This document defines key terms and concepts related to the physical properties of pharmaceutical materials, including: 1. It defines the four phases of matter - solids, liquids, gases, and plasma - and describes their characteristic properties such as definite/indefinite shape and ability to flow. 2. It explains physical and chemical properties, including properties related to phase changes like melting, boiling, freezing, and condensation. Density, color, and conductivity are given as examples of physical properties. 3. Chemical properties like flammability and reactivity that result in chemical changes forming new substances are also addressed. The differences between physical and chemical changes are summarized.

1. Physical Properties of Pharmaceutical-
Related Materials

2.  Classification of Matter
 Properties of matter

4.  Specific types of matter
 Described according to phase material
types (solid, liquid, gas)

5. Contain only one type of
matter
Cannot be separated
physically

6. Elements - simplest pure
substances made of only
one type of atom
(Referred to Periodic Table)

7. Compounds - – two or
more elements that are
chemically combined
(H2O, CuSO4)

8. Physical combination of
two or more substances
Can be separated
physically

9. Substances can be easily
distinguished and separated
Example: sand and salt, iron
and sugar, sand and gravel

10. Substances are well
mixed and appear the
same throughout mixture
matrix
 Example: Solution of sugar & salt

11. Solute dissolves in solvent to
form solution.
Concentrated solution
contains more solute than
dilute solution.
Example: Kool-Aid, tea,
coffee, sodium chloride

12. Depend on sample size
Specific to a single object
Example: length, mass,
diameter

13. Do not depend on sample
size
Used to identify types of
matter
All physical and chemical
properties are intensive

14. Describe substances
undergoing physical changes
Ex: density, color, texture,
conductivity, malleability,
ductility, boiling point, melting
point

15. Describe substances
undergoing chemical
changes
Ex: flammability,
corrosiveness, volatility

16. Same substance remains
after change
Used to separate mixtures
Ex: pounding, tearing,
cutting, dissolving,
evaporating, melting,
boiling, pulling

17. Results in new substance
with new properties
Also known as a chemical
reaction
Ex: burning, digesting,
fermenting, decomposing

18.  1. Precipitate forms (solid)
 2. Gas evolves (bubbles)
 3. Color change
 4. Energy change
Exothermic = releases energy
Endothermic = absorbs energy
 5. Odor produced (sometimes)

20. Matter is anything that
has mass and volume
Everything is made of
matter
20

21. Characteristics used to
describe an object
Ex: color, odor, shape,
size, texture,hardness
21

22. Mass, weight, volume,
and density
Properties are used to
identify a substance
22

23. Mass is the amount of
matter in an object
Mass is constant
Mass is also the
measure of inertia
23

24. Inertia is the
resistance of an object
to changes in its
motion
The more mass the
greater the inertia
24

25. How is mass related to
inertia?
Why are properties of an
object important?
25

26. Which object has more
inertia, an empty
wagon or one loaded
with rocks? Why?
27

27. What does a seatbelt
do for a passenger
when a car stops
suddenly?
28

28. Why would the
passenger move
forward without the
restraining force of
the belt?
29

29. What would stop a
passenger if the
seatbelt were not in
place?
30

30. What other safety
features are present in
a car in response to a
person’s inertia in a
moving vehicle?
31

31.  This is the measure of
the force of gravity on
the mass of an object
 Weight changes with
gravity
 The metric unit for
weight is a Newton (N)
32

32.  1 kg = 2.2 pounds
 Weight is mass times gravity (9.8
m/s2)
 W= m x g
 What is your mass?
 What is your weight in Newtons?
33

33.  The force of attraction
between objects is
gravity
 All objects exert a
gravitational force on
each other
34

34. Why can’t you feel the
attraction between you
and other objects the
same way you are
pulled toward Earth?
35

35. The greater the mass
of an object the
greater the
gravitational force
36

36. Why can’t we feel the
pull of gravity from
Jupiter even though it
is so massive?
37

37. The pull of gravity
weakens as the
distance between
objects increases
gravity depends on
mass and distance
38

38. The further an object
is from the center of
the earth, the less the
object will weigh
39

39. Would you weigh less,
more, or the same on
top of Mount Everest?
40

40. The moon is smaller
than the earth. How
would your weight be
different on the moon?
41

41. What are three
properties of matter
related to mass?
42

42. What is density and
how is it calculated?
43

43. The density of water is
1.0 g/ml
Objects with densities
greater than 1.0 will
sink in water
44

44. Objects with densities
less than 1.0 g/ml will
float on water
45

45. Ice floats therefore it is
less dense than water
Ice mostly remains
underwater with only a
portion of it being exposed
46

46. The planet Saturn has a
density of less than 1.0
g/ml. If there was an ocean
big enough to hold it, it
would float!
47

47. If 96.5 grams of gold
has a volume of 5
cubic centimeters,
what is the density of
gold?
48

48. If 96.5 g of aluminum
has a volume of 35
cm3, what is the
density of aluminum?
49

49. If the density of a
diamond is 3.5 g/cm3,
what would be the
mass of a diamond
whose volume is 0.5
cm3?
50

50. A comparison of the
density of a substance
and the density of
water is specific
gravity
51

51. How is density different
from specific gravity?
52

52. Physical properties
are those that can be
observed without
changing the identity
of the substance
53

53.  Four phases of matter: solid,
liquid, gas, and plasma
 solids have a definite shape
and volume
54

54.  Solids are tightly packed
and the particles vibrate
 Two types of solids are
crystalline and amorphous
55

55. Crystalline solids are
arranged in repeating
patterns called crystals
(salt, sugar)
Amorphous solids can lose
their shape
56

56.  Tar, candle wax, glass,
some drug crystals as
sulphur
 Shape changes under
certain conditions
(differences in
temperature)
57

57. Liquids have particles
that are close
together, but are free
to move
58

58. Describe the shape of
a liquid.
59

59. Liquids do not have a
definite shape, but
they have a definite
volume
60

60. What happens when
one-liter of soda is
poured into a four-liter
container?
61

61. Liquids do not expand to fill
the volume of a container
Liquids are characterized
by their ability to flow
62

62.  The resistance of a liquid to
flow
 The difficulty of a liquid to
flow easily
 Honey, motor oil, corn syrup
have a high viscosity
63

63.  Cohesion is the force of
attraction between LIKE
particles
 Adhesion is the force of
attraction between UNLIKE
particles
64

64. Tendency of particles to
pull together at the
surface of a liquid due to
cohesion
65

65. Describe the viscosity of
a liquid.
Describe a liquid’s
shape.
66

66. How is adhesion
different from cohesion?
Explain surface tension.
67

67. Gases do not have a
definite shape or volume
They fill all the available
space in a container
68

68. Matter is made of tiny
particles in constant
motion
69

69. How are solids, liquids,
and gases different from
one another?
70

70.  Boyle’s and Charles’ law
describe the behavior of
gases with changes in
temperature, pressure, and
volume
71

71. Charles’ law describes a
relationship between the
temperature and volume
of a gas (constant
pressure)
72

72.  As the temperature of a
gas increases, the volume
of a gas increases
 Heating air causes it to
expand
73

73. How can you explain
the fact that gas
particles expand to fill
space?
74

74. The force that particles
of a substance
(gas/liquid) will apply
over a certain area
75

75. Boyle’s law describes
the relationship between
the volume and pressure
of gases (constant
temperature)
76

76. If the volume of a gas
decreases, then the
pressure of a gas increases
(Boyle’s law)
The smaller the space a
gas occupies, the more
pressure
77

77.  Plasma (phase)
 most common phase in the
universe, dangerous, very
high energy (found in stars)
78

78. What are the four phases
of matter?
Describe the plasma
phase of matter.
79

79. Phase changes in matter
are melting, freezing,
vaporization,
condensation, and
sublimation
80

80.  Physical changes involve the
changing of physical
properties
 Type of matter remains the
same
81

81.  Describe each of the five
phase changes (melting,
freezing, vaporization,
condensation, and
sublimation).
82

82. Changing color, shape,
phase, texture,
hardness, odor would
be a physical change
83

83. Phase change from a
solid to a liquid
84

84. Temperature in which
a solid changes to a
liquid
Physical property
85

85. How is melting different
from freezing?
86

86.  Involve a change in volume,
but mass remains constant
 Adding or removing energy
from matter results in phase
changes
87

87. Phase change from a
liquid to a gas
88

88.  The temperature in which a
liquid boils
 Point at which a liquid
changes to a gas
89

89. Phase change of a liquid
to a solid
The temperature in
which this occurs is the
freezing point
90

90. Condensation is the phase
change from a gas to a
liquid
Sublimation is a phase
change from solid to a gas
91

91. Describe a difference
between condensation
and vaporization.
92

92. Dry ice and iodine are
examples solids that
undergo sublimation
93

93. Describe how a substance
changes into new
substances are chemical
properties
Ex: flammability
94

94.  The change of a substance
into a new and different
substance
 Also known as a chemical
reaction
95

95.  What is another name for a
chemical change?
 Describe sublimation.
 How is a chemical change
different from a physical
change?
96

97.  Define the following terms:
[solid, liquid, gas, pure substance, compound, mixture, element, heterogeneous mixture, homogeneous mixture,
extensive properties, intensive properties, chemical properties, physical properties, density, color, texture,
conductivity, malleability, ductility, boiling point, melting point, flammability, corrosiveness, volatility, pounding,
tearing, cutting, dissolving, evaporating, fermenting, decomposing, Exothermic, endothermic, mass, density, gravity,
adhesive force, cohesive force, etc]
 Respond to the following questions:
➢ What is a mass, inertia, and how do these two variables affect the movement of material substance
➢ What is gravity and how does it affect the movement of material substance
➢ Give a descriptive account of the phases of matter with logical relevance to state of medicines as they are taken
for their respective therapeutical values
➢ What is viscosity and its relation with fluids
➢ What is surface tension and association with activities a substance material with surface area
➢ Describe some key phase changes of materials substance when exposed to some environmental conditions of
change
➢ How is a chemical change different from a physical change
 Group work discussional questions:
➢ Give a detailed account of the properties of matter and how such react to the changes of the surrounding
media
➢ Describe the material phases according to the type of material substance
➢ Give a scientiic account of the differences between physical and chemical properties of material substance