2. A. Kinetic Molecular Theory
KMT
Particles of matter are always in
motion.
The kinetic energy (speed) of these
particles increases as temperature
increases.
3. B. Four States of Matter
Solids
very low KE - particles
vibrate but can’t move
around
fixed shape
fixed volume
4. B. Four States of Matter
Liquids
low KE - particles can
move around but are
still close together
variable shape
fixed volume
5. B. Four States of Matter
Gases
high KE - particles can
separate and move
throughout container
variable shape
variable volume
6. B. Four States of Matter
Plasma
very high KE - particles collide with
enough energy to break into
charged particles (+/-)
gas-like, variable
shape & volume
stars, fluorescent
light bulbs, CRTs
8. A. Matter Flowchart
MATTER
Can it be physically
separated?
Homogeneous
Mixture
(solution)
Heterogeneous
Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be chemically
decomposed?
noyesIs the composition
uniform?
noyes
Colloids Suspensions
9. A. Matter Flowchart
Examples:
graphite
pepper
sugar (sucrose)
paint
soda
element
hetero. mixture
compound
hetero. mixture
solution
10. B. Pure Substances
Element
composed of identical atoms
EX: copper wire, aluminum foil
11. B. Pure Substances
Compound
composed of 2 or more
elements in a fixed ratio
properties differ from those
of individual elements
EX: table salt (NaCl)
12. B. Pure Substances
Law of Definite Composition
A given compound always contains
the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different
ratios to form different compounds.
13. B. Pure Substances
For example…
Two different compounds,
each has a definite composition.
14. C. Mixtures
Variable combination of 2 or more pure
substances.
Heterogeneous Homogeneous
15. C. Mixtures
Solution
homogeneous
very small particles
no Tyndall effect
Tyndall Effect
particles don’t settle
EX: rubbing alcohol
20. A. Extensive vs. Intensive
Extensive Property
depends on the amount of matter
present
Intensive Property
depends on the identity of substance,
not the amount
21. A. Extensive vs. Intensive
Examples:
boiling point
volume
mass
density
conductivity
intensive
extensive
extensive
intensive
intensive
22. B. Physical vs. Chemical
Physical Property
can be observed without changing the
identity of the substance
Chemical Property
describes the ability of a substance to
undergo changes in identity
23. B. Physical vs. Chemical
Examples:
melting point
flammable
density
magnetic
tarnishes in air
physical
chemical
physical
physical
chemical
24. B. Physical vs. Chemical
Physical Change
changes the form of a substance
without changing its identity
properties remain the same
Chemical Change
changes the identity of a substance
products have different properties
25. B. Physical vs. Chemical
Signs of a Chemical Change
change in color or odor
formation of a gas
formation of a precipitate (solid)
change in light or heat
26. B. Physical vs. Chemical
Examples:
rusting iron
dissolving in water
burning a log
melting ice
grinding spices
chemical
physical
chemical
physical
physical
28. Phase Changes
Are Physical Changes
Most substances can exist in 3 states
(Solid, Liquid, Gas)
Temperature and pressure determine
the state of matter.
29. Phase Changes
States of matter are called Phases
when they exist together as physically
different parts of a mixture.
For example: Ice water is a
heterogeneous mixture of 2 phases –
it exists as a liquid and a solid
together.
When energy is added or removed,
one phase can change into another
30. Phase Changes Requiring Energy
Melting – solid to liquid
Vaporization – liquid to a gas
Sublimation – solid to gas
These phase changes require energy
to be added to the system.
31. Phase Changes the Release Energy
Condensation – gas to liquid
Deposition – gas to solid
Freezing – liquid to solid
These phase changes require energy
to be removed from the system.
32. Phase Diagrams
Phase diagram shows phase of matter
at different temperatures and
pressures
Each substance unique
There is usually a “Triple Point”
where all three phases can coexist
“Critical Point” – temperature and
pressure at which above substance
cannot exist as liquid
36. Filtration
To separate an insoluble solid from a
liquid. The solid remains in the filter
paper and the liquid goes through the
paper into the beaker.
37. Chromotography
Used to separate small amounts of liquids from
each other, such as to separate different colored
dyes that make up the ink in a marker.
Some dyes are more soluble than others, the
dyes travel up the chromatography paper at
different distances.
The more soluble dyes move further up the paper
than the less soluble ones, and you can see the
separation of the colors.
38. Is used to separate and
collect a liquid from the solid
that is dissolved in it.
The solution is heated in a
flask until the liquid boils.
The gas produced passes
into the condenser where it
is cooled and condenses to
a liquid.
The pure liquid (distillate) is
collected in a beaker.
Distillation
39. Other Separation Techniques
Evaporation – Is used to separate and collect a
soluble solid out of a liquid it is dissolved in. The
solution is heated until the liquid boils. When the
liquid has boiled away, the solid remains.
Magnetism – To separate a magnetic particle
from a non-magnetic particle. A strong magnet is
passed over the mixture, which collects the
magnetic particle and leaves the other particle(s)
behind.