Matter,%20Solutions,%20and%20Gas%20Laws

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Matter, Solutions, and Gas Laws
Georgia Performance Standard SPS2. Students will
explore the nature of matter, its
classifications, and its system for naming types
of matter.
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Gas Laws

• Charles Law
• The direct proportion of the volume of a gas to
  its temperature (in Kelvin) if the pressure is at
  STP (standard temperature pressure)
• V1/T1 V2/T2

• Boyles Law
• The inverse variation of the volume of a gas with
  its pressure if the temperature and the number of
  particles are constant
• P1V1P2V2

Larger volume, less pressure
smaller volume, pressure goes up
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Matter

• Matter is anything that has mass and takes up
  space
• When matter is not the same throughout it is
  called heterogeneous
• A mixture is two or more substances that do not
  combine chemically (they keep their own
  properties)

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Properties of Matter

• Physical Property- a characteristic of a material
  that you can observe without changing its
  identity.
• Ex.- Color, shape, size, magnetic quality,
  malleability, ability to flow

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What are the physical properties of these items?
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• During a Physical Change the internal makeup of a
  substance does not change.
• Ex.- Freezing, Melting, Boiling, condensing,
  cutting into, distillation.

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Distillation

• physical change
• The process of
• separating a mixture
• by its boiling point
• Examples
• Making alcohol, separating petroleum, or salt
  water

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Petroleum Fractional Distillation
Oil was formed from the remains of animals and
plants that lived millions of years ago.  Over
the years, the remains were covered by layers of
mud.  Heat and pressure from these layers helped
the remains turn into what we today call crude
oil .  The word "petroleum" means "rock oil" or
"oil from the earth."
Other products made from petroleum include ink,
crayons, bubble gum, dishwashing liquids,
deodorant, eyeglasses, records, tires, ammonia,
and heart valves.
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Other materials made from petroleum

• Solvents Diesel Motor Oil Bearing Grease Ink
  Floor Wax Ballpoint Pens Football Cleats
  Upholstery Sweaters Boats Insecticides Bicycle
  Tires Sports Car Bodies Nail Polish Fishing lures
  Dresses Tires Golf Bags Perfumes Cassettes
  Dishwasher Tool Boxes Shoe Polish Motorcycle
  Helmet Caulking Petroleum Jelly Transparent Tape
  CD Player Faucet Washers Antiseptics Clothesline
  Curtains Food Preservatives Basketballs Soap
  Vitamin Capsules Antihistamines Purses Shoes
  Dashboards Cortisone Deodorant Footballs Putty
  Dyes Panty Hose Refrigerant Percolators Life
  Jackets Rubbing Alcohol Linings Skis TV Cabinets
  Shag Rugs Electrician's Tape Tool Racks Car
  Battery Cases Epoxy Paint Mops Slacks Insect
  Repellent Oil Filters Umbrellas Yarn Fertilizers
  Hair Coloring Roofing Toilet Seats Fishing Rods
  Lipstick Denture Adhesive Linoleum Ice Cube Trays
  Synthetic Rubber Speakers Plastic Wood Electric
  Blankets Glycerin Tennis Rackets Rubber Cement
  Fishing Boots Dice Nylon Rope Candles Trash Bags
  House Paint Water Pipes Hand Lotion Roller Skates
  Surf Boards Shampoo Wheels Paint Rollers Shower
  Curtains Guitar Strings Luggage Aspirin Safety
  Glasses Antifreeze Football Helmets Awnings
  Eyeglasses Clothes Toothbrushes Ice Chests
  Footballs Combs CD's Paint Brushes Detergents
  Vaporizers Balloons Sun Glasses Tents Heart
  Valves Crayons Parachutes Telephones Enamel
  Pillows Dishes Cameras Anesthetics Artificial
  Turf Artificial limbs Bandages Dentures Model
  Cars Folding Doors Hair Curlers Cold cream Movie
  film Soft Contact lenses Drinking Cups Fan Belts
  Car Enamel Shaving Cream Ammonia Refrigerators
  Golf Balls Toothpaste Gasoline

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Properties of Matter

• Chemical Property-- describes its "potential" to
  undergo some chemical change or reaction because
  of its composition.
• Chemical properties can only be observed by
  changing a substance's chemical properties.
  Examples Flammability, Reactivity, etc
• Once a chemical change has occurred a NEW
  SUBSTANCE OR SUBSTANCES is/are produced with
  totally new physical and chemical
  characteristics.

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Examples of Chemical Changes
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Chemical Changes

• Soft, silver metal
• Reacts violently
• with water

• Green gas
• toxic

• Love it on French
• fries
• Need it to live

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Conservation of Mass

• During a chemical reaction, energy is taken in or
  given off
• The Law of Conservation of Mass states mass is
  neither created or destroyed.
• The mass of the reactant(s) is equal to the mass
  of the product(s).

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Composition of Matter

• Main Types of Matter
• Pure Substances either elements or compounds.
• Has the same composition throughout
• A. Elements all atoms in the substance are the
  same
• 90 elements found in nature
• 20 made in laboratories
• Atom is the smallest particle of an element that
  still retains the characteristics of that element
• Examples copper, gold, hydrogen, carbon

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• Compounds consisting of two or more different
  elements bonded together (chemically combined) in
  a fixed Mass ratio that can be split into simpler
  substances.
• Examples water (H20), carbon dioxide (CO2),
  sugar (C6H1206), hydrochloric acid (H2S04),
• salt (NaCl)

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• 3. Mixtures
• 2 or more materials combined together BUT NOT
  CHEMICALLY combined, they still retain their own
  chemical makeup.
• Unlike compounds,
• mixtures do not always
• contain substances in
• fixed proportions.

Heterogeneous
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Types of Mixtures

• Heterogeneous Mixtures
• A type of mixture in which parts of the mixture
  are noticeably different from one another
• Usually can pick out the different particles
• Hetero means different
• 2 Main Types
• Suspension
• Mixture
• Examples salad, hotdog, hamburger, marble

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Suspension

• Heterogeneous mixture between liquids or
  liquids/solids that will separate out upon
  standing.
• Examples Italian dressing, pond water, oil and
  vinegar

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Types of Mixtures

• Homogeneous Mixture
• a mixture that contains 2 or more gases, liquids
  or solids blended consistently throughout.
• Hard to pick out individual particles (looks the
  same throughout)
• Homo means same
• Two Main Types
• Solutions
• Colloids (most of the time)

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Solutions

• A homogeneous mixture where one material is
  indistinguishable in another
• the dissolved particles are so small you cant
  see them
• Alloy-- a solution of two or more elements,
  usually metals.
• brass zinc and copper
• stainless steel copper, nickel and iron
• Pewter lead, copper, tin
• White gold nickel, palladium and gold
• Rose gold copper and gold
• Bronze aluminum and copper

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Colloid

• A homogenous mixture that contains some particles
  that are larger in size, but still evenly
  distributed throughout
• Does not settle upon standing unless it has gone
  bad (e.g. milk)
• Tyndall Effect dispersion of light due to larger
  particles causes milky/cloudy color in
  colloidscan be used to determine whether
  something is a solution or colloid
• Example milk, fog, peanut butter, butter,
  mayonnaise, yogurt

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Parts of a Solutions

• Solute BEING DISSOLVED the particles dissolved
  in the solution
• Examples sugar, Koolaid mix, salt
• 2. SolventDOES DISSOLVING the substance in a
  solution in which the particles dissolve
• Usually water

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Solubility

• The maximum of amount of solute that normally
  dissolves in a given amount of solvent at a
  certain temperature.
• Solubility chart shows how much of a substance
  will dissolve at a particular temperature.
• Soluble--- will dissolve in
• Salt is soluble in water.
• Sugar is soluble in water.
• Insoluble will NOT dissolve in
• An oil is insoluble in water.
• Ink is insoluble in water.

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Solutions

• Solutions are concentrated when they contain a
  lot of solute
• Solutions are dilute when they contain a small
  amount of solute
• Solubility is the ability of a substance to
  dissolve

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Rate of Solution

• Stirring- agitating the solution causes solute
  particles to come in contact with solvent
  particles
• Heating- higher temperature increase the movement
  of particles to speed dissolving
• Increasing Surface Area- More solute comes in
  contact with solvent e.g. granulated sugar versus
  sugar cubes

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Solubility

• Unsaturated- Solution contains less than the
  maximum amount of solute that can dissolve in the
  solvent at a given temperature
• Saturated- Solution that contains the maximum
  amount of solute that can dissolve at a given
  temperature
• Supersaturated- Solution that contains more
  solute that can dissolve at a given temperature
• Only stays supersaturated when condition change
  e.g. heated then cooled
• Otherwise the unusable solute will stay at the
  bottom

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Solubility Curves

• A solubility curve is a graph of a solute usually
  dissolved in 100 g of water
• Water is considered the universal solvent
• Solubility-Ability to dissolve
• Looking at the solubility curve we see that the
  type of solute will make a difference in how much
  is dissolved.
• Solubility the amt of solute that can dissolve
  in a solvent (100 mL of water)
• SOLUBILITY CURVES ARE
• ALWAYS ON THE GRAD TEST!!!

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Solubility chart various materials