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Chapter 3 Matter
I. Properties & Changes in Matter
Extensive vs.
Intensive
Physical vs.
Chemical
A. Extensive vs. Intensive
Extensive Property
depends on the amount of matter present
Intensive Property
depends on the identity of substance, not the amount
A. Extensive vs. Intensive
Examples:
boiling point
volume
mass
density
conductivity
intensive
extensive
extensive
intensive
intensive
B. Physical vs. Chemical
Physical Property
can be observed without changing the identity of the substance
Click for movie
Chemical Property
describes the ability of a substance to undergo changes in identity
B. Physical vs. Chemical
Examples:
melting point
flammable
density
magnetic
tarnishes in air
physical
chemical
physical
physical
chemical
B. Physical vs. Chemical
Physical Change
changes the form of a substance without changing its identity
properties remain the same
Chemical Changechanges the identity of a substanceproducts have different properties
B. Physical vs. Chemical Signs of a Chemical Change
change in color or odor
formation of a gas
formation of a precipitate (solid)
change in light or heat
B. Physical vs. Chemical
Examples:
rusting iron
dissolving in water
burning a log
melting ice
grinding spices
chemical
physical
chemical
physical
physical
Chemical verses physical changeWhich one is a physical change?
A. Sodium reacting B. Iodine changing with chlorine. from a solid to a gas
Matter
II. States of Matter
Kinetic Molecular Theory
States of Matter
Click for movie
Physical Properties
States of matter
solid liquid gas
A. Kinetic Molecular Theory
KMT
Particles of matter are always in motion.
The kinetic energy (speed) of these particles increases as temperature increases.
B. Four States of Matter
Solids very low KE - particles
vibrate but can’t move around
fixed shape fixed volume
B. Four States of Matter
Liquids low KE - particles can
move around but are still close together
variable shape fixed volume
B. Four States of Matter
Gases high KE - particles can
separate and move throughout container
variable shape variable volume Click for movie
The States of Matter
VAPORIZATION
CONDENSATIONMELTING
FREEZING
Changes of State
Melting - the transition from the solid substance into a liquid The melting Point
Freezing or Fusion - liquid to solid The Freezing point
When does water melt? When does water freeze?
Changes of State
Boiling or Vaporization or Evaporation
liquid to gas Condensation - gas to liquid
Sublimation - solid to gas Deposition - gas to solid
B. Four States of Matter
Plasma very high KE - particles collide with
enough energy to break into charged particles (+/-)
gas-like, variableshape & volume
stars, fluorescentlight bulbs, CRTs
Matter
III. Classification of Matter
Matter Flowchart
Pure Substances
Mixtures
A. Matter Flowchart
MATTER
Can it be physically separated?
Homogeneous Mixture
(solution)
Heterogeneous Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be chemically decomposed?
noyesIs the composition uniform?
noyes
Colloids Suspensions
A. Matter Flowchart
Examples:
graphite
salt & pepper
sugar (sucrose)
paint
soda
element
hetero. mixture
compound
hetero. mixture
solution
B. Pure Substances
Element composed of identical atoms Ex: copper wire, aluminum foil
B. Pure Substances
Compound
composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
Ex: table salt (NaCl)
B. Pure Substances
Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.
B. Pure Substances
For example…
Two different compounds, each has a definite composition.
C. Mixtures
Variable combination of 2 or more pure substances.
Heterogeneous Homogeneous
C. Mixtures
Solution homogeneous very small particles no Tyndall effect Tyndall Effect
particles don’t settle EX: rubbing alcohol
C. Mixtures
Colloid heterogeneous medium-sized particles Tyndall Effect particles don’t settle EX: milk
C. Mixtures
Suspension heterogeneous larger particles Tyndall Effect particles settle EX: fresh-squeezed
lemonade with pulp
Heterogeneous Mixtures
Heterogeneous mixtures occur when you can see the physical differences between the substances.
Is a salt and water mixture a heterogeneous mixture?
Is a mixture of sand and water a heterogeneous mixture?
Rubbing Alcohol
Oil
Corn syrup
C. Mixtures
Examples:
milk
muddy water
fog
salt & water
Italian salad dressing
colloid
suspension
colloid
solution
suspension
Physical Separation Techniques
Mixtures are combinations of two or more substances that when mixed do not change.
Therefore, physical properties can be used to separate them.
What physical properties could be used? Think about how you could separate iron,
salt and sand. Total Cereal
Physical Separations
Filtering Separation by the
physical property of solubility. One substance is soluble the other is not.
Coffee filters Tea bags Spaghetti
Physical Separations
Chromatography Separation by
solubility, mass or bonding properties
Separation of inks Separation of M&M
dyes Separation of leaf
pigments.
Physical Separations
DistillationSeparation by
the physical properties of melting point or boiling point
Purifying water