States of Matter
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Transcript of States of Matter
Chapter 2:Chapter 2:Matter & ChangeMatter & Change
I. States of Matter
– Kinetic Molecular Theory
– States of Matter
A. Kinetic Molecular TheoryA. Kinetic Molecular Theory
KMT
– Matter is made of tiny particles
– Particles of matter are always in motion.
– The kinetic energy (speed) of these particles increases as temperature increases.
B. Four States of MatterB. Four States of MatterSolids
– very low KE - particles vibrate but can’t move around
– fixed shape
– fixed volume
– Not easily compressed
B. Four States of MatterB. Four States of MatterLiquids
– low KE - particles can move around but are still close together
– variable shape (that means they take the shape of the container)
– fixed volume– Not easily compressed
B. Four States of MatterB. Four States of MatterGases
– high KE - particles can separate and move throughout container
– variable shape (that means they take the shape of the container)
– variable volume (that means it will expand to fit the size of its container)
– Easily compressed
B. Four States of MatterB. 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, flat screen TVs
Quickie QuestionsQuickie Questions
This theory says particles are always in motion?
What are the four states of matter?
What state of matter has fixed volume and shape?
What state of matter consists of charged particles
Kinetic Molecular Theory
Solid, Liquid, Gas, Plasma
Solid
Plasma
Ch. 2 Matter & ChangeCh. 2 Matter & Change
II. Classification of Matter
–Matter Flowchart
–Pure Substances
–Mixtures
Matter FlowchartMatter 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 FlowchartA. Matter Flowchart
Examples:
– graphite
– pepper
– sugar (sucrose)
– paint
– soda
Element (Carbon)
heterogeneous mixture
compound
heterogeneous mixture
solution
B. Pure SubstancesB. Pure SubstancesElement
– Simplest form of matter that has a unique set of properties
– composed of identical atoms– EX: copper wire, aluminum foil
B. Pure SubstancesB. Pure Substances
CompoundCompound
– composed of 2 or more elements in a composed of 2 or more elements in a fixed ratio fixed ratio
2:1 - like H2:1 - like H22O or O or
1:1 like NaCl1:1 like NaCl
– properties differ from those of properties differ from those of individual elementsindividual elements
– EXEX: table salt (NaCl): table salt (NaCl)
B. Pure SubstancesB. 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 SubstancesB. Pure Substances For example…
Two different compounds, each has a definite composition.
C. MixturesC. Mixtures
Variable combination of 2 or more pure substances.
Heterogeneous Homogeneous
C. MixturesC. Mixtures
Homogeneous Mixture (aka Solution)– homogeneous– very small particles– no Tyndall effect
Tyndall Effect
particles don’t settleEX: rubbing alcohol
C. MixturesC. Mixtures
Heterogeneous Mixture
Colloid– heterogeneous– medium-sized particles– Tyndall effect– particles don’t settle– EX: milk
C. MixturesC. Mixtures
Heterogeneous MixtureSuspension
– heterogeneous– large particles– No true Tyndall effect– particles will settle– EX: fresh-squeezed
lemonade
C. MixturesC. Mixtures
Examples:
– mayonnaise
– muddy water
– fog
– saltwater
– Italian salad dressing
colloid
suspension
colloid
solution
suspension
Ch. 2: Matter & ChangesCh. 2: Matter & Changes
III. Properties & Changes
Extensive vs. Intensive
Physical vs. Chemical
A. Extensive vs. IntensiveA. 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. IntensiveA. Extensive vs. Intensive
Examples:
– boiling point
– volume
– mass
– density
– conductivity
Intensive
Extensive
Extensive
Intensive
intensive
B. Physical vs. ChemicalB. 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. ChemicalB. Physical vs. Chemical
Examples:
– melting point
– flammable
– density
– magnetic
– tarnishes in air
Physical
Chemical
Physical
Physical
Chemical
B. Physical vs. ChemicalB. 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. ChemicalB. Physical vs. Chemical
Signs of a Chemical Change
–change in color or odor
– formation of a gas
– formation of a precipitate (solid)
–change in energy (light or heat)
B. Physical vs. ChemicalB. Physical vs. Chemical
Examples:
– rusting iron
– dissolving in water
– burning a log
– melting ice
– grinding spices
chemical
physical
chemical
physical
physical
B. Physical vs. ChemicalB. Physical vs. Chemical
Law of Conservation of MassMass can not be created nor destroyed
*Mass of Reactants = Mass of Products