ch. 1 - matter i. states of matter (p.12) kinetic molecular theory states of matter
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Ch. 1 - Matter
I. States of Matter (p.12)
Kinetic Molecular Theory
States of Matter
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
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
Ch. 1 - Matter
II. Classification of Matter
(p.15-17, 397-398)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
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 large particles Tyndall effect particles settle EX: fresh-squeezed
lemonade
C. Mixtures
Examples:
mayonnaise
muddy water
fog
saltwater
Italian salad dressing
colloid
suspension
colloid
solution
suspension
Ch. 1 - Matter
III. Properties & Changes in Matter (p.11-14)
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
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 Change
changes the identity of a substance
products 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