2. Intermolecular forces are much weaker than the
intramolecular forces of attraction but are important
because they determine the physical properties of
molecules like their:
Boiling point- temperature
Melting point- change in temperature
Density- weight
Enthalpies of fusion
- The heat which a solid absorbs when it
melts.
3. Types of intermolecular forces that exist
between molecules
Dipole-dipole interactions ION-dipole interactions
London dispersion forces HYDROGEN BONDING
4. Van Der Waals Force
-Proposed by Johannes van der Waals
-distance dependent interactions.
occur when adjacent atoms come close enough
that their outer electron clouds just barely touch.
This action induces charge fluctuations that
result in a nonspecific, nondirectional attraction.
These interactions are highly distance dependent,
decreasing in proportion to the sixth power of the
separation.
6. • Electrons in atoms have different distributions depending on which one
you choose.
• They come in pairs and have specific energies that define the state they
are in.
10. LONDON DISPERSION FORCE
• Are weak attractions that results from the temporary dipoles of molecules.
All molecules have London Dispersion Forces.
• It is how nonpolar molecules can be attracted to each other.
• MIGHT be called van der Waals by other sources.
• How noble gases can have other states.
• Weaker as distance increases.
• Proposed by Fritz London
14. • The attraction of bond dipoles
(Unequal sharing of electons)
from covalently bonded atoms.
• Only polar molecules.
• Stronger than London Dispersion
Forces.
16. ION POLAR
SLIGHT
SLIGHT
Ion-Dipole Force
• electrostatic interaction
involving a partially charged
dipole of one molecule and a
fully charged ion
• strength of the force is
proportionate to ion charge
18. Hydrogen Bonding
• forces created when a hydrogen atom bonded to an electronegative atom
approaches a nearby electronegative atom
• a relatively strong force of attraction between molecules
• greater electronegativity of the hydrogen bond acceptor will create a
stronger hydrogen bond
19. Intermolecular
force
Occurs between … Relative strength
Dipole-dipole
attraction
Partially
oppositely
charged ions
Strongest
Hydrogen
bonding
H atom and , N,O
or F atom
As strong as
dipole-dipole
attraction
London
dispersion
attraction
Temporary or
induced dipoles
Weakest
Relative strength of intermolecular forces of
attraction
20. How forces of
attraction affect
properties of
compounds?
the stronger the
intermolecular forces of
attraction,
the more energy is required to
break those forces
30. answErs
1-3: BOILING POINT, Melting point, Density, enthalpies of fusion
and vaporization
4: OXYGEN, Nitrogen, Fluorine
5: Johannes van der waals
6: Fritz London
7: London dispersion force
8: HYDROGEN BONDING
9: DIPOLE-DIPOLE
10:BONUS
Editor's Notes
Clear up misconception. Electrons are not found on a single spot.
Helium is a noble Gas and nonpolar. Kaya walang mga “Helium Dioxide”. Electrons are always moving.
This is not permanent because electrons are always moving. Dipoles are molecules/atoms with positive and negative region.
Electrons are always moving. London dispersion force.
Nonpolar covalent bonds, with equal sharing of the bond electrons, arise when the electronegativities of the two atoms are equal.
“When temperature increases electrons get more excited and their speed increase. ”
Larger atoms have higher energy shells (S,P,D,F).
Water is a polar molecule.
This is not permanent because electrons are always moving. Dipoles are molecules/atoms with positive and negative region.
Ion-dipole forces are generated between polar water molecules and a sodium ion. The oxygen atom in the water molecule has a slight negative charge and is attracted to the positive sodium ion. These intermolecular ion-dipole forces are much weaker than covalent or ionic bonds.