1. MATTER
Matter is everything that has mass and
occupies a place in space
If the matter has mass and occupies a place
in space means that it is quantifiable, i.e. it
can be measured.

2. • Everything we can imagine, from a book, a
car, a computer and even the chair that
sat and the water we drink, or even
something intangible as the air we
breathe, is made of matter.
• The planets of the universe, living beings
like insects and inanimate objects like
rocks, are also made of matter.

3. MASS
• The amount of matter in a body is given by
its mass, which is normally measured in
kilograms or in multiple units or
submultiple of it (often measured in
grams).

4. VOLUME
• Volume of a body is the place or space it
occupies. There are many different sizes.
To express the volume of a body is the
cubic metre (m³) and other multiples and
submultiples.

5. ELEMENTS, COMPOUNDS AND
MIXTURES
• Substances that make up matter can be
classified into elements, compounds and
mixtures.

6. ELEMENTS AND COMPOUNDS
• Elements are substances which are
formed by atoms equal, that is of the same
nature. For example: iron, gold, silver,
calcium, etc.
• Compounds are composed of different
atoms.

7. ELEMENTS AND COMPOUNDS
• Water and hydrogen are examples of pure substances.
Water is a compound while the hydrogen is an element.
The water is only made up of two atoms of hydrogen and
one of oxygen and hydrogen by two hydrogen atoms.
• If water changes state, its composition does not vary
because it is a pure substance, but if it undergoes
chemical changes water can be decomposed into
hydrogen and oxygen atoms.
• With the hydrogen cannot be the same. If you are
subjected to heat, the molecule will continue to be
constituted by hydrogen atoms. If you try to separate by
chemical means it always will be hydrogen.

8. ELEMENTS AND COMPOUNDS
• There are over 100 known chemical
elements (see table periodic items) and
more than one million compounds in
nature.

9. MIXTURES
• The mixtures are obtained from the
combination of two or more substances
that can be elements or compounds.
• In mixtures not laying down chemical
bonds between the components of the
mixture.
• Mixtures can be homogeneous or
heterogeneous.

10. HOMOGENEOUS MIXTURES
• Homogeneous mixtures are those in which
all its components are distributed
uniformly, i.e. the concentration is the
same in all the mix, in other words in the
mix there is a single phase.
• Examples of homogeneous mixtures are
the lemonade, salt dissolved in water, etc.
This type of mixture is called solution or
dissolution.

11. HETEROGENEOUS MIXTURES
• Heterogeneous mixtures are those in which its
components are not distributed evenly in the
mix, i.e., there is more than one phase; each of
them retains its features.
• Example of this type of mixture is the water with
oil, sand dissolved in water, etc; both examples
shows that as much as try to dissolve a
substance in another always last a certain time
they separate and each retains its features.

12. PROPERTIES OF MATTER
• Matter properties correspond to specific
characteristics by which a particular substance
can be distinguished from another.
• These properties can be classified into two
groups:
• Physical properties: depend essentially of the
same substance. Can be cited as an example:
the colour, the smell, the texture, the taste, etc.
• Chemical properties: depend on the behaviour of
matter from other substances. For example, the
oxidation of a nail (consists of iron).

13. PHYSICAL PROPERTIES
• Physical properties can be classified in turn into
two groups:
• Extensive physical properties: depend on the
amount of material present. They correspond to
the mass, volume, length.
• Intensive physical properties: depend only on
the material, regardless of the amount you have,
the volume deal with, etc. For example, a litre of
water has the same density than one hundred
litres of water

14. PHYSICAL STATES OF MATTER
• In conditions not extreme temperature,
matter can occur in three different physical
States: solid, liquid and gaseous state.

15. THE SOLIDS
• The solids have own form as a result of its
rigidity and its resistance to any deformation.
• The density of the solids is in general very little
more than the liquid, so not you can think that
such rigidity characteristic of solids is attributable
to greater proximity of its molecules. In addition,
there are even solids as the ice which is less
dense than the liquid from which they come.
• They also occupy a given volume and are
dilated to increase the temperature.

16. THE FLUIDS
• Fluids are characterized by having an own
volume, adapt to the shape of the vessel in
which they are contained, power flow, be very
compressible and move to the State of steam at
any temperature.
• They are little compressible under pressure,
because, unlike what happens in the case of
gases, liquids in the average distance between
molecules is very small, and thus if it shrinks
further, originate intense repulsive forces
between molecules of the liquid.

17. THE GASES
• Gases are characterized because they
completely fill the space in which they are
locked.
• If the container increases volume gas
immediately takes the new space, and this is
possible only because there is a force directed
from within the gas towards the walls of the
container that contains.
• The pressure is the force per unit area.
• The gases are easily compressible and able to
expand indefinitely.

18. • The bodies can change from State to vary
the pressure and temperature.
• In nature water changes state to modify
the temperature; it occurs in solid state,
such as snow or ice, as liquid and
gaseous vapour of water (clouds).

19. LIVING AND INERT MATTER
• The Earth is home to many living things, such as
plants and animals.
• A butterfly seems something very different from
a stone; however, both are composed of atoms,
but they are combined differently in one case.
• Most of the area is inanimate; i.e., it does not
grow, reproduces, or moves by itself. Good
examples of inanimate matter are the rocks that
make up the Earth.

20. CHANGES OF MATTER
• Changes that may experience matter can
be grouped in two fields:
• Chemical changes
• Physical changes

21. PHYSICAL CHANGES
• Physical changes are those where there is not any
alteration or change in the composition of the substance.
• Include physical changes state (melting, evaporation,
sublimation, etc.) changes, and changes in size or
shape.
• For example, when a piece of silver has been
transformed into a ring, a fortune cookie, pair of earrings,
there have been physical changes because the silver
maintains its properties in different objects.
• In general, the physical changes are reversible, i.e., you
can return to obtain the substance in its initial form

22. CHEMICAL CHANGES
• Chemical changes are transformations
experienced by a substance when its structure
and composition vary, giving rise to the
formation of one or more new substances.
• The substance is transformed into one or more
other substances different from the original.
• These chemical bonds will determine the
properties of the new substance or substances.

23. • The majority of chemical changes are
irreversible.
• Examples: to burn a role we cannot get it again
from the ashes and gases released in
combustion.
• However, there are other chemical changes that
the addition of another substance causes the
obtaining of the original substance and in this
case it is a reversible chemical change.
• Thus, to trigger a reversible chemical change
should lead to other chemical change.

24. CHANGES OF PHYSICAL
SATATES MATTER
• Changes of fitness as apply you heat or
apply you cold. When heat is applied to
the bodies it speaks of progressive
changes of State of matter. When bodies
are frozen talks about regressive state
changes.

25. PROGRESSIVE CHANGES IN
STATE
• 1. Sublimation: this change occurs when a body passes from the
solid state to the gaseous directly. The gradual sublimation occurs
only in some substances such as iodine and naphthalene.
• 2 Merger. It is the passage of a substance from the solid state to the
liquid by the action of heat. The temperature at which melting
occurs is characteristic of each substance. For example the
temperature which occurs the melting ice is or ° C while the iron is
1,525 ° c. Constant temperature which occurs the fusion is known
as melting point.
• 3 Evaporation. It is the passage of a substance from the liquid to the
gaseous. This change of State occurs normally at room
temperature, and without having to apply heat. Under these
conditions, only the surface of the liquid particles will pass to a
gaseous state, while those which are below will remain in the initial
state.

26. REGRESSIVE CHANGES IN
STATE
• 1. Solidification. It is the passage of a substance from
the liquid to the solid. This process occurs at a typical
temperature for every substance called point of
solidification and agreed with its melting point.
• 2. Condensation. It is the state change that occurs in a
substance from the gaseous state to the liquid state. The
temperature to which this transformation occurs is called
dew point and corresponds to the boiling point of that
substance. This change of State is one of the most
exploited by man in the fractional distillation of oil
derivatives such as paraffin, gas station and gas pipeline
are obtained by means of which.