MATTER AND MATERIAL

1. MATER AND MATERIALS
CLASSIFICATION OF MATTER
STATES OF MATTER
Edited by MUSA ELVIS CHAUKE
3RD YEAR STUDENT AT THE UNIVERSITY
OF JOHANNESBURG 201115985

2. Chemistry
A
physical science
that involves the
study of the
properties,
composition,&
structure of matter
and the changes it
undergoes.

3. What is a chemical?
 Any
substance
that has a
definite
composition or is
used or produced
in a chemical
process.

Sugar is an example of a
chemical

4. MATTER

Anything that has mass and occupies space

All matter is composed of atoms

Atom:

Extremely small chemically indivisible particle

Atom is Greek for “that which cannot be divided”

Greek philosopher Democritus is given credit for idea

Modern science can now divide an atom, so new definition
includes chemically indivisible

An atom cannot be divided and retain it’s chemical properties

5. Three Major Classes of Elements
 Metals-
located on the left of the Periodic Tablemost of the elements
 Non-Metals-
Table

located on the right of the Periodic
Metalloids- on the zigzag line between Metals
and Nonmetals- have properties that are skewedie…Silicon is conductive
 You
will have to memorize the symbol and
element name for approximately 40 common
elements

6. More ways to describe matter

Element: any substance that cannot be broken up into simpler
substances by chemical means


Compound: a substance formed when atoms of two or more
elements join together


silver, copper, hydrogen, oxygen nitrogen
H20 (water), CO2 (carbon dioxide)
Mixture: a material of two or more substances that are not
chemically bound to each other and can be separated

Blood: water-based mixture including

Proteins, sugars, salt, oxygen, carbon dioxide

7. Properties of Metals
Metals are good
conductors of heat and
electricity

Metals are malleable
(can be
shaped)

Metals are ductile (can
be drawn into wires)

Metals have high tensile
strength


Metals have luster

8. Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a great
example of a nonmetallic element.

Nonmetals are poor conductors of heat and
Electricity

Nonmetals tend to be brittle
Many nonmetals are gases at room
temperature


9. What is not
matter?
•
ght
Li
•
city
tri
lec
E
•
und
So

10. 
Fixed composition

Cannot be separated into simpler
substances by physical methods
(physical changes)

Can only be changed in identity and
properties by chemical methods

Properties do not vary- Unique
Density, Constant Boiling and Melting
Points

11. Elements
 Cannot be
decomposed
into simpler
substances by
chemical
changes
Compounds

Chemically joined
elements- Can be
decomposed into
simpler substances
by chemical
changes, always in
a definite ratio

12. Compounds (cont.)
Section 3-4
• The properties of a compound are different
from its component elements.

13. Compounds
Section 3-4
• A compound is a made up of two or more
elements combined chemically.
• Most of the matter in the universe exists as
compounds.
• Table salt, NaCl, and water, H2O, are
compounds.

14. Compounds (cont.)
Section 3-4
• This figure shows
electrolysis of
water to form
hydrogen and
oxygen.

15. Variable composition
 Components retain their characteristic
properties
 May be separated into pure substances
by physical methods sifting,
evaporation, magnetism, etc…
 Mixtures of different compositions may
have widely different properties
 Do NOT have definite boiling/melting
points


16. Homogenous mixtures look the same
throughout but can be separated by
physical means
Examples:
salt water, soda

17.  Have
the same composition
throughout
 Components are
indistinguishable
 Can exist between all phases of
matter: air (gases) brass (alloyblend of multiple metals -solids)
soda (gas, solid, liquid)

18. Solutions are homogenous mixtures that
do not scatter light. These mixtures are
created when something is completely
dissolved in pure water. Therefore, they
are easily separated by distillation or
evaporation. Appear in one phase of
matter
Examples: sugar water, salt water

19. Parts of a solution
 Solvent-
part that
does the dissolvingwater is our
universal solvent
 Solute-
part that
was dissolved (salt)

20. How do we increase solubility of a solid
into a liquid
 Heat
it- more
collisions between
solute and solvent
 Mix-
Fresh solvent
to solute
 Crush-
more surface
area- more contact

21. Increase solubility of a gas in a liquid

Henrys Law- solubility of the gasis directly
proportional to the pressure above the
liquid-

Effervescence- rapid escape of gas from
liquid

Decrease temperature- slows down
diffusion

22. Heterogeneous mixtures are composed of
large pieces that are easily separated by
physical means (ie. density, polarity,
metallic properties, size).
Pond Water, Vegetable Soup- Suspensions
Visible particles
Starch Water: invisible to the eye :colloid

23. Physical Properties – Observable traits
of a material that may be measured
without altering the substance
Examples: Mass, Color, Melting Point,
Boiling Point, Density

24. We can use physical
properties to separate
mixtures: a method to separate the
Please determine
following and determine the type of matter:
Oil and Water
Iron and Sand
Sand and Salt
Sulfur and Sugar

25. What are the
physical properties
of the substance to
the right?
What do you think the material is that made this
bracelet?
How could you be sure?
Density- the amount of material in a given
volume- unique to the material

26. Chemical Changean irreversible change
that changes the
identity and make up of
the material
Examples:
Rusting
Burning

27. 
There is no observable change in the
quantity of matter during a chemical
reaction or a physical change.
In other words, matter cannot be
created nor destroyed. It is just
converted from one form to
another

28. Energy comes in two forms :
Kinetic Energy: Movement
Potential Energy: Stored

29. All matter, regardless of state, undergoes
physical and chemical changes. These
changes can be microscopic or
macroscopic.

30. A physical change occurs when the
substance changes state but does not change
its chemical composition. It is not
permanent and is reversible! Example
Phase Changes!

31. Physical Change
For example: Ice melting
to water. The form or
appearance has
changed, but the
properties of that
substance are the same
(i.e. it has the same
melting point, boiling
point, chemical
composition, etc.)

32. PHYSICAL PROPERTIES

Characteristic of a substance that can be observed
without changing substance into another substance

Color

Odor

Taste

Size

Physical state (liquid, gas, or solid)

Boiling point

Melting point

Density

34. Names of Water Phase
Changes
Endothermic Requires Energy to go
Exothermic Gives energy off
forward

Melting: Solid Liq

Boiling (forced)
Liquid Gas

Evaporation ( spon)
Liquid Gas

Sublimation
Solid Gas
Condensation

Gas Liq

Freezing:
Liq Solid

Deposition:
Gas Solid

35. A substance
changes into
something new.
It is irreversible.

36. All Chemical Changes can be written as a
reaction

A + B  AB
 A,
B are the starting
materials- reactants
 AB
is the resultproduct

37. 
Reaction with acids


Reaction with bases
(alkalis)
Ability to act as
reducing agent

Reaction with oxygen
(combustion)
Reaction with other
elements

Ability to act as
oxidizing agent
Decomposition into
simpler substances

Corrosion



38. 
Physical and chemical properties may be intensive or extensive.

39. 

Intensive properties such as density, color, and
boiling point do not depend on the size of the
sample of matter and can be used to identify
substances.

40. 
Extensive properties such as mass and volume do depend on the
quantity of the sample.

41. 
Physical properties are those that we can determine
without changing the identity of the substance we are
studying.

42. 
The physical properties of sodium metal can be
observed or measured. It is a soft, lustrous, silvercolored metal with a relatively low melting point and
low density.

Hardness, color, melting point and density are all
physical properties.

43. Specific Heat
 Physical
Property that is
unique to the material
 Amount
of energy required to
heat 1 gram of a substance
by 1 degree Celsius
 -Why do you choose to sit on the
wooden bleachers on a cold fall
day for a football game instead of
the metal bleachers?

44. 
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.

45. 
One of the chemical properties of
alkali metals such as sodium and
potassium is that they react with
water. To determine this, we would
have to combine an alkali metal with
water and observe what happens.

In other words, we have to define
chemical properties of a substance by
the chemical changes it undergoes.

46. States of Matter
.
The physical forms of matter, either solid,
liquid, or gas, are called the states of matter.
• Solids are a form of matter that
have their own definite shape and
volume.
• Liquids are a form of matter that
have a definite volume but take the
shape of the container.

47. States of Matter (cont.)
.
• Gases have no definite shape or
volume. They expand to fill their
container.
• Vapor refers to the gaseous state
of a substance that is a solid or
liquid at room temperature.

48. Resources Menu
Chemistry Online
Study Guide
Chapter Assessment
Standardized Test Practice
Image Bank
Concepts in Motion

49. Reference
Atreasuredsecret.(2013). Matter and material. Available from :
http://www.slideshare.net/musachauke/savedfiles?s_title=matter16243469&user_login=atreasuredsecret [ Accessed 06 March 2014]
Braisitz(2011). Matter and change. Available from
:http://www.slideshare.net/briansitz/matter-and-change-9735404[06 March 2014]
Hamz, J.(2010). Chemistry and change. Available from:
//www.slideshare.net/jhamze/cmc-chapter-03 [06 March 2014]
Hernandez,E.(2012).Matter and material. Available from:
http://www.slideshare.net/alexrhernandez7777/matter-27998160?qid=6343c4aef420-4fb7-bab5-c888b8836185&v=default&b=&from_search=1 [Accessed 06 March
2014]