what is matter? anything that takes up space (volume) and has mass. anything on earth
TRANSCRIPT
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What is Matter? Anything that
takes up space (volume) and has mass.
Anything on EARTH.
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Types of Matter Homogeneous
Matter that is made up of the same or alike particles.
SAME THROUGHOUT Can’t see the particle
HeterogeneousMatter that is
made up of different types of particles.
DIFFERENT THROUGHOUT
Can see the particles
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Homogeneous Materials
Kool aidTeaClear sodasRubbing alcoholWaterElementsCompoundsAcids
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Heterogeneous Materials
CerealSaladSnack mixKabobsItalian dressingsUncooked pizzaM & M’sSkittlesVegetable soupMilk
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Now it is your turn… you tell me:
Homogeneous or Heterogeneous Flat soda pop
Cherry vanilla ice cream Sugar (C2H3O2)
Salt (NaCl) City Air Iron (Fe) Beach Sand Spaghetti Sauce
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Mixtures vs. Pure Substances MIXTURES
Heterogeneous or Homogeneous
Easily separated
EXAMPLES
Any Heterogeneous or homogeneous examples
PURE SUBSTANCESHomogeneousHard to separateIn it simplest form
EXAMPLES
Elements and compounds
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Types of Pure
Substances Elements: Purest
substance known that can’t be broken downNeon: Ne
Compounds: 2 or more elements chemically combinedWater: H2O
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Atoms are the counting units or quantity of the
element.
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Properties of Mixtures
Easily separated Physically combined to
easily separate. Amounts vary when
mixed Changes only in
physical appearance when dissolved.
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Types of Mixtures
Heterogeneous Mixtures
SuspensionsColloids
Homogeneous Mixtures
Solutions
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Solution
Homogeneous Mixture: Same throughout
Examples: Ice teaSugar waterKool aidSprite
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Solutions and Its Properties Particles are individual atoms,
molecules, or ions (charged particles)
Clear Can’t be filtered Particles are evenly spread out Can’t see the particles Homogeneous
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Parts of a Solution Solute – Part being
dissolved in the solvent.ex: Sugar, Hot Chocolate, Salt
Solvent – Part that does the dissolving.ex: Water – universal solvent
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Aqueous vs. Tincture Solution Aqueous – water
is the solvent
Tincture – alcohol is the solvent
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Combinations of Solutions
SOLUTES
1. Solid
2. Solid
3. Solid
SOLVENT
Solid
Liquid
Gas
EXAMPLES
Alloy (pots)
Sea water
Soot in air
4. Liquid
5. Liquid
6. Liquid
Solid
Liquid
gas
Dental fillings
Antifreeze
Humid air
7. Gas
8. Gas
9. Gas
Solid
Liquid
Gas
Gas mask
Sodas
Air
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Special Activities of Solutions
Dissociation – splitting ions to form charges
Ionization – gaining or losing electrons to form ions
Electrolyte – Solution that produce electricity(Salt and Water)
Non-electrolyte – solution that does not produce electricity (Sugar and Water)
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Special Solutions Miscible – when a liquid is dissolved
into a liquid Example: Antifreeze, alcohol and water
Alloy – when a solid is dissolved into a solidExamples: Stainless steel pots and
pans, bronze, brass, jewelry
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Rates of Solutions (how to speed up a solution)
Stirring Heating Powdering-
increasing the surface area
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Solubility and Its Factors Solubility – ability of a solute to
dissolve into a solvent. Factors that affect solubility of a gas in a
solution Temperature – decreasing temperaturePressure – increasing pressure
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Dilute vs. Concentrated
Dilute – weak solution
“watered down”
ConcentratedStrong solution
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Levels of Solutions
Saturated – Holding as much solute at a given temperature
Supersaturated – UNSTABLE – more solute in the solvent at a high temp.
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Colloid Properties
Heterogeneous Mixture
Can’t see particles Particle size is larger
than those in solutions
Scatters light – Tyndall Effect
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Examples of Colloids Fog- clouds Smoke- smoke Foam- whipped
cream Emulsion-
mayonnaise Sol- paints Gel- butter
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Suspension Properties
Heterogeneous Mixture
Can see the particles Easily separated EXAMPLES
waste
oil and water
trail mix
eggs
cereals
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Ways to Separate Mixtures Filtering – Suspensions
Evaporation – Solution, Colloids, Suspensions
Distillation – Solutions, Colloids, Suspensions
Chromatography - Solutions
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Physical Properties and Changes Physical Properties
Characteristic you can observe without changing the substance
Examples:○ Appearance: color, shape, …○ Measurements: mass, length,
volume…○ Behavior: attracted by magnet,
soluble…○ Changes of State: melting point,
boiling point…
Physical Changes Change made to material
that does not change the substances
Usually, the change can be reversed Examples:
○ Tearing, shredding crushing…○ Boiling, melting, freezing…○ Dissolving
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Chemical Properties
Characteristic of a substance that undergoes a certain chemical changeExamples:
○ Flammability or combustibility○ Reactivity
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Chemical Change Change of one substance in a
material to a different substance Usually the change can’t be
reversed Signs of a chemical change:
SmellColorFoaming or gas productionPrecipitate – solid forming when two items
are mixed togetherLight or explosion (release of energy)
Examples: rusting, burning, …
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Law of Conservation of Mass Matter is neither created nor destroyed
during a chemical change or physical change
original mass = final mass