1. Chapter 3: Matter—Properties
and Changes
Section 3.4 Types of Matter
Elements & Compounds

2. What is matter?
• Anything that has mass and
takes up space
• Mass is a measurement of the
amount of matter in an object. It
is different than weight which
measures the amount of matter
AND the gravitational pull on an
object.

3. Now that you’re an expert, which of the
following is matter?
Matter Not
1. A book Matter
2. A house
3. A thought
4. Your brain
5. Light
6. Your cell phone
7. Radio waves

4. There is so many different kinds of
matter, that we need to organize it.
 Substances have a uniform and unchanging
composition
examples: salt,
water,
sugar

5. Chemical symbols
• Make it easy to write the formulas for chemical
compounds
• Ex: salt water
NaCl
H 2O

6. Elements
• A pure substance that cannot be broken down
into simpler substances by physical or
chemical means
• 91 naturally occurring elements
• Symbolized by one capital letter or one
capital letter and 1 lower case
– ex: S = sulfur
– Na = sodium
• In mid 1800’s, no chart for organizing the
elements that were known at the time

7. Dmitri Mendeleev--1869
-Organized the known
elements into a table of
rows and columns based
on their similarities and
masses.

8. Periodic table
• Organized into horizontal rows called
periods and vertical columns called families
• Called “periodic” because properties of
elements repeat as you move from period to
period
• Mendeleev’s table left blank spaces for
elements yet to be discovered and predicted
their properties

9. Compounds
• A combination of 2 or more different elements
that are combined chemically
• Most of the matter in the universe are
compounds
• Ex: water (H2O), sugar (C12H22O11), salt (NaCl),
aspirin (C9H8O4)

10. Compounds
• Can be broken down into simpler
substances by chemical means
• Usually requires energy

11. Compounds
• Properties of a compound are different from
its component elements
• Ex: water—liquid at
room temp.
Hydrogen—a
colorless,
tasteless gas
Oxygen—a
colorless,
tasteless gas

12. Sodium chloride
• As a compound, it is a white, unreactive
solid that adds flavor to food
• Its component elements:
Chlorine—poisonous, pale,
green gas Sodium—a highly
reactive element
that fizzes in water

13. States of Matter
Classification based upon the following:
 Particle arrangement
 Energy of particles
 Distance between particles
State of matter is dependent on
temperature and pressure of the
surroundings

14. 3 states of matter

15. States of Matter
1. Solid—has a definite shape and volume
exs: wood, desk, shoes, sugar
-particles are tightly packed,
incompressible

16. States of Matter
2. Liquids—have a constant volume,
-no definite shape
-takes the shape of its container
-particles are not held rigidly in place,
allows material to
flow

17. States of Matter
3. Gases—have no definite shape or
volume
-particles are very far apart
-particles are easily compressed

18. Section 3.3
Mixtures of Matter

19. Mixtures
• A combination of 2 or more pure substances
in which each pure substance retains its
individual chemical properties.

20. Types of Mixtures
1. Heterogeneous—individual substances
remain distinct

21. Types of Mixtures
2. Homogeneous—has a constant
composition throughout
-called a solution

22. Types of Solutions
• Gas-gas: air
• Gas-liquid: soft drinks
• Liquid-gas: moist air
• Liquid-liquid: vinegar
• Solid-liquid: Crystal Light
• Solid-solid: steel (called
“alloys”—mixture of metals
producing greater strength)

23. Separating Mixtures
1. Physical separation:
hand selection or
pouring through sieves

24. Separating Mixtures
2. Filtration—uses a
porous barrier to separate
a solid from a liquid

25. Separating Mixtures
3. Distillation—based on
differences in the
boiling points of the
substances involved

26. Separating Mixtures
4. Crystallization—results
in the formation of pure
solid particles of a
substance from a solution
containing the dissolved
substance

27. Separating Mixtures
5. Chromatography—
separating the
components of a mixture
based on the tendency of
each to travel across the
surface of another
material.

28. Matter
Pure
Mixtures
substances
Heterogeneous Homogeneous
Mixtures Mixtures
Elements Compounds
Dirt, blood, Lemonade, Oxygen, gold, Salt, baking
milk gasoline, steel iron soda, sugar

29. Section 3.1
Properties of Matter

30. Physical Properties of Matter
 A characteristic that can be observed
or measured without changing the
composition of the sample
 Properties such as density, color, odor,
taste, hardness, melting point, boiling
point

31. Physical Properties of Matter: Two Types
1. Extensive: dependent on the amount of
substance present
--length, volume
2. Intensive: independent of the amount of
substance present
--density, melting point, boiling point
--used to identify substances

32. Chemical Properties
 Ability or inability of a substance to
combine with or change into one or
more other substances

33. Physical Chemical
Properties Properties
• Conducts electricity • Forms dark blue
• Malleable solution with
• Ductile ammonia
• Reddish brown • Forms green
• Shiny compound when
exposed to air
• Density = 8.92 g/cm 3
• Melting pt = 1085°C
• Boiling pt = 2570°C

34. Classify each as a physical or
chemical property:
1. Iron and oxygen form rust.
2. Iron is more dense than aluminum
3. Magnesium burns brightly when ignited.
4. Oil and water do not mix.
5. Mercury melts at -39°C.

35. Section 3.2
Changes in Matter

36. Physical Change
• Changes in a substance’s appearance, not in
composition

37. Types of physical changes:
•Bend, grind, crumple
•Split, crush, twist
•Boil, freeze, melt, vaporize
(changes of state or phase)
(.wav)

38. Chemical Changes
• A change in the composition of a
substance
• Also called a chemical change or
chemical reaction
• Ex: rust, corrode, tarnish, rot, burn,
ferment, explode, oxidize

39. become
s
The substance
has changed.
becomes

40. Evidence of Chemical Change
2. Energy change:
absorbed or released

41. 3. Odor changes
or production
4. Gas production
5. Precipitate
formation

42. Classify each as a physical or
chemical change:
1. A dead fish rotting
2. Dissolving salt in water
3. Boiling salt water until only salt remains
4. Melting steel
5. Bending steel
6. Cracking ice

43. Section 3.3 & 3.4
Laws of Matter

44. Law of Conservation of Mass
Mass is neither created nor destroyed
during a chemical reaction—it is
conserved. (Antoine Lavoisier)
Mass of reactants = Mass of products

45. Antoine Lavoisier—a
French scientist
o 1743-1794
o Father of Modern
Chemistry
o One of the first to use
an analytical balance

46. When you burn a big pile of wood, why do
you only end up with a tiny pile of ashes?

47. In an experiment, 10.00 g of red mercury (II) oxide
powder is placed in an open flask and heated until it
is converted to liquid mercury and oxygen gas. The
liquid mercury has a mass of 9.26 g. What is the
mass of oxygen formed in the reaction?

48. Practice problems—pg. 65 #6, 7, 9

49. Law of Definite Proportions
• John Dalton
• A pure substance will always have the same
percent by weight
• Ex: water (H2O) = 11.2 % hydrogen
88.8% oxygen

50. To find percent by mass:
Percent by mass = mass of element x 100
mass of compound

51. Analysis of sugar:
20.0 g sugar 500.0 g sugar
Carbon 8.44 g 42.2% Carbon 211.0 g 42.2%
Hydrogen 1.30 g 6.5% Hydrogen 32.5 g 6.5%
Oxygen 10.26 g 51.30% Oxygen 256.5 g 51.30%

52. Therefore…
• Sugar always has the same proportions of
ingredients
• If a substance has different proportions, it is
a different substance

53. A 78.8 g sample of an unknown compound contains
12.4 g of hydrogen. What is the percent by mass of
hydrogen in the compound?
Percent by mass = mass of element x 100
mass of compound

54. Practice problems—pg. 76 #21-24

55. Law of Multiple Proportions
• When different compounds are formed
using the same elements, different masses
of one element combine with the same
relative mass of the other element in small,
whole number ratios.

56. Carbon monoxide/carbon dioxide
CO CO2
O= 1 O= 2
C= 1 1
C=

57. Copper (I) chloride
Copper (II) chloride