MATTER

1. Matter

2. A) Classification of Matter
 Review of prior knowledge:
 Talk with your shoulder partner, how is matter
classified?

3. Some Criteria for the
Classification of Matter
 Properties
 State (solid, liquid, gas)
 Composition

4. Properties
Intensive
-DOES NOT
depend on
amount of
matter.
Extensive
-DOES depend
on amount of
matter present.

5. Intensive and Extensive
Properties
Sulfur

6. Properties of Matter fall under
two categories: Intensive and
Extensive
Extensive properties depend on the quantity of matter Intensive properties do not depend
on the quantity of matter.
Extensive Properties
are:
Length Width Height
Area Volume
Surface Area
Color Intensity or
Absorbance
Intensive Properties are:
Density Viscosity
Melting Point (same value as Freezing Point)
Boiling Point (same value as Condensation
Point)
Hardness (often interchangeably used as
Tensile Strength)
Malleability (Bending ability of metals)
Ductility (Ability of metals to be drawn into
wires)

7. Properties
Physical: observed without
without changing the composition
of the substance.
Chemical: the ability of a
substance to undergo a specific
chemical change

8. Examples of Physical
Properties
Color, odor, hardness, density,
melting point, boiling point, state,
solubility.

9. Substance State Color Melting
Point (C°)
Boiling
Point (C°)
Density
(g/cm3
)
Oxygen O2 Gas Colorless -218 -183 0.0014
Mercury Hg Liquid Silvery-
white
-39 357 13.5
Bromine Br2 Liquid Red-brown -7 59 3.12
Water H2O Liquid Colorless 0 100 1.00
Sodium
Chloride
NaCl Solid White 801 1413 2.17
Example: Physical Properties

10. STATES OF MATTER
The Five States of Matter
Solid
Liquid
Gas
Plasma
Bose-Einstein Condensate

11. STATES OF MATTER
 Based upon particle arrangement
 Based upon energy of particles
 Based upon distance between particles

12. STATES OF MATTER
SOLIDS
•Particles of solids
are tightly packed,
vibrating about a
fixed position.
•Solids have a
definite shape and a
definite volume. Heat

13. STATES OF MATTER
LIQUID
 Particles of liquids
are tightly packed,
but are far enough
apart to slide over
one another.
 Liquids have an
indefinite shape
and a definite
volume.
Heat

14. STATES OF MATTER
GAS
 Particles of
gases are very
far apart and
move freely.
 Gases have an
indefinite
shape and an
indefinite
volume.
Heat

15. Phase Properties
Phase
Particle Properties
Proximity Energy Attraction Volume Shape
Solid
Liquid
Gas
close little strong definite definite
close moderate moderate definite indefinite
far apart a lot weak indefinite indefinite

16. But what happens if you raise
the temperature to super-high
levels…
between
1000°C and 1,000,000,000°C ?
Will everything
just be a gas?

17. STATES OF MATTER
PLASMA
 A plasma is an
ionized gas.
 A plasma is a
very good
conductor of
electricity and is
affected by
magnetic fields.
 Plasmas, like
gases have an
indefinite shape
and an indefinite
volume.

18. STATES OF MATTER
SOLID LIQUID GAS PLASMA
Tightly packed, in
a regular pattern
Vibrate, but do not
move from place
to place
Close together
with no regular
arrangement.
Vibrate, move
about, and slide
past each other
Well separated
with no regular
arrangement.
Vibrate and move
freely at high
speeds
Has no definite
volume or shape
and is composed
of electrical
charged particles

19. Some places where plasmas are
found…
1. Flames

20. 2. Lightning

21. 3. Aurora (Northern Lights)

22. The Sun is an example of a star in its
plasma state

23. But now what happens if you lower the
temperature way, way, down to
100 nano degrees above
“Absolute Zero” (-273°C)
Will everything
just be a frozen
solid?

24. Not Necessarily!
In 1924 (82 years ago), two scientists, Albert
Einstein and Satyendra Bose predicted a 5th
state of matter which would occur at very
very low temperatures.
Einstein Bose
+

25. The 5th
state of matter:
Bose-Einstein Condensate
Finally, in 1995 (only 11
years ago!), Wolfgang
Ketterle and his team of
graduate students
discovered the 5th
state of
matter for the first time.
Ketterle and his students

26. In a Bose-Einstein condensate, atoms
can no longer bounce around as
individuals.
Instead they must all act in exactly the
same way, and you can no longer tell
them apart!

27. A computer image of a Bose-Einstein Condensate

29. Change of Phase
Melting solid  liquid
Condensation gas  liquid
Freezing liquid  solid
Evaporation liquid  gas
Sublimation solid  gas
Boiling: Evaporation occurring beneath the
liquid’s surface.

30. Is changing phase a physical
or chemical change?
Review of prior knowledge:
Talk with your shoulder partner and be
prepared to share out

31. Classification of Matter
(by composition)

32. Classification of Matter
by Composition
1) made of one type
of particle
2) All samples show
the same intensive
properties.
1) made of multiple
types of particles
2) Samples may
show different
intensive
properties.
32

33. (Pure) Substance
Matter that has a uniform and
definite composition.
Elements
Compounds

34. Classification of Pure Substances
1) made of one
type of atom
(some
elements
found as multi-
atom
molecules in
nature)
2) combine
together to
make
compounds
1) made of one
type of
molecule, or
array of ions
2) units contain
two or more
different kinds
of atoms
34

35. Mixture: a physical blend of two or
more substances that are not
chemically combined.
Homogeneous
Heterogeneous

36. Classification of Mixtures
1) made of
multiple
substances,
but appears
to be one
substance
2) All portions of
an individual
sample have
the same
composition
and
properties.
1) made of
multiple
substances,
whose
presence can
be seen
2) Portions of a
sample have
different
composition
and
properties.
36

37. Copper II Sulfate and its
solution in water.

38. Example: Stainless Steel
A homogeneous
mixture of:
-Iron (Fe)
-Chromium (Cr)
-Nickel (Ni)

39. Example: Gaseous Mixture
Elements argon and nitrogen and
a compound (water vapor).

40. Heterogeneous Mixtures
Non-uniform composition
throughout the mixture
Two or more phases.
Example:
Oil and vinegar

41. Note:
Mixtures can be physically
separated.
Mixtures exhibit physical
properties similar to the
components of the mixture.

42. Separation Methods
Use differences in the physical
properties of the components of
the mixture.

43. Example: Separate iron filings
from sulfur using a magnet.

44. Filtration: separates a solid from a
liquid in a heterogeneous mixture

45. Distillation:
-separate dissolved solids from a liquid
-uses boiling and condensation.

46. Distillation of Crude Oil
(Refining)
Crude Oil is a mixture of Hydrocarbons

47. Distillation of Crude Oil

48. c) Elements and Compounds

49. Elements
The simplest substances.
Can not be separated into simpler
substances.
Building blocks of all matter.
More than 100 known elements.
Represented by chemical
symbols.

50. Chemical Symbols of Elements
System started by Jons Berzelius
(Sweden, 1779-1848)
One or two first letters of name of
the element.
Many elements names have roots
from: Latin, Greek, mythology,
geography, names of scientists.

51. Examples:
 Americium, Am
 Einsteinium, Es
 Bromine, Br
 Helium, He
 Lead(Plumbum), Pb
 Niobium, Nb
 Iron (Ferrum), Fe
 Mendelevium, Md

52. Compound
A substance that contains two or more
elements chemically combined.
Compounds have different properties
from the individual substances.
(Ex: H2O)

53. Example: H2O

54. Substance or mixture?
If composition is fixed and may
not changesubstance

56. d) Chemical Properties
and Chemical Changes

57. H2O composition is fixed-
compound
Gaseous Phase Liquid Phase

58. Chemical Properties
The ability of a substance to
transform into a new substance
(to undergo a chemical change).
Example: Magnesium reacts with
oxygen to form magnesium
oxide.

59. Magnesium Mg

60. Burning of Magnesium
2Mg+ O2 2MgO

61. Physical Changes
Physical change: a change in the
physical properties of a substance.
Composition does not change.
May be reversible or irreversible.
Examples:
Reversible:
Irreversible:

62. Chemical Change
A change that produces matter with a
different composition than the original
matter.
Atoms rearrange themselves into new
combinations.

63. Burning of Methane
CH4 +2O2 CO2 + 2H2O

64. Burning of Methane
CH4 + 2O2 CO2 + 2H2O

65. Recognizing a Chemical Change
energy exchange
production of a gas
color change
formation of a precipitate

66. Formation of a Precipitate
Cu(OH)2
Precipitate

67. The Law of Conservation of Mass
(Antoine Lavoisier)
In any chemical or physical
change, mass is neither
created or destroyed
Mass is CONSTANT