1. Chapter 10: States of Matter
⢠Kinetic Molecular Theory: the idea that
particles of matter are always in motion;
this applies to all states of matter
⢠Used to explain properties of matter in
terms of energy
2. Ideal Gas
= hypothetical gas that perfectly fits all 5 assumptions of
the Kinetic Molecular Theory:
1) Gases consist of a large # of particles that occupy a
larger space with respect to their relative sizes thus
gases can be easily compressed
2) Collisions b/t particles and walls are perfectly elastic
( = no loss of KE)
3) Gas particles are in rapid, random, constant motion
4) There are no forces of attraction b/t gas particles
5) Temperature of a gas depends on the average
KE of the particles; directly proportional
A gas that is always a gas - Doesnât exist!
3. Characteristics of Gases
⢠Expansion: no definite shape or volume; fill any container,
regardless of shape
⢠Fluidity: particles slide easily over one another; act like
liquids, thus they are both fluids
⢠Low Density and Compressibility: volume can be
decreased greatly
⢠Diffusion: since gases are always randomly moving, freely
mix together with other gases
⢠Effusion: process by which gases move out of a small
opening; molecules with low mass effuse more quickly than
those with larger masses
KE= ½ mv2
4. Liquids
⢠Least common state of
matter in universe; not so
on Earth
⢠Operate at slim range of
temps/pressures
⢠Volume, shape, density?
⢠Particles in constant
motion, and closer than
those of a gas (d/t
intermolecular forces
5. Other Characteristics of liquids:
⢠Have a very high density when compared to
gases; depends on temperature ď lower
tempâŚexcept for water
⢠Not easily compressed
⢠Easily diffuse in other liquids it can dissolve
in d/t⌠much slower than it is in gases â
why?
6. Surface Tension
⢠All liquids exhibit surface
tension = a force that tends to
pull adjacent particles at a
liquids surface together,
decreasing its surface area to
the smallest possible size;
meniscus
⢠Results from⌠water shows
high surface tension
⢠Capillary action = attraction of
a liquid to a solid; rises in a
small tube against gravity
7. Surface Tension
Look at the picture below. The milk forms small droplets that
resemble a crown. But why does this happen?
Because of the surface tension of water, which keeps the
droplets spherical.
8. Some terms:
solid liquid gas
MELTING BOILING
FREEZING CONDENSATION
0ÂşC 100ÂşC
melting/freezing point boiling/condensation point
(ice) (steam)(water)
SUBLIMATION
9. More info on Liquids
⢠Vaporization â liquid to
gas
⢠Evaporation â escape
from a non-boiling
liquid at its surface
⢠Boiling â vaporization
through the entire liquid
⢠Freezing â physical
change from liquid to
solid through the loss
of HEAT. Evaporation- a beautiful process.
10. Solids
⢠Particles in a solid are tightly-
packed together due to attractive
forces. Highly-ordered.
⢠Atomic/molecular motion is
restricted, but it occurs.
⢠2 types:
1) Crystalline: consists of crystals
(orderly, geometric, repeating
pattern)
2) Amorphous: particles are
randomly arranged
Sodium Chloride crystals
Amorphous solid
11. Properties of solids
⢠Definite shape and volume
⢠Definite melting point (d/t addition of heat)
⢠High density and incompressible
⢠Low rates of diffusion
12. Crystals
⢠Arranged in a lattice structure
⢠Smallest unit of a crystal that shows the 3-
D pattern of the lattice = UNIT CELL
13. Changes of State
⢠Phase = any part of a
system that has a
uniform composition
and properties
⢠Condensation =
process by which a
gas turns into a liquid
⢠Vapor = a gas in
contact with its liquid
or solid phase
14. Vapor Pressure
⢠The pressure exerted by a vapor that is in
equilibrium with its corresponding liquid
⢠Develops in a closed system
⢠Increase AKE, increase particles leaving
liquid, increased pressure
⢠Volatile liquids evaporate
easily d/t weak IMF
16. Notes on Boiling Point
⢠BP = when vapor pressure
equals atmospheric pressure
⢠Increase pressure, increase
BP = pressure cooker
⢠Molar Enthalpy of
Vaporization = amount of
heat needed to vaporize 1
mole of a liquid at the liquidâs
BP at a constant pressure; the
stronger the attractionâŚ.
⢠Vapor pressure is directly
proportional to temperature
⢠Vacuum evaporator â how
does it work?
17. Freezing and Melting
⢠Definitions?
⢠What is the difference b/t freezing water
and ice? Boiling water and steam?
19. More Vocab
⢠Molar Enthalpy of Fusion = the amount
of heat required to melt one mole of a
solid
(40.79 kJ/mol for water)
⢠Sublimation vs. deposition
20. Phase Diagrams
graph of pressure vs. temperature that shows the conditions
under which the phases of a substance would exist
21. Water
⢠Most abundant liquid
on Earth; essential to
life; most reactions
take place in it
IMPORTANT!!!
⢠Review its structure
and propertiesâŚ