1. Matter
I. States of Matter
 Kinetic Molecular Theory
 States of Matter

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

7. Matter
II. Classification of Matter
Matter Flowchart
Pure Substances
Mixtures

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

16. C. Mixtures
 Colloid
 heterogeneous
 medium-sized particles
 Tyndall effect
 particles don’t settle
 EX: milk

17. C. Mixtures
 Suspension
 heterogeneous
 large particles
 Tyndall effect
 particles settle
 EX: fresh-squeezed
lemonade

18. C. Mixtures
 Examples:
 mayonnaise
 muddy water
 fog
 saltwater
 Italian salad
dressing
colloid
suspension
colloid
solution
suspension

19. Matter
III. Properties & Changes in
Matter
Extensive vs. Intensive
Physical vs. Chemical

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

27. Matter
IV. Phase Changes
Phase Changes
Phase Change Diagrams

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

33. Phase Diagram - Water

34. Phase Diagram CO2

35. Matter
V. Separation Techniques
Filtration
Chromotography
Distillation

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.