2. DIVERSITY OF MATTER

Eclipse
(Pink Floyd –The Dark side of the
Moon)
All that you touch
All that you see
All that you taste
All you feel
All that you love
All that you hate
All you distrust
All you save
All that you give
All that you deal
All that you buy
beg, borrow or steal

All you create
All you destroy
All that you do
All that you say
All that you eat
everyone you meet
All that you slight
everyone you fight
All that is now
All that is gone
All that's to come
And everything under the sun is in tune (*)
But the sun is eclipsed by the moon.

And is made of MATTER!

…Matter is anything that occupies
space.

States of Matter
The

Four States of
Matter

Solid

Liquid
Gas

Plasma

4

States of Matter


The Four States of
Matter

Basis

of Classification of the Four
Types

 Based

upon particle arrangement
 Based upon energy of particles
 Based upon distance between
particles

5

States of Matter
Solids




Particles of solids are tightly packed, vibrating
about a fixed position.
Solids have a definite shape and a definite
volume.
Solids have an infinite number of free surfaces.

6

States of Matter
Microscopic Explanation for Properties of
Solids
 Solids have a definite shape and a definite
volume
because the particles are locked into place
 Solids are not easily compressible because
there is little free space between particles
 Solids do not flow easily because the
particles cannot move/slide past one another

7

States of Matter





Liquids

Particles of liquids are tightly packed, but are
far enough apart to slide over one another.
Liquids have an indefinite shape and a definite
volume.
Liquids have one free surface.

8

States of Matter
Microscopic Explanation for Properties of
Liquids
 Liquids have an indefinite shape because the
particles can slide past one another.
 Liquids are not easily compressible and have
a definite volume because there is little free
space between particles.
 Liquids flow easily because the particles can
move/slide past one another.

9

States of Matter





Gases

Particles of gases are very far apart and move freely.
Gases have an indefinite shape and an indefinite
volume.
Gases have no free surfaces.

10

States of Matter

Microscopic Explanation for Properties of
Gases
 Gases have an indefinite shape and an
indefinite volume because the particles can
move past one another.
 Gases are easily compressible because there
is a great deal of free space between
particles.
 Gases flow very easily because the particles
randomly move past one another.
11

States of Matter


Plasma

A plasma is an ionized gas at very high
temperature.
 A plasma is a very good conductor of
electricity and is affected by magnetic fields.
 It is is by far the most common form of
matter. Plasma in the stars and in the
tenuous space between them makes up over
99% of the visible universe and perhaps
most of that which is not visible.

12

States of Matter

13

States of Matter
Microscopic Explanation for Properties of
Plasmas
 Plasmas have an indefinite shape and an
indefinite volume because the particles can
move past one another.
 Plasmas are easily compressible because
there is a great deal of free space between
particles.
 Plasmas are good conductors of electricity
and are affected by magnetic fields because
they are composed of ions (negatively
charged electrons and positively charged
nuclei).
14

States of Matter


The Four States of
Matter

The

Classification and Properties of
Matter Depend Upon Microscopic
Structure

 Particle
 Particle
 Particle

arrangement
energy
to particle distance

15

Gases, Solids, and Liquids

Particle Properties

Phase

Spacing

Energy

Motion

Volume

Shape

Solid

close

low

vibrational

definite

definite

Liquid

close

moderate

rotational

definite

indefinite

far apart

high

translational

indefinite

indefinite

Gas

Physical

properties are those that
we can determine without
changing the identity of the
substance we are studying.

The physical properties can be observed or measured.
Hardness, color, melting point and density are all physical properties

Intensive

properties do not
depend on the size of the
sample of matter and can be
used to identify substances.

density, color, melting and boiling
point , …..

Extensive

properties depend on
the quantity of the sample.

mass , area, volume, …

All matter, regardless of state, undergoes
physical and chemical changes.

A physical change occurs when the substance changes state but does
not change its chemical composition.
For example:
•water freezing into ice
•cutting a piece of wood into smaller pieces
•breaking a paper
The form or appearance has changed, but the physical properties of
that substance are the same:
Melting point Density Boiling point Color Vapor pressure
Electrical conductivity Solubility Hardness……

Chemical

properties describe the
way a substance can change or
react to form other
substances. These properties,
then, must be determined using a
process that changes the identity
of the substance of interest.

A chemical change occurs when a substance
changes into something new.
This occurs due to heating, chemical reaction, etc. You can tell a
chemical change has occurred if the density, melting point or freezing
point of the original substance changes. Many common signs of a
chemical change can be seen (bubbles forming, mass or colour
changed, etc).

Mixtures are two or more substances that are NOT
chemically combined.

Mixtures do not:
·      Have constant boiling points
·      Have constant melting points

Variable

composition
Components retain their
characteristic properties
May be separated into pure
substances by physical methods
Mixtures of different
compositions may have widely
different properties

Heterogeneous

mixtures are
composed of large pieces that are
easily separated by physical means
(ie. density, polarity, metallic
properties).

Do

not have same composition
throughout
Components

are distinguishable
Examples: fruit salad, vegetable soup,
wood, granite, etc.

Solutions are homogenous. Therefore, they are easily
separated by physical methods like distillation or
evaporation.
Examples:
• Sugar /water
• Stainless steel
• Salt / water
• Wine
• Brass
• Air
• Cola drink

Separating Mixtures
Dirty
water

Oil and
Water

Saltwate
r

Settling
Density

causes
parts of the mixture
to settle to the
bottom.

This

process is used
during water
filtration.
Contaminants sink
and clearer water is
skimmed off.
31

MAGNETIC

To separate a magnetic component from a
mixture containing non- magnetic
components
(e.g. iron and sand or sulphur).

Decantation
Decanting is the
simplest possible way of
separating a liquid (pure
or a solution) from an
insoluble solid which
has a density greater
than water

A mixture of two
immiscible liquids can
also be separated by

Filtration
A

mixture is
passed through
material with
many holes.
Anything larger
than the hole is
trapped while the
rest of the
mixture passes
through.
 Examples:
 Dirty water lab

34

Crystallization
The

separation
process in which
the solvent is
evaporated,
leaving crystals
of solute behind.
◦ Examples:

 Rock candy
 Saltwater lab

35

 The

Distillation

separation process in which the desired
component is evaporated from the solution
and collected.
 Water is boiled and the steam is collected. As
the steam cools, it condenses to form pure
water and anything that was dissolved in the
water is left behind

36

Chromatography
This

process is mostly
used to identify
substances.
As the substance is
drawn up the material
(e.g., filter paper), it
carries the solutes
with it.
The least dense are
drawn farthest up the
filter paper.
 Example:

37

A substance is matter of a particular kind.
A substance cannot be further broken down or
purified by physical means.
Each substance has its own characteristic properties
that are different from the set of properties of any
other substance.

 Fixed

composition

 Properties

do not vary

 Cannot

be separated into simpler substances
by physical methods (physical changes)

 Can

only be changed in identity and
properties by chemical methods

Compounds
 Can

be decomposed
into simpler
substances by
chemical changes,
always in a definite
ratio*






Elements
 Cannot

be decomposed
into simpler substances
by chemical changes
 Gold
 Iron
 Sulfur
 Oxygen
 Chlorine

Water
Sugar
Salt
Ammonia
* Water always contains 88,9 % oxygen and 11,1 % hydrogen
Propane

MATERIAL SYSTEM
HAS IT UNIFORM PROPERTIES?

YES

NO: MIXTURE

HOMOGENEOUS

HETEROGENEOUS
Wood
Granite
Hamburger
Pencil

Has it always the same
composition and properties?

NO: MIXTURE

SOLUTION
drinking water
Bronze
Air
Bleach
Coca-Cola

YES: PURE SUBSTANCE
Can it be broken down into a simpler substance
by a chemical reaction?

NO

YES

COMPOUND
Water
Sugar
Sulfuric acid
Salt

ELEMENT
Gold
Oxygene
Copper

Solutions

Definitions
A

solution is a homogeneous mixture

A

solute is dissolved in a solvent.
 Solute is present in the smaller amount
 The solvent is present in the larger
amount.
an aqueous solution has water as solvent
*ey-kwee-uhs

Solutions

a homogenous mixture of 2 or more
substances
Solvent
Solute

the substance
present in the
larger amount

is(are) the
substance(s)
present in the
smaller
amount(s)

When the solvent is water the solution is
said to be aqueous

Types of solutions
􀂄 Gases

 Gases dissolved in gases (air)
 Liquids dissolved in gases (humid air)
 Solids dissolved in gases (moth balls *)

􀂄 Liquids
 Gases in liquids (air dissolved in water)
 Liquids in liquids (ethanol in water)
 Solids in Liquids (salt in water)

􀂄 Solids

 Gases in solids (H2 in Pt)
 Liquids in solids (Hg/Ag amalgam)
 Solids in solids (Cr in Fe alloy)
(*) bolas antipolilla

Terminology
 Solubility: The maximum amount of solute that will dissolve in
a solvent.
 Dilute: A solution that contains relatively little solute.
 Concentrated: A solution that contains a relatively large
amount of solute.
 Saturated: is one where the concentration is at a maximum no more solute is able to dissolve.
 Supersaturated: A solution that contains more than the
solubility limit.

Concentration
Concentration is the amount of solute in a given amount
of either solution or solvent
mass solute
% (w / w ) 
mass solution
% (v / v ) 

g/L 

volume solute
volume solution

grams of solute
liters of solution

x 100

x 100

Factors Affecting Solubility
1. Nature of Solute / Solvent.

- Like dissolves like

2. Temperature -

Solids/Liquids- Solubility increases with Temperature
Gases - Solubility decreases with Temperature

3. Pressure Factor -

Solids/Liquids - Very little effect
Gas - Solubility increases with Pressure.

Solubilities of Solids vs
Temperature

Solubilities of Gases vs
Temperature