View
69
Download
0
Category
Preview:
DESCRIPTION
Matter: Properties & Change. A. Matter. MATTER – ANYTHING THAT HAS MASS AND TAKES UP SPACE EVERYTHING AROUND US CHEMISTRY – THE STUDY OF MATTER AND THE CHANGES IT UNDERGOES. MIXTURE. PURE SUBSTANCE. yes. no. yes. no. Is the composition uniform?. Can it be chemically decomposed?. - PowerPoint PPT Presentation
Citation preview
Matter: Properties & Change
A. Matter
• MATTER – ANYTHING THAT HAS MASS AND TAKES UP SPACE
– EVERYTHING AROUND US
• CHEMISTRY – THE STUDY OF MATTER AND THE CHANGES IT UNDERGOES
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
ANUDDER FLO CHART
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)
C. Mixtures
• Variable combination of 2 or more pure substances.
Heterogeneous Homogeneous
C. Mixtures
• Solution– homogeneous– very small particles– particles don’t settle– EX: rubbing alcohol
SOLUTE, SOLVENT AND SOLUTION
C. Mixtures
• Heterogeneous–medium-sized to
large-sized particles
– particles may or may not settle
– EX: milk, fresh-squeezed
lemonade
SOLUTIONS, SUSPENSIONS AND COLLOIDS
PROPERTIES
C. Mixtures• Examples:
– tea
– muddy water
– fog
– saltwater
– Italian salad dressing
• Answers:– Solution
– Heterogeneous
– Heterogeneous
– Solution
– Heterogeneous
A. Physical Properties• Physical properties can be described
as one of 2 types:
• Extensive Property
– depends on the amount of matter present (example: length)
• Intensive Property
– depends on the identity of substance, not the amount (example: scent)
A. Physical Properties
• Physical Property
– can be observed without changing the identity of the substance
F. Physical Changes
• Physical Change
– changes the form of a substance without changing its identity
– properties remain the same
• Examples: cutting a sheet of paper, breaking a crystal, all phase changes
F. Phase Changes – Physical
• Evaporation =
• Condensation =
• Melting =
• Freezing =
• Sublimation =
Liquid -> Gas
Gas -> Liquid
Solid -> Liquid
Liquid -> Solid
Solid -> Gas
D. Chemical Properties
• Chemical Property– describes the ability of a substance to
undergo changes in identity
G. Chemical Changes
• Process that involves one or more substances changing into a new substance– Commonly referred to as a chemical
reaction– New substances have different
compositions and properties from original substances
FAMOUS CHEMICAL STUFF U SHOULD KNOW #JIMMY NEUTRON
• ACIDS - THINGS THAT RELEASE HYDROGEN IONS ( H + ) WHEN DISSOLVED IN WATER
• BASES ( ALKALINE ) - THINGS THAT RELEASE HYDROXIDE IONS ( OH - ) WHEN DISSOLVED IN WATER
• THE pH SCALE MEASURES THE RANGE OF ACIDS/BASES
NURD WARNING
• PH CAN BE VIEWED AS AN ABBREVIATION FOR POWER OF HYDROGEN - OR MORE COMPLETELY, POWER OF THE CONCENTRATION OF THE HYDROGEN ION.
• THE MATHEMATICAL DEFINITION OF PH IS A BIT LESS INTUITIVE BUT IN GENERAL MORE USEFUL. IT SAYS THAT THE PH IS EQUAL TO TO THE NEGATIVE LOGARITHMIC VALUE OF THE HYDROGEN ION (H+) CONCENTRATION, OR
• PH = -LOG [H+]
• PH CAN ALTERNATIVELY BE DEFINED MATHEMATICALLY AS THE NEGATIVE LOGARITHMIC VALUE OF THE HYDROXONIUM ION (H3O+) CONCENTRATION. USING THE BRONSTED-LOWRY APPROACH
• PH = -LOG [H3O+]
• TOLD YA IT WAS NURDY
pH SCALE
7 IS YOUR FRIEND
G. Chemical Changes
• Signs of a Chemical Change
– change in color or odor
– formation of a gas
– formation of a precipitate (solid)
– change in light or heat
E. Physical vs. Chemical Properties
• Examples:
–melting point
– flammable
– density
–magnetic
– tarnishes in air
physical
chemical
physical
physical
chemical
H. Physical vs. Chemical Changes
• Examples:
– rusting iron
– dissolving in water
– burning a log
–melting ice
– grinding spices
chemical
physical
chemical
physical
physical
What Type of Change?
What Type of Change?
B. Four States of Matter
• Solids– particles vibrate but can’t move
around
– fixed shape
– fixed volume
– incompressible
B. Four States of Matter
• Liquids– particles can move
around but are still close together
– variable shape
– fixed volume
– Virtually incompressible
B. Four States of Matter
• Gases– particles can separate and
move throughout container– variable shape– variable volume– Easily compressed– Vapor = gaseous state of a
substance that is a liquid or solid at room temperature
B. Four States of Matter
• Plasma– particles collide with enough energy
to break into charged particles (+/-)
– gas-like, variableshape & volume
– stars, fluorescentlight bulbs, TV tubes
STATES OF MATTER
• The Four States of Matter
• Four States• Solid• Liquid• Gas• Plasma
STATES OF MATTER
Based upon particle arrangementBased upon energy of particlesBased upon distance between particles
Kinetic Theory of Matter
Matter is made up of particles which are in continual random motion.
STATES OF MATTERSOLIDS
•Particles of solids are tightly packed, vibrating about a fixed position.
•Solids have a definite shape and a definite volume. Heat
STATES OF MATTERLIQUID
Particles of liquids are tightly packed, but are far enough apart to slide over one another.
Liquids have an indefinite shape and a definite volume. Heat
STATES OF MATTERGAS
Particles of gases are very far apart and move freely.
Gases have an indefinite shape and an indefinite volume. Heat
PHASE CHANGESDescription of Phase Change
Term for Phase Change
Heat Movement DuringPhase Change
Solid to liquid
MeltingHeat goes into the solid as it melts.
Liquid to solid
FreezingHeat leaves the liquid as it freezes.
PHASE CHANGESDescription of Phase Change
Term for Phase Change
Heat Movement During Phase Change
Liquid to gas
Vaporization, which includes boiling and evaporation
Heat goes into the liquid as it vaporizes.
Gas to liquid
CondensationHeat leaves the gas as it condenses.
Solid to gas SublimationHeat goes into the solid as it sublimates.
LATENT HEAT = HEAT ABSORBED WHEN CHANGING PHASE
Specific HEAT CAPACITY = THE AMOUNT OF HEAT NEEDED TO RAISE 1 GRAM OF MATERIAL 1DEGREE C
But what happens if you raise the temperature to super-high levels…
between 1000°C and 1,000,000,000°C ?
Will everything just be a gas?
STATES OF MATTERPLASMA
A plasma is an ionized gas.
A plasma is a very good conductor of electricity and is affected by magnetic fields.
Plasmas, like gases have an indefinite shape and an indefinite volume.
• Plasma is the common state of matter
STATES OF MATTER
SOLID LIQUID GASPLASM
A
Tightly packed, in a regular pattern
Vibrate, but do not move from place to
place
Close together with no regular
arrangement.Vibrate, move
about, and slide past each other
Well separated with no regular
arrangement.Vibrate and move
freely at high speeds
Has no definite volume or shape
and is composed of electrical charged
particles
Some places where plasmas are found…
1. Flames
2. Lightning
3. Aurora (Northern Lights)
MATTER REVIEW
QUIZLET CH 2QUIZLET CH 3
SAYS TO DO YOUR
MATH AND LIKE IT
SAYS TO DO YOUR
MATH AND LIKE IT
Recommended