Day 6 12-5
______
liquids and ______
gases are both fluids, but
gases can only flow if …
Polar
bond(s)?
HCl
SiS2
BCl3
NH3
Polar
molecule?
Intramolecular forces are bonds inside of
molecules that hold different atoms
together (like the force between a carbon
and oxygen atom in CO2).
List as many intramolecular forces as
you can think of:
I. Forces Determine Phase
A. Intramolecular Forces
1. Intramolecular forces are forces
within
_______ molecules.
2. Hold atoms
______ together; nonpolar
_________ and
polar
______ bonds
type __
of compound
3. Determine _____
___________
4. Dependent upon electronegativity
_________________
differences between bonded atoms
5. Contribute to phase determination
since intramolecular bonds determine
polarity
________
B. Intermolecular forces
1. Intermolecular forces are forces
between
different molecules.
________ _________
different __________
molecules together
2. Hold _________
3. Determine phase; type of force
polarity of molecules
depends upon ________
C. Relative Strengths of Forces by Phase
solids
1. Strongest forces found in ______;
gases
weakest forces found in ______
a. melting points - increase
________ with
increase in the strengths of
an ________
intermolecular forces
b. boiling points – the stronger
________ the
intermolecular forces the higher
_______
the boiling point
C. Relative Strengths of Forces by Phase
2. Consider several properties of the
different phases as evidence of force
strength:
a. Entropy - solids  organization comes
from strong bonds  ionic crystals; gases
 weak bonds allow them to be free
b. Ability to hold shape or volume solids  strong bonds  rigid shapes; liquids
 fairly strong bonds  flexible shapes; gases
 weak bonds  variabale shape and volume
c. Diffusion / dissolving rates - solids 
slow  strong bonds hold particles together;
gases  fastest  weaker bonds allow freedom
to mingle
d. Fluidity - solids  bonds are too strong to
allow for flow; liquids + gases  can flow since
attractions are weaker
Bent
Linear
Intermolecular forces
Entropy
Polar molecule
Intramolecular force
Electronegativity Trigonal planar
Pyramidal
VSEPR theory
Lone pair of electrons
Tetrahedral
Read section 8.4 and answer #s 33, 36,
and 38 (be sure to answer all of the
questions for 38) on page 253
e. Smell - solids  toughest to smell  strong
bonds hold particles together making it harder
for them to escape and fly into your nose
f. Reaction rates - gases  fastest reaction
rates  weakest bonds give them the least
obstacles to overcome with activation energy
List the states of matter in order of increasing:
Diffusion rate
Entropy
Reaction rate
Intermolecular attraction
1. The boiling point of acetone is much lower
than that of water. What can you deduce
about the intermolecular forces in acetone
compared to water? Explain!
- Use your notes if necessary
Day 1 12-8
Read section 8.4 and answer #s 33, 36,
and 38 (be sure to answer all of the
questions for 38) on page 253
Practice 1 Unit 5
II. Types of Intermolecular Forces
A. Ion-Dipole Forces
1. Ion-dipole forces exist between an
___
ion and a ______
polar __________
molecule
2. Diagram an example: NaCl dissolved
in H2O
B. Dipole-Dipole Forces
1. Dipole-dipole forces exist between
polar __________
molecules
______
2. The dipole moment is the measure
of the separation
__________ of the + & - charges.
greater
a. Higher value indicates ________
polarity
lesser
b. Lower value indicates ______
polarity
3. Diagram an example: carbon monoxide
D. Induced dipole - ___________________
temporary dipole in a
____________________________________
nonpolar molecule usually caused by brining
____________________________________
it near a polar molecule
1. Exists in a molecule that is normally
nonpolar
_________.
temporary
2. Induced dipoles are ___________.
D. Induced dipole - ___________________
temporary dipole in a
____________________________________
nonpolar molecule usually caused by brining
____________________________________
it near a polar molecule
Soluble O2
Ex.– (+) pole
of water
(-)
temporarily
attracts the
elecs. of O2
O
H
(+) (-)
H
electrons
O O
(+)
BINDERS