Ozone Summary Notes

Dipoles

Dipole: Two opposite charges separated by a (short) distance.

The bonds are types of intermolecular bonds (bonds between molecules. Ex: H -- Cl)

Types:

• Instantaneous dipole-induced dipole (1)
• Permanent dipole - induced dipole (2)
• Permanent dipole - permanent dipole (3)

1.When two neighboring molecules do not have a permanent dipole, they are attracted. These constantly break and reform - constant change in electron distribution.

2. The charge of the permanent dipole causes a temporary change in the neighboring molecule 

3. If both molecules have a permanent dipole, there is an electrostatic attraction between the charges of the dipoles.

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How these bonds arise:

• Electrons in a molecule are in continuous random motion, and may be distributed unevenly (creating an instantaneous dipole)
• Dipole can induce another dipole (permanent-induced or instantaneous-induced)
• Electrostatic attraction between both dipoles

Factors:

• Electrons in the molecule. the higher the no. of e-, the more chance of instantaneous dipole
• Less distance between molecule = greater electrostatic attraction

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Hydrogen Bonding:

• The strongest type of intermolecular bond
• H atoms are represented as multiple lines between molecules (see O-H bond)
• 
• A d+ H atom in one molecule and a small electronegative atom (O,N or F). There is a lone pair on the electronegative atom
• The lone pair points directly at the d+ H atom. 
• There is a linear structure so the bond angle = 180 degrees.
• Liquid Water:

- Contain O atom with 2 lone pairs and 2 d+ H atoms attached. 

- Has a higher boiling point than other molecules of similar Mr values. 

• Ice (as 2 H2O molecules are shown above):

- H bonds are formed when water freezes. 

- Tetrahedral shape

- Arrangement around the O atom gives ice an open structure

- Low density, hence it floats on water

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Haloalkanes

• Boiling…