Transcript Classification of Matter

Classification of Matter
Integrated Physic and Chemistry
Fall 2014
CLASSIFICATION OF MATTER
1.DISTINGUISH
BETWEEN MASS
AND MATTER.
 Mass - the quantity of
matter in an objectmeasured in grams
 Matter - anything that
has mass and occupies
space- (anything that
has mass and volume)
CLASSIFICATION OF MATTER
 2. STATE THE KINETIC
THEORY OF MATTER.
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- matter is made of tiny
particles called atoms
- these atoms are in
constant motion
- adding heat makes the
atoms move faster and
farther apart
- removing heat makes the
atoms move slower and
closer together
CLASSIFICATION OF MATTER
LIST THE FOUR STATES OF MATTER.
 The four states of matter are solid, liquid, gas and
plasma.
 4. IDENTIFY MAJOR CHARACTERISTICS OF
SOLIDS, LIQUIDS AND GASES.
 3.
Solids
Liquids
Gases
Shape
definite
shape of its
container
fill its container
(takes the shape)
Volume
definite
definite
fill its container
Molecular
Attraction
strong
in between
weak
Particles
close together;
very strong force
holding them in
place- vibrate
flow past each
other
very far apart, very
weak force holding
them together
CLASSIFICATION OF MATTER
 5.
STATE THE LAW OF CONSERVATION OF
MASS.
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Matter cannot be created or destroyed in a chemical or
physical change.
 6.
DEFINE AND DESCRIBE PHYSICAL
PROPERTIES.

Physical Properties - characteristics which can be
observed without changing the chemical composition of
the substance
 - size, shape, color, smell, density, melting point,
freezing point, and boiling point
 7.
DEFINE AND DESCRIBE PHYSICAL
CHANGES.
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Physical change - a change in the appearance or
state of a substance but NOT it's chemical make-up
 -Examples are the evaporation of water, melting of ice,
dissolving of salt into water, and breaking a glass.
CLASSIFICATION OF MATTER
 8. DEFINE AND CALCULATE DENSITY.
 Density - a measure of mass per volume
 - The formula is D = m
v
 m = mass (grams)
 V = volume (ml or cm3)
 D = density (g/ml or g/cm3)
CLASSIFICATION OF MATTER
 9.
DEFINE AND DESCRIBE CHEMICAL
PROPERTIES
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Chemical Properties - those characteristics which depend
upon the reaction with another substance
- Examples are iron will rust, wood will burn, milk will sour,
and sodium will explode in water (it all depends on what you
mix it with).
 10. DEFINE AND DESCRIBE CHEMICAL
CHANGES.
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Chemical Changes - changes that produce new substances
which are chemically different than the original substances
- Examples are burning, rusting, combustion, flammability,
rotting, and digestion
CLASSIFICATION OF MATTER
 11.LIST INDICATIONS OF A
CHEMICAL CHANGE.
 (a)
production of a gas
 (b) permanent color change
 (c) formation of a precipitate
 (d) change in energy
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(1) endergonic - takes in energy
(2) exergonic - releases energy production of light
energy
CLASSIFICATION OF MATTER
 12. DESCRIBE AN ELEMENT.
 Element - a pure substance in which all of its
atoms are alike - refer to the periodic table of
elements
 13. DESCRIBE A COMPOUND.
 Compound - a pure substance made of two or
more elements that are chemically combined in a
definite proportion or ratio- compounds do not
usually look or behave like the elements from
which they are made
 (water, salt, sugar)
CLASSIFICATION OF MATTER
 14. DESCRIBE A MIXTURE.
 Mixture - composed of two or more substances,
simply mixed together.
 - CAN be separated easily by filtration,
evaporation, etc...
 - substances are NOT chemically combined
 Example are this class, tossed salad, and salt
water
 We will discuss in more detail in the next series of
notes.
CLASSIFICATION OF MATTER
 15. DEFINE AND GIVE EXAMPLES OF
FLUIDS.
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A fluid is any substance that can flow or be
poured.
Gases and liquids are fluids.
 16. DEFINE VISCOCITY.
 Viscosity is a fluid's resistance to flow.
 The higher the viscosity, the slower it pours.
(syrup, motor oil)
 Temperature affects viscosity
Mixtures
Integrated Physic and Chemistry
Fall 2014
MIXTURES
 1. A pure substance is either an
element or a compound. But a
mixture is made up of two or more
substances that can be separated
by physical means.
 2. There are two types of mixtures.
A
heterogeneous mixture differs
from point to point.
 A homogeneous mixture the same
throughout.
MIXTURES
 3. A solution is a homogeneous
mixture of two or more substances. A
solution consists of a solute and
solvent. The solute is dissolved into
the solvent.
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The solute usually occurs in the smaller
amount.
The solvent usually occurs in the larger
amount.
Solutions form when particles of the solute
spread out evenly in the solvent.
MIXTURES
 4. Water is described as the universal
solvent because more substances will dissolve
in water than any other known solvent. There
is no such thing as a true universal solvent!
 5. Five physical properties of solutions
are:
 a. It is homogeneous. (evenly mixed)
 b. Liquid solutions appear clear or
transparent. (does not mean colorless)
 c. Proportions may vary. (weak or strong)
 d. The solute will not settle from the
solvent.
 e. The solute cannot be filtered from the
solvent.
MIXTURES
 6. The rate of solution depends upon
3 factors: (how quickly something
dissolves)
a. Particle size (Crushing a sugar cube
will dissolve it faster).
 b. Stirring or shaking the mixture
increases the rate of solution. (solid into a
liquid - NOT gas into a liquid)
 c. Temperature (solids dissolve faster in
warmer solvents)
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MIXTURES
 7.
Solubility is the amount of solute that can
be dissolved in a given amount of solvent at a
given temperature. Amount of solvent and
temperature MUST be controls.
 8. The factors that determine IF
something will dissolve.
 a. Temperature - Solids dissolve more in
warm liquid solvents. Gases dissolve less in
warm liquid solvents.
 b. Pressure - Increased pressure will cause
more solute to stay in the solution (sodas)
 c. Nature of the solvent and solute
 Organic solvents dissolve organic solutes.
Inorganic solvents dissolve inorganic
solutes. Water is an exception.
MIXTURES
 9. A solubility curve is a graph showing how
much solute is dissolved in a solvent over a
range of temperatures.
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MIXTURES
 10. The methods of separating
mixtures are:
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a. Evaporation is removing water from
a solution or removing the liquid
portion from a mixture without adding
heat.
b. Distillation is the separation of two
liquids because of a difference in
boiling points.
c. Filtration is the removal of an
insoluble solid from a liquid mixture.
Filtrate is the portion of the mixture
that passes through the filter.
Evaporation, distillation and filtration
are all physical changes!
MIXTURES
 11. The levels of concentration are
unsaturated, saturated, or
supersaturated.
 An unsaturated solution will hold
more solute.
 A saturated solution will not
dissolve more solute.
 A supersaturated solution contains
more solute than usual because it
was
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(a) heated
(b) more solute added and then
(c) cooled back to original temperature.
(dissolving sugar in warm tea, then adding ice)
MIXTURES
 12. The addition of solute particles
raises the boiling point of a
solution. (anti-freeze in radiator).
The addition of solute particles
lowers the freezing point of a
solution.(salt on ice for homemade
ice cream or on sidewalks to melt
ice).
MIXTURE
 13. A comparison of solutions, colloids and
suspensions.
Solutions
Colloids
Suspensions
clear
Will scatter light
cloudy
Solute will not settle
Solute will not settle
Solute will settle
Homogenous
Heterogeneous
Heterogeneous
Cannot be filtered
Cannot be filtered
Can be filtered
Proportions may vary Proportions may vary Proportions may
vary
Kool-Aid, Soda, Iced
Tea
Gelatin, fog, milk,
paint
Muddy water, oil &
vinegar