UNZA Pharmacy Training Lecture notes

2.  Characteristics of Matter
 Mass
 Mass inertia
 Weight
 Weight formula
 Gravity
 Density
 Classification of Matter
 Materials
 Pure Substances
 Mixtures
 Properties of Matter
 Physical Properties
 Chemical Properties
 Extensive Properties
 Intensive Properties
 Kinetic Molecular Theory of Matter

4. Mass is the amount
of matter in an object
Mass is constant
Mass is also the
measure of inertia
4

5. Inertia is the
resistance of an object
to changes in its
motion
The more mass the
greater the inertia
5

6.  How is mass related to inertia?
 Why are properties of an object important?
 Which object has more inertia, an empty wagon or one
loaded with rocks? Why?
 What does a seatbelt do for a passenger when a car stops
suddenly?
 Why would the passenger move forward without the
restraining force of the belt?
 What would stop a passenger if the seatbelt were not in
place?
 What other safety features are present in a car in response
to a person’s inertia in a moving vehicle?
7

7.  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)
8

8.  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?
9

9.  The force of attraction
between objects is
gravity
 All objects exert a
gravitational force on
each other
10

10. A comparison of the
density of a substance
and the density of
water is specific
gravity
11

11. The greater the mass
of an object the
greater the
gravitational force
12

12. The pull of gravity
weakens as the
distance between
objects increases
gravity depends on
mass and distance
13

13. The further an object
is from the center of
the earth, the less the
object will weigh
14

14.  Why can’t you feel the attraction between you and
other objects the same way you are pulled toward
Earth?
 Why can’t we feel the pull of gravity from Jupiter even
though it is so massive?
 Would you weigh less, more, or the same on top of
Mount Everest?
 The moon is smaller than the earth. How would your
weight be different on the moon?
 What are three properties of matter related to mass?
 What is density and how is it calculated?
 How is density different from specific gravity?
15

15.  The density of water is 1.0 g/ml
 Objects with densities greater
than 1.0 will sink in water
 Objects with densities less than
1.0 g/ml will float on water
16

16. Ice floats therefore it is
less dense than water
Ice mostly remains
underwater with only a
portion of it being exposed
17

17. 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!
18

18.  If 96.5 grams of gold has a volume of 5 cubic
centimeters, what is the density of gold?
 If 96.5 g of aluminum has a volume of 35 cm3,
what is the density of aluminum?
 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?
19

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

21.  Contain only one type of matter
 Cannot be separated physically
 Elements - simplest pure substances
made of only one type of atom
(Referred to Periodic Table)
 Compounds - – two or more elements
that are chemically combined
(H2O, CuSO4)

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

23.  Substances can be easily
distinguished and separated
 Example: sand and salt, iron and
sugar, sand and gravel
 Substances are well mixed and appear
the same throughout mixture matrix
 Example: Solution of sugar & salt

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

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

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

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

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

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

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

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

33.  Matter is anything that has
mass and volume
 Everything is made of matter
 Mass, weight, volume, and
density
 Properties are used to identify
a substance
34

34. Physical properties
are those that can be
observed without
changing the identity
of the substance
35

35.  Four phases of matter: solid,
liquid, gas, and plasma
 solids have a definite shape
and volume
36

36.  Solids are tightly packed
and the particles vibrate
 Two types of solids are
crystalline and amorphous
37

37. Crystalline solids are
arranged in repeating
patterns called crystals
(salt, sugar)
Amorphous solids can lose
their shape
38

38.  Tar, candle wax, glass,
some drug crystals as
sulphur
 Shape changes under
certain conditions
(differences in
temperature)
39

39. Liquids have particles
that are close
together, but are free
to move
40

40. Liquids do not have a
definite shape, but
they have a definite
volume
41

41. Liquids do not expand to fill
the volume of a container
Liquids are characterized
by their ability to flow
42

42.  Cohesion is the force of
attraction between LIKE
particles
 Adhesion is the force of
attraction between UNLIKE
particles
43

43. Tendency of particles to
pull together at the
surface of a liquid due to
cohesion
44

44.  The resistance of a liquid to
flow
 The difficulty of a liquid to
flow easily
 Honey, motor oil, corn syrup
have a high viscosity
45

45.  Describe the shape of a liquid.
 What happens when one-liter of soda is poured into a
four-liter container?
 Describe the viscosity of a liquid.
 Describe a liquid’s shape.
 How is adhesion different from cohesion?
 Explain surface tension.
46

46. Gases do not have a
definite shape or volume
They fill all the available
space in a container
47

47. Matter is made of tiny
particles in constant
motion
48

48.  Boyle’s and Charles’ law
describe the behavior of
gases with changes in
temperature, pressure, and
volume
49

49. Charles’ law describes a
relationship between the
temperature and volume
of a gas (constant
pressure)
50

50.  As the temperature of a
gas increases, the volume
of a gas increases
 Heating air causes it to
expand
51

51. The force that particles
of a substance
(gas/liquid) will apply
over a certain area
52

52. Boyle’s law describes
the relationship between
the volume and pressure
of gases (constant
temperature)
53

53. 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
54

54.  Plasma (phase)
 most common phase in the
universe, dangerous, very
high energy (found in stars)
55

55.  Phase changes in matter are melting,
freezing, vaporization, condensation,
and sublimation
 Physical changes involve the changing
of physical properties
 Type of matter remains the same
 Changing color, shape, phase, texture,
hardness, odor would be a physical
change
56

56.  Phase change from a solid to
a liquid
 Temperature in which a solid
changes to a liquid
 Physical property
57

57.  Involve a change in volume,
but mass remains constant
 Adding or removing energy
from matter results in phase
changes
58

58. Phase change from a
liquid to a gas
59

59.  The temperature in which a
liquid boils
 Point at which a liquid
changes to a gas
60

60. Phase change of a liquid
to a solid
The temperature in
which this occurs is the
freezing point
61

61. Condensation is the phase
change from a gas to a
liquid
Sublimation is a phase
change from solid to a gas
62

62. Dry ice and iodine are
examples solids that
undergo sublimation
63

63.  Describe how a substance
changes into new substances are
chemical properties
 Ex: flammability
 The change of a substance into a
new and different substance
 Also known as a chemical
reaction
64

64.  How is melting different from
freezing?
 Describe a difference between
condensation and vaporization.
 What is another name for a
chemical change?
 Describe sublimation.
 How is a chemical change
different from a physical
change?
65

66.  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