Properties and States of Matter Chapters 2 and 3.
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Transcript of Properties and States of Matter Chapters 2 and 3.
Properties and Statesof Matter
Chapters 2 and 3
Classifying Matter
Matter Anything that has mass and takes up space Either a pure substance or a mixture
end
Classifying Matter-Pure Substance
Pure Substance Matter that always has exactly the same make-up Either an element or a compound Salt, table sugar, water, gold, aluminum
end
Classifying Matter- Pure Substance Element
Something that cannot be broken down into simpler things
Given a 1 or 2 letter symbol on the Periodic Table (C, N, O, Au, Fe)
Carbon, iodine, gold, iron
end
Classifying Matter- Pure Substance Compound
Made from 2 or more things and can be broken down into those things
2 or more elements joined in a fixed proportion Water, table salt, sugar
end
Classifying Matter- Mixture Mixtures
Contains 2 or more elements with no fixed make-up
Heterogeneous Mixtures Can identify different parts of the mixture Does not look the same all the way through Salad dressing, sand/dirt
Homogeneous Mixtures Substances cannot be distinguished Looks the same all over Tap water, Fruit Punch, stainless steel
end
Classifying Matter- Mixtures
Solutions When something dissolves and forms a
homogeneous mixture Salt water, Kool-Aid, Sweet Tea
Suspension A heterogeneous mixture that separates into
layers over time Salad dressing, paint, liquid medicines
“Shake well before using”
end
Physical Properties
Physical property Something that can be observed or measured
without changing the material 7 physical properties you need to know
end
Physical Properties
Viscosity Liquid’s resistance to flowing Honey = high water = low
Conductivity Ability to allow heat/electricity to flow Iron = good rubber = bad
Malleability Solid’s ability to be hammered without shattering Gold = very glass = not
end
Physical Properties
Hardness Ability of something to cut something else Diamond is the hardest substance on Earth
Melting Point Temp. where a substance goes from a solid to a liquid
Boiling Point Temp. where a substance gores form a liquid to a gas
end
Physical Properties
Density (D) A substances’ mass divided by its volume
Measured in either g/mL or g/cm3
Remember: 1 mL = 1 cm3 !!! Things that are more dense will sink, Things that
are less dense will float
V
mD
Density
(g/mL or g/cm3)
mass
(g)
Volume
(mL or cm3)
end
Physical Properties
A rock has a mass of 12 g. If it has a volume of 50 mL, what is the rock’s density?
A block has a density of 0.005 g/cm3. If the block has a volume of 56 mL, what is the block’s mass?
A graduated cylinder has 13.4 mL of water. When a marble, with a density of 6.2 g/mL, is dropped in the cylinder the water level rises to 34 mL. What is the marble’s mass?
end
Using Physical Properties
Physical properties are used for: Identifying a material Choosing a material for a specific purpose To separate the substances in a mixture
end
Separating Mixtures
Filtration Separates materials based on the size of their
particles Using a coffee filter
Distillation Separates things in solution based on boiling points Making moonshine
end
Chemical Properties
Chemical property A property that produces a change in something’s
composition Something is changing into something else
end
Chemical Properties
Flammability Ability to burn in the presence of oxygen Different elements burn different colors Think fireworks!!!
Reactivity How quickly something combines with other
things
end
Physical vs. Chemical Changes Physical Change
Some properties of a substance change, but the substance is still the same
Shredding paper, breaking glass, ice cube melting
end
Physical vs. Chemical Changes Chemical Change
When a substance reacts and forms one or more new substances
The composition of the matter changes
end
Physical vs. Chemical Changes Evidence of a chemical change:
Change in color Copper roof -> green
Production of a gas See bubbles forming
Formation of a precipitate Forms a solid
Temperature change Production of light
end
States of Matter
There are 5 states of matter (phases of matter) We only care about 3 of them
Solid Liquid Gas
end
States of Matter- Solids
Solid Something with a fixed shape
and a fixed volume Particles are very close
together and vibrate
end
States of Matter- Liquid
Liquid Something with no fixed shape
but a fixed volume Particles are free to move around Also called a fluid
end
States of Matter- Gas
Gas Something with no fixed shape
and no fixed volume Particles spread apart to fill the
space available
end
States of Matter- Other
Plasma Exists at high temperatures and high pressure Stars
Bose-Einstein Condensate (BEC) Exists near absolute zero at very low pressures Solid acts as a single particle
end
Behavior of Matter
Kinetic Theory of Matter All particles of matter are in constant motion The state of matter depends on the amount of
motion Originally developed to describe gases
Kinetic Energy The energy an object has due to motion More Speed = More Kinetic Energy
end
Behavior of Matter- Gases
Particles move so fast that they are not attracted to each other
Particles move in a straight line until they hit something Act like billiard balls
end
Behavior of Matter- Gases
Kinetic Theory of Gases The motion of a gas allows it to fill a container of
any shape or size 3 main points
Particles in a gas are in constant, random motion The motion of 1 particle is not affected by the motion of
other particles, unless the particles hit each other Forces of attraction between particles are ignored
end
Behavior of Matter- Liquids
Particles move slower than gases Each particle is attracted to the others Fight between a particle’s constant motion
and the attraction to the other particles
end
Behavior of Matter- Solids
Particles are extremely attracted to each other They move very little
Vibrate back and forth in the same spot
end
Changes of State (Phase Changes) Phase Change
A reversible physical change A substance goes from 1 state of matter to another
6 common phase changes Melting and Freezing Vaporization and Condensation Sublimation and Deposition
end
Changes of State (Phase Changes)
Gas
Solid Liquid
Sublimation
Deposition
Melting
Freezing
Vaporization
Condensation
end
Changes of State- Energy
When you heat something up you give it energy And the temperature goes up
UNTIL it changes to another state! When something goes through a phase change, the
temperature stays the same. The heat you add is breaking the attraction
between particles and pushing them away from each other
end
Changes of State- Energy
Solid- Temperature is going up
Melting- Temperature is
staying the same
Liquid- Temperature is going up
Changes of State- Energy
Temperature is not changing during melting, but heat is added
Temperature is not changing during boiling, but heat is added
Changes of State- Energy
If you have to add energy, the phase change was endothermic Melting, Vaporization, Sublimation
If you have to take away energy, the phase change was exothermic Freezing, Condensation, Deposition
end
Changes of State- Melting and Freezing
Melting Some molecules in a solid,
gain energy to overcome attractive forces to become a liquid
Freezing Some molecules in a liquid,
start to slow down and become attracted to each other as a solid
end
Changes of State- Vaporization and Condensation Vaporization
Some molecules in a liquid, gain energy to overcome attractive forces to become a gas
Heat of Vaporization The amount of energy needed to move
from a liquid to a gas Evaporation
Changing a liquid to a gas at temperatures below the boiling point
Spilled water “disappears” after a few hours
end
Changes of State- Vaporization and Condensation
Condensation Some molecules in a gas, start to slow down
and become attracted to each other as a liquid The outside of your cold drink, on a hot day
end
Changes of State- Sublimation and Deposition
Sublimation Some molecules in a solid,
gain energy to overcome attractive forces to go to a gas
Dry Ice (carbon dioxide)
Deposition Some molecules in a gas, start to
slow down and become attracted to each other as a solid
Frost on cold windows
end