SCIENCE 7 MATTER

1. MATTER
T Y P E S , S TAT E S , A N D P R O P E R T I E S ,

2. MATTER
• Anything that occupies space and has mass.
• It has two types:
1. PURE SUBSTANCES – have uniform and definite composition. They
have constant physical and chemical properties.
2. MIXTURE – different substances are combined with no chemical
reaction taking place.

3. PURE SUBSTANCES has two types:
a. ELEMENT
b. COMPOUND
MIXTURE has two types:
a. HOMOGENEOUS MIXTURE
b. HETEROGENEOUS MIXTURE

4. PURE
SUBSTANCES

5. ELEMENTS
• Contains only one type of atom
• Cannot be broken down into simpler forms of matter.
• There are 118 known elements, most of them are naturally occurring
while some are synthesized or made in the laboratory.
Example:
C – Carbon (C – symbol, carbon – name)
Ne – neon; Pb – lead; W – tungsten; Mn – manganese

6. COMPOUNDS
• Contains two or more atoms that are chemically combined, elements
have undergone a chemical reaction.
• When compounds are formed, a new set of properties can be seen.
• Can still be broken down to simpler compounds or their corresponding
elemental components through chemical processes
• ELECTROLYSIS – splitting of compounds into the corresponding
elements with the use of electricity.
Example: salt (C6H12O6) – carbon, hydrogen, & oxygen
baking soda (NaHCO₃) – sodium, hydrogen, carbon, & oxygen
magnesium oxide (MgO2) – magnesium & oxygen

7. MIXTURE
• Can be separated into their individual components by physical
methods
• Methods in separating mixtures:
- distillation - evaporation
- extraction
- filtration
- using of magnet
- decantation

8. HOMOGENEOUS MIXTURE
• Also called as solution, are uniform all throughout, components are not
easily separated.
• Examples:
– Salt solution (salt and water)
– Coffee (coffee powder, hot water & sugar)
– Sea water (salt and water)
– Air (O, H, N, C)
– Soft drinks (water, sweetener, CO2, flavorings, etc.)

9. HETEROGENEOUS MIXTURE
• Have to or more phases, that is not uniform in appearance.
• Examples:
– Sugar and sand
– Vegetable salad (different vegetables, mayonnaise, etc.)
– Fruit salad (different fruits, creamer, condense, etc.)
– Salt and pepper
– Concrete (cement & water)

10. PROPERTIES OF
MATTERT R A I T S O F A N Y M A T E R I A L , P H Y S I C A L O R
C H E M I C A L P R O P E R T I E S .

11. PHYSICAL PROPERTIES
• Pertain to those that are measured without changing the composition
of the substance.
• This include color, odor, texture, boiling point, density, etc.
• It is categorized into:
A. Intensive properties – those that are inherent to the pure substance such
as density, color, melting point, and boiling point.
B. Extensive properties – incidental to the pure substance such as length,
mass, volume, height, and shape.

12. Difference between Intensive and Extensive
properties
INTENSIVE EXTENSIVE
Independent property Dependent property
Size does not change Size changes
It cannot be computed It can be computed
Can be easily identified Cannot be easily
identified
Example: melting point,
colour, ductility,
conductivity, pressure,
boiling point, lustre,
freezing point, odour,
density, etc
Example: length, mass,
weight, volume

13. Extensive examples:
• Lemon juice differ in volume
• Aluminum differ in sizes and
length depending on how it used
• Metals have different mass
according to its size
Intensive Properties Example
• Color - Aluminum metal is gray
colored.
• Taste - Lemon juice (citric acid) is
sour.
• melting point - Aluminum has
melting point of 660°C.
• boiling point - Water has a
boiling point of 100°C.
• Density - Water has a density of 1
g/mL.
• Luster - Metals are lustrous
(shiny).
• Hardness - Diamond is the
hardest substance known

14. 1. Which of the following is an intensive property of a box of crackers?
A. Calories per serving.
B. Total grams.
C. Total number of crackers.
D. Total calories.
2. Which of the following is an extensive property?
A. The color of charcoal is black.
B. Gold is shiny.
C. The volume of orange juice is 25 mL

15. CHANGES OF MATTER
1. Physical change – change without affecting the chemical composition
of matter. Example: grinding, breaking, crushing, breaking, and
changes in matter (E, C, F, S, S, D).
2. Chemical change – involves a change in the substance’s chemical
composition, new substance is formed/produced. Examples: rusting,
ripening of fruits, decomposition of plants/animals, and changing of
taste, etc.

16. STATES
OF
MATTERT H I N G S M A Y E X I S T I N T H R E E D I F F E R E N T
F O R M S O R P H Y S I C A L S T A T E S , T H E Y D I F F E R I N
T H E D I S T A N C E S B E T W E E N P A R T I C L E S A N D
T H E I R A R R A N G E M E N T .

17. SOLID STATE
• Particles are fixed in crystal lattices forming cubic structure, tetragonal
structure, etc.
• Particles are tightly packed together and as such movement is very
limited, molecules or atoms tend to only vibrate.
• Limited movement of the particles contributed to the rigid shape of
solid
• No free spaces can be found between the particles
• Particles cannot slide with one another, their position is fixed.
• Have definite shape and volume

18. LIQUID STATE
• Has a definite volume but always take the shape of the container
• Particles are not too tightly and as such they can move past each other.
• The molecules have greater kinetic energy and the attraction between
them is only large enough to hold these molecules or atoms together.

19. GASEOUS STATE
• Distance between particles are larger compared to their sizes and thus
there is freedom of movement
• Kinetic energy is much greater than the force of attraction.
• Do not have definite shape and volume
• Particles are far from each other, gases can be compressed.

20. PLASMA
• Consists of ionized gas making it electrically conductive and responsive
to strong electromagnetic fields
• Examples: lightning, polar aurorae, ionosphere, the sun, and the other
stars, also present inside the fluorescent lamps and in neon signs.

21. BOSE-EINSTEIN CONDENSATE
• Works of Albert Einstein and Satyendra Nath Bose
• Formed by a system of bosons that is confined in an external potential
and cooler near 0 K or absolute zero.
• First condensate was produced in 1995 by Eric Cornell and Carl
Weimann at the University of Colorado.
• such as cold liquid helium, or superconductors, such as the nucleons
inside a neutron star.