July 2004
Chemistry: the science that deals with
the composition, structure and behavior of
matter. It is also concerned with the
energy and the energy changes associated
with matter.
Matter
• Volume is the amount of three dimensional space an
object occupies.
• Mass is a measure of the amount of matter. It is a
function of the amount of atoms in a substance.
• Matter is anything that has mass and takes up
space.
CLASSIFICATION OF MATTER
ACCORDING TO ITS STATE
Solid, liquid and gas.
STATES OF MATTER
Matter
Gas
Liquid
Solid
STATES OF MATTER
Matter
Gas
Liquid
Variable shape and
volume that fill
container.
Variable shape: It
adopts the shape of
the container.
Random particle
movement.
Definite volume.
Large intermolecular
distances.
Random particle
movement within
fixed volume.
Particles are closer
than in the gas
state.
Solid
Definite shape and
volume.
Restricted particle
movement to fixed
positions: vibration.
Short intermolecular
distances.
Crystalline and
amorphous
structures.
Plasma – at extreme temperatures like those of the
sun, high-energy collisions between atoms may strip
off electrons, creating plasma, in which positive nuclei
move about in a sea of electrons.
Stars are
composed of a
dense hydrogenand helium-rich
plasma mixture.
Properties of Matter
Physical properties: properties which can be
observed without changing the composition of matter.
Physical Change
Solid iodine is heated and it
sublimes, that is it changes
from a solid to a gas state
directly.
CHANGES IN THE STATES OF MATTER
MELTING -The process of a solid transforming to a liquid
FREEZING - The process of converting a liquid into a solid.
CONDENSATION - the gas being converted to a liquid.
EVAPORATION - the liquid being converted to a gas.
Freezing
Melting
Melting
Condensation
Evaporation
Chemical properties:
describe the ability of a substance to
form a new substance. They are only observed when the substance
undergoes a change in composition.
CHEMICAL PROPERTIES
For example, hydrogen has the potential to ignite and explode given
the right conditions. This is a chemical property. Metals in general
have they chemical property of reacting with an acid. Zinc reacts with
hydrochloric acid to produce hydrogen gas. This is a chemical
property.
See video for differences
between physical and
chemical properties.
See video for differences
between physical and
chemical changes.
Chapter 1
Chemical Reactions
• The reactants are the substances that react in a
chemical change.
• The products are the substances that are formed by
the chemical change.
reactants
product
Carbon plus oxygen yields (or forms) carbon dioxide.
carbon
+ oxygen
carbon dioxide
• Evidence of a Chemical Change
Evolution of a gas
Formation of a
precipitate
Energy changes
light, sparks, warm
or cold container
Color Change
Properties of matter
Physical properties
Chemical properties
Can be observed without
changing the substance into
another substance.
Describes the way the
substance undergoes or
resists change to form
another substance.
Color
Odor
Texture
Boiling point
Melting point
Density
Solubility
Decomposition
Explosiveness
Flammability
Combustibility
Corrosion
Reactivity
Classification of changes as physical or chemical
Change
Rusting of iron
Melting of snow
Sharpening a pencil
Digesting food
Taking a bite of food
Burning gasoline
Slicing an onion
Detonation of dynamite
Souring of milk
Breaking of glass
Classification
Chemical
Physical
Physical
Chemical
Physical
Chemical
Physical
Chemical
Chemical
Physical
Classification of Matter
Mixtures
1. Physical combination of two or
more substances.
2. Variable composition.
3. Properties vary as composition
varies.
4. Components can be separated using
physical means.
Pure Substances
1.Only one substance is present.
2. Definite and constant composition.
3. Properties are always the same
under a given set of conditions.
Classification of Matter
Mixtures
Heterogeneous
Pure Substances
Homogeneous
1. Two or more distinct phases.
2. Each phase has different
properties
1. Only one visibly distinct phase.
2. The phase has the same
properties throughout.
Classification of Matter
Mixtures
Pure Substances
Compounds
1. A chemical combination of two
or more elements.
2. Can be broken down into
constituent elements using
chemical, but not physical
means.
3. Has a definite, constant
elemental composition.
See video
Elements
1. Cannot be broken down into
simpler substances by chemical or
physical means.
2. The building blocks for all other
types of matter.
3. 115 elements are known.
Homogeneous
Heterogeneous
Physical methods to separate mixtures
Filtration - method to separate a liquid from a solid.
Physical methods to separate mixtures
Distillation – to separate mixtures by using the differences in boiling
point.
See periodic table video
1A
1
H
1.008
3
Li
6.941
11
The symbols of the elements in red are derived from Latin
Na
natrium
Sn
stannum
K
kalium
Sb
stibium
2A
3A
4A
5A
Fe
ferrum
Au
aurum
4
5
6
7
Cu
cuprum
Hg
hydrargyrum
Be
B
C
N
9.012
10.811
12.011
14.007
Ag
argentum Pb
plumbum
12
Na
Mg
22.99
24.305
13
8B
3B
4B
5B
6B
7B
1B
2B
14
8A
2
He
6A
7A
4.0026
8
9
10
O
F
Ne
15.999
18.998
20.179
16
17
18
15
Al
Si
P
S
Cl
Ar
26.981
28.086
30.974
32.066
35.453
39.948
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
39.098
40.078
44.956
47.88
50.94
51.996
54.938
55.847
58.93
58.69
63.546
65.39
69.723
72.61
74.922
78.96
79.904
83.80
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
85.468
131.29
88.906
91.224
92.906
95.94
(98)
101.07
102.9
106.4
107.87
112.41
114.82
118.71
121.75
127.60
126.9
131.29
55
56
72
73
74
75
76
77
78
79
80
81
82
83
84
85
86
Cs
Ba
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
132.9
137.33
178.49
180.95
183.85
186.2
190.2
192.2
195.1
196.97
200.59
204.38
207.2
208.98
(209)
(210)
(222)
87
88
104
105
106
107
108
109
110
111
112
114
Fr
Ra
Rf
Db
Sg
Bh
Hs
Mt
Uun
Uuu
Uub
Uug
(223)
(226)
(261)
(262)
(266)
(264)
(277)
(268)
(272)
(272)
(285)
(289)
The symbol of the element in blue is derived from German
57
58
59
60
61
62
63
64
65
66
67
W
68
wolfram
69
70
71
La
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
138.9
140.1
140.9
144.24
(145)
150.36
151.97
157.25
158.96
162.5
164.93
167.26
168.93
173.04
174.97
89
90
91
92
93
94
95
96
97
98
99
100
101
102
Ac
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
103
Lr
(227)
232.04
231.04
238.03
(237)
(244)
(243)
(247)
(247)
(251)
(252)
(257)
(258)
(259)
(260)
Basic Laws of Matter
Law of Conservation of Mass - first published by Antoine
Lavoisier, French chemist (1743-1794). It states that
when a chemical or physical change occurs, the total
mass after the change is the same as the total mass
before the change.
Mass: is independent from the location.
Weight: the measure of the earth’s gravitational
attraction for a body. In general, it is a measure of
the gravitational force between two masses.
Balance - The instrument
used in the lab to get the
mass of an object.
Scale - The instrument used
in the lab to get the weight
of an object. Mostly used in
Physics
Some common
laboratory glassware
for measuring volume.