1. STATES OF MATTER #1 ATTRACTIONS
The Van der Waals attraction (London Dispersion):
Temporary (induced) dipole – transient.
Occurs in all particles.
The major attraction in NONPOLAR substances.
BECOMES STRONGER AS MOLECULAR MASS INCREASES.
As molecular mass increases
GREATER temporary polarity
CAUSES
More electrons in the particle
CAUSES
CAUSES
EFFECTS OF STRONGER ATTRACTIONS.
HIGHER BOILING TEMP.
HIGHER MELTING TEMP
INCREASING HARDNESS OF SOLID STATE.
STRONGER INDUCED DIPOLE ATTRACTIONS
CAUSES

2. The Van der Waals attraction (London Dispersion):
VERY IMPORTANT IN NON-POLAR COVALENT SUBSTANCES INCLUDING H2,O2,N2,Cl2,Br2,I2,F2 and CO2 and CH4.
THE PREDOMINANT ATTRACTION IN THE METALLIC SUBSTANCES (Au, Ag, Cu, Zn, Na etc), WHERE IT IS VERY STRONG AS MANY METALS HAVE LARGE ATOMIC MASSES.
As molecular mass increases
CAUSES
More electrons in the particle
GREATER temporary polarity
STRONGER INDUCED DIPOLE ATTRACTIONS
EFFECTS OF STRONGER ATTRACTIONS.
HIGHER BOILING TEMP.
HIGHER MELTING TEMP
INCREASING HARDNESS OF SOLID STATE.

3. THE DIPOLE ATTRACTION
AN INTERMOLECULAR ATTRACTION BETWEEN THE δ- AND δ+ POLES OF A POLAR COVALENT MOLECULE.
2. POLAR COVALENT SUBSTANCES HAVE PERMANANT DIPOLAR MOLECULES, THE DIPOLE ATTRACTION IS NOT PERMANENT.
DIPOLE ATTRACTIONS ARE STRONGER THAN Van der Waals attractions.
THE STRENGTH OF DIPOLES INCREASES WITH IONIC CHARACTER.

4. The DIPOLE-DIPOLE ATTRACTION (POLAR ATTRACTION):
DIPOLE-DIPOLE (POLAR or DIPOLE) ATTRACTIONS, IN COVALENT POLAR MOLECULES that INCLUDE SO2 AND H2S.
AS IONIC CHARACTER INCREASES
GREATER MOLECULAR polarity
CAUSES
GREATER BOND POLARITY
CAUSES
CAUSES
EFFECTS OF STRONGER ATTRACTIONS.
HIGHER BOILING TEMP.
HIGHER MELTING TEMP
INCREASING HARDNESS OF SOLID STATE.
STRONGER DIPOLE ATTRACTIONS
CAUSES

5. THE HYDROGEN BOND ATTRACTION
A VERY STRONG DIPOLE ATTRACTION THAT OCCURS WHEN H IS BONDED TO F,O,N IN AN ASYMETRICAL MOLECULE.
IT IS NOT A TRUE BOND.
IS UNUSUAL IN THAT IT HAS A BOND LENGTH, CAUSES H2O TO EXPAND ON FREEZING.
BECOMES STRONGER WITH INCREASING IONIC CHARACTER OF THE MOLECULE.
THE δ- OF OXYGEN ATTRACTS TO A + ION
THE δ+ OF H ATTRACTS TO A – ION,
IONIC
CRYSTAL LATTICE
H-BOND BETWEEN δ- AND δ+

6. H BOND ATTRACTION δ+ δ- δ+ δ- δ+ δ- δ+ δ- δ+ δ- δ+ δ-
The white arrows represent H-bonds which:
-order the molecules into a crystal formation.
-cause spacing between the molecules in the solid phase – causes expansion of ice.. H
OXYGEN δ+ δ- H
OXYGEN δ+ δ- H
OXYGEN δ+ δ- H
OXYGEN δ+ δ- H
OXYGEN δ+ δ- H
OXYGEN δ+ δ-

7. MOLECULE TO ION ATTRACTION ATTRACTION
MOLLECULE ION ATTRACTIONS ARE VERY STRONG AND HARD TO BREAK, MAKING THE SEPARATION OF WATER AND SALTS CONSUME LARGE AMMOUNTS OF ENERGY. H
OXYGEN δ+ δ- H
OXYGEN δ+ δ- H
OXYGEN δ+ δ-
THE MOLLECULE TO ION ATTRACTION BETWEEN THE δ- OF THE OXYGEN POLE OF WATER AND THE + ION.
- ION
THE MOLLECULE TO ION ATTRACTION BETWEEN THE δ+ OF THE HYDROGEN POLE OF WATER AND THE – ION.
+ ION H
OXYGEN δ+ δ- H
OXYGEN δ+ δ- H
OXYGEN δ+ δ-

8. ELECTROSTATIC (IONIC) ATTRACTION
Electrostatic ATTRACTIONS STTRACT POSITIVE IONS TO NEGATIVE IONS IN A CRYSTAL LATTICE SOLID WHERE:
THE IONS CANNOT MOVE AND THUS CANNOT CARRY A CHARGE (CONDUCT).
THE ATTRACTIONS ARE SO STRING THAT THE CRYSTAL IS HARD AND BRITTLE WITH VERY HIGH MELTING AND BOILING POINTS.\
WHEN THE IONS DISSOLVE IN WATER, THEY CAN CARRY A CHARGE.
Na+
The lines represent the electrostatic attraction. Notice the ions are in a regular, predicable geometrical arrangement. There is no randomness (LOW ENTROPY)
Cl-

9. Fracture planes of ionic crystals, brittleness.

10. ORDERING OF MELTING AND BOILING POINTS
INCREASING MELTING AND BOILING POINTS 
NON-POLAR COVALENT
- Order based on molar mass.
POLAR COVALENT
- Order based on ionic character
IONIC
- Order based on ionic character
COVALENT NETWORK
SiO2
C(s) diamond
METALLIC
ORDER METALS BASED ON MASS