bonding
- Hydrogen bonds are permenant dipole interactions found between molecules which contain highly polar bonds.
- They are usually found in molecules when H is bonded to either Fluorine, Nitrogen or oxygen.
- When H bonds are present the compound will have a much higher melting point and boiling point.
- London Dispersion Forces
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