Nature and State of Matter
The five main principles of Leucippus and Democritus' theory include the following:
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All matter is made up of atoms that are too tiny to be seen by the naked eyes. They
cannot be broken down into smaller portions. All forms of Matter result from the
coming together or breaking apart of atoms.
Atoms are in constant motion around an empty space called void.
Atoms are completely solid.
Atoms are uniform, with no internal structure.
Atoms come in different shapes and sizes.
States of Matter
Matter
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Solid
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Liquid
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Gas
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Plasma
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anything that occupies space and has mass
it can be in the form of solid, liquid, gas, plasma and bose-einstein condensate
Has definite shape and volume
Cannot be compressed by a moderately high pressure
Very slight expansion during heating
High density
Particles are in relatively fixed position and wiggle in their position.
Examples are pencil, board, eraser
No definite shape; takes the shape of the container
Has definite volume
Can be compressed (but only to a negotiable extent) by a moderately high pressure
Slight expansion during heating.
Medium density
Particles are close to one another and move past one another
-No definite shape; takes the shape of the container
Has no definite volume.
Can be compressed or expanded as pressure is increased or decreased
Great expansion during heating.
Low density
Particles are far apart, move randomly, and repeatedly collide with one another
is the fourth state of matter. Formed by heating and ionizing a gas, plasma is made
up of groups of negatively and positively charged particles. Plasma are not the
same as gases; they have neither a definite volume nor a definite shape. They are
often observed in ionized gases, aurora borealis, lightning and comet.
Bose- Einstein Condensate
 is the fifth state of matter that produced when a cloud of bosons (a type of
elementary particle of matter) is cooled to temperatures very close to absolute zero
such that large fraction of the bosons condenses. Bose Einstein include superfluid
like cold liquid helium, and superconductors like nucleons inside a neutron star.
Properties of matter provide a basis for its identification and for differentiating it from
other substances. These properties can either be physical or chemical; or can also be
intensive or extensive.
Physical Properties
Physical properties are those perceived by the senses that can be observed, measured, and
tested without changing the composition of the matter.
Physical properties include phase (solid, liquid or gas), color, solubility, density, melting, shape,
melting point, boiling point, hardness, volume, mass, and length.
Example:
Gold is yellow in color.
- The act of observing the color of gold does not change its composition. The same is
true in observing its physical state as a solid and in noting its ability to conduct an
electricity. Determining a physical property of matter may be accompanied by a
change in its physical state.
Example:
- Determining the boiling point of water by finding the temperature.
Physical properties can be classified into two: intensive or extensive properties.
1. Intensive Properties
- are properties that do not depend on the amount of matter present or being
measured. if there is a change in the amount of matter, these properties will
remain the same.
Color is the quality of an object that is reflected with respect to the wavelength of
transmitted light.
Example: Sulfur is yellow
Hardness is the ability of a material to resist scratching.
Example: Hardness of wood
Boiling Point is the temperature at which the solid turns to liquid.
Example: Boiling point of water
Melting Point is the temperature at which the solid turns to liquid.
Example: When ice melt, it
turns from solid to liquid.
Density a mass per unit volume of the matter determines whether a substance will
float on water.
Example: A Styrofoam floats on a water.
2. Extensive Properties
- are properties that depend on the amount of matter present or being tested. If
there is a change in the amount of matter, these properties will change too.
Volume is a derived unit from length, width and height of the substance or from the
space the substance is occupying.
Example: The student measure the length, width and height of a wooden block.
Mass is the actual quantity of matter that a substance contains.
Example: Maria bought 5 kg of rice.
Length is the distance between two points.
Example: The distance between the two tables is five feet.
Shape is the outline of an object with respect to its circumference.
Example: The crystalline shape of halite is cube.
Chemical Properties
- Chemical properties are those involved in the transformation of substances into
other materials which possess a completely different structure and composition
from the original.
Chemical properties include flammability, toxicity, combustibility, reactivity and
oxidation.
1. Flammability
- is the ability to catch fire and burn easily at normal working temperature.
2. Toxicity
- is how dangerous a chemical to organisms and to environment
3. Combustibility
- is the ability to be burnt at temperature that are above normal working
temperature.
4. Reactivity
- is a measure of how likely a sample is to participate in a chemical reaction under
variety of conditions.
Example: Iron nails become dull when exposed to air
5. Oxidation
- is the resistance of a substance to change in the presence of oxygen.
Example: Burning of paper.
- It is under flammability which is the ability of a substance to burn when in contact
with flame, producing substances. When you are burning a paper it is converted to
carbon dioxide and water, new substances with different chemical composition
than the paper.
Classifications of Matter
Pure Substance
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contains only one type of particle and has same element all throughout
can be classified into element and compound
Classification of Pure Substance
1. Element
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are substances composed of only one kind of atom
examples can be seen in the periodic table of elements
Classification of Elements
1.1 Metal
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lustrous
malleable
ductile
good conductors of heat and electricity
mostly hard
have high densities
Metalloid
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elements which have both the properties of metal and nonmetals
form a staircase pattern located between the metal and nonmetal in periodic table
of elements
example: boron, silicon, germanium, arsenic, antimony, tellurium, polonium and
astatine
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1.3 Nonmetal
 dull in appearance
 brittle
 poor conductor of heat and electricity
 good insulators
 exists in three states (solid, liquid and gas) at room temperature
 have low densities
2. Compound
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substances composed of two or more kinds of atoms that are chemically
bonded together in fixed proportion
can be classified into acid, base or salt
Classification of Compound
2.1 Acid
 a compound that donates H+ ions in an aqueous solution
 tastes sour
 produce a piercing pain in wound
 turns blue litmus paper to red
 examples are vinegar, citrus fruits, soft drinks
2.2 Salts
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compound that is formed when acid and base reacts
this reaction where salt and water are formed is called neutralization
examples are table salt, calcium chloride
2.3 Base
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a compound that accepts H+ ions in an aqueous solution
tastes bitter
fell slippery to the touch
turns red litmus paper to blue
examples are soap, ammonia, detergent powders, baking soda
Mixtures
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are made up of two or more substances mixed together but not chemically
combined
can be homogeneous or heterogeneous
Classification of Mixtures
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Homogeneous
 a mixture that has a uniform composition and also called a solution
 particles are difficult to distinguish from one another
 can be classified to different types of solution
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Heterogeneous Mixture
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Type of mixture that has two or more phases
It doesn't have a uniform composition
One substance can be separated easily from other substance
Can be classified into colloid or suspension
Classification of Heterogeneous Mixture
1. Colloid
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Particles are larger than the particles of solution but smaller than the
particles of suspension
Particles are evenly distributed throughout the mixture
Particles does not settle at the bottom
Seemingly homogeneous but particles are recognizable under microscope
Suspension
 Particles are bigger than those of colloids
 Contains solid particles that eventually settle
 Examples are sand and water, food and beverages having a "shake well
before using” notice
Methods of Separating of Mixtures
The component of mixtures are pure substances which have different physical
properties such as solubility, density, and boiling points. Using this properties one
can select a method on how to separate the components of a mixture.
1. Filtration
 Often used to separate water- soluble from insoluble components
 Requires filtering medium (cheesecloth or filter paper)
 Residue- are solid components that remains in the filtering medium
 Filtrate- the clear liquid collected
 Example is silver chloride and potassium nitrate
2. Sedimentation
 Heavy suspended particles are allowed to settle at the bottom of the
container
 Followed by decantation
3. Decantation
 A process of separating a solid from a liquid, by pouring off the liquid
after sedimentation
 Example is sand and water
4. Dissolution
 Is another method in which a mixture of a soluble and insoluble solid
substances can be separated by using an appropriate solvent. The
solvent chosen will either dissolve any of the solid substances in the
mixture. The one that is not dissolved in the chosen solvent can be
removed by filtration.
 Example is salt and sand
5. Sublimation
 Is the process of changing solid to the gaseous form without passing
through the liquid state.
 Example is naphthalene and salt mixture.
6. Distillation
 A process where by a liquid is converted into a vapor by boiling and
the vapor is converted back to liquid by cooling
 Simple distillation is used if the impurities are not volatile and the
liquid compound does not decompose at its boiling point
 Fractional distillation is used to separate two or more immiscible
liquids with different boiling points.
7. Crystallization
 Is a method to separate a soluble solid from its solution based from the
different solubility of solid in water at 25 degrees Celsius. Generally,
the solubility of most of solids increases as the temperature increases.
Therefore, when a so-called saturated solution is cooled, the solubility
of the solid substances will decrease and the excess solid will
crystallize.
8. Chromatography
 A process utilizing the strategy that lets the mixture flow over a
material that retains some component more so different components
flow over the material at different speeds.
 It has two components, the mobile phase and the stationary phase.
9. Centrifugation
 A process of separating mixtures by applying centripetal force to a
mixture using a centrifuge machine
10. Evaporation
 This process involves the application of heat to the solution to allow
the solvent to evaporate leaving behind the solid component as a
residue
11. Use of Magnet
 Used when separating metallic and non- metallic substances.
12. Use of Separatory Funnel
 Used to facilitate the separation of liquid- liquid mixture that did not
mix.