Matter and Change
2.1 Properties of Matter
2.2 Mixtures
2.3 Elements and Compounds
2.4 Chemical Reactions
2.1 Properties of Matter
 Objectives:



Identify properties of matter as extensive and intensive
Define physical and chemical properties
Differentiate between the 3 states of matter
KEY TERMS
Mass
Volume
Extensive Property
Intensive Property
Substance
Physical Property
Solid
Liquid
Gas
Vapor
Physical Change
Definitions
Mass (m) – the amount of matter an object contains (a numerical value
of its inertia)
Volume(V) – the amount of space an object occupies
Extensive
property - a property that depends on the amount of matter an object
contains
Intensive
property – a property that depends on type of matter an object contains
Substance – matter with uniform properties
Physical
property - a quality or condition of a substance that can be observed without
changing the composition of the substance
Chemical
property – a quality or condition of a substance that can be observed with
changing the composition of the substance
Physical
change - a change that do not affect the composition of a substance
Chemical
change – a change that does affect the composition of a substance
Some Criteria for the
Classification of Matter

Properties

State (solid, liquid, gas)

Composition
Intensive and Extensive
Properties
Sulfur
Examples of Physical
Properties
 Color,
odor, hardness, density,
melting point, boiling point, state,
solubility.
Example: Physical Properties
Substance
State
Color
Oxygen
O2
Gas
Colorless
Mercury
Hg
Liquid
Silverywhite
Bromine Br2
Liquid
Red-brown
Water
Liquid
Colorless
H2O
Sodium NaCl Solid
Chloride
White
Melting
Boiling
Density
3
Point (C°) Point (C°) (g/cm )
-218
-183 0.0014
-39
357
13.5
-7
59
3.12
0
100
1.00
801
1413
2.17
States of Matter
 Solid
fixed shape and volume,
incompressible
 Liquid
 fixed volume, takes the shape of
its container
 Gas
 takes the volume and shape of
its container

Solid
Liquid
http://www.chem.purdue.edu/gchelp/atoms/states.html
Gas
Bromine
Gas
(Vapor)
Liquid
Change of Phase
Melting
Condensation
solid
gas


liquid
liquid
Freezing
liquid

solid
Evaporation
Sublimation
liquid
solid


gas
gas
Boiling: Evaporation occurring beneath the
liquid’s surface.
Is changing phase a physical
or chemical change?
Classification of Matter
(by composition)
(Pure) Substance
 Matter
that has a uniform and
definite composition.
 Elements
 Compounds
2.2 MIXTURES

Objectives:

Categorize samples of matter into substance or mixture
Differentiate between homogeneous and heterogeneous
Describe two ways that components of mixtures can be
separated


KEY TERMS








Mixture
- physical blend of 2 or more substances
Heterogeneous – mixture in which the composition is not uniform
throughout
Homogeneous – mixture with a uniform composition throughout
Phase
– a part of a mixture with uniform composition
Solution
– another name for homogeneous mixture
Filtration
- a process that separates a solid from a liquid
Distillation - a process that separates a solid dissolved in a liquid/
separation of 2 miscible liquids with different boiling
temperatures
Miscible
- 2 or more liquids that can form a homogeneous mixture
Mixture
 A physical blend of two or more
substances.
Copper II Sulfate and its
solution in water.
Example: Stainless Steel
A homogeneous
mixture of:
-Iron (Fe)
-Chromium (Cr)
-Nickel (Ni)
Example: Gaseous Mixture
 Elements
argon and nitrogen and
a compound (water vapor).
Heterogeneous Mixtures
Example:
Oil and vinegar
 Non-uniform
composition
throughout the mixture
 Two or more phases.
Note:
 Mixtures
can be physically
separated.
 Mixtures
exhibit physical
properties similar to the
components of the mixture.
Separation Methods
 Use
differences in the physical
properties of the components of
the mixture.
Example: Separate iron filings
from sulfur using a magnet.
Filtration: separates a solid from a
liquid in a heterogeneous mixture
Distillation:
-separate dissolved solids from a liquid
-uses boiling and condensation.
Distillation of Crude Oil
(Refining)

Crude Oil is a mixture of Hydrocarbons
Distillation of Crude Oil
c) Elements and Compounds
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.
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.
Examples:

Americium, Am

Lead(Plumbum), Pb

Einsteinium, Es

Niobium, Nb

Bromine, Br

Iron (Ferrum), Fe

Helium, He

Mendelevium, Md
Compound

A substance that contains two or more
elements chemically combined.

Compounds have different properties
from the individual substances.
(Ex: H2O)
Example: H2O
Substance or mixture?
 If
composition is fixed and may
not changesubstance
d) Chemical Properties
and Chemical Changes
H2O composition is fixedcompound
Gaseous Phase
Liquid Phase
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.
Magnesium
Mg
Burning of Magnesium
2Mg+ O2 2MgO
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:

Chemical Change
A change that produces matter with a
different composition than the original
matter.
 Atoms rearrange themselves into new
combinations.

Burning of Methane
CH4 +2O2 CO2 + 2H2O
Burning of Methane
CH4 + 2O2 CO2 +
2H2O
Recognizing a Chemical Change
energy exchange
 production of a gas
 color change
 formation of a precipitate

Formation of a Precipitate
Cu(OH)2
Precipitate
The Law of Conservation of Mass
(Antoine Lavoisier)
 In
any chemical or physical
change, mass is neither
created or destroyed
 Mass
is CONSTANT