chapter 2 matter and change sc1 students will analyze the nature of matter and its classifications...
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Chapter 2Matter and Change
SC1 Students will analyze the nature of matter and its classificationsSC1.b. Identify substances based on chemical and physical properties.SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.SC2. b. Experimentally determine indicators of a chemical reaction specifically precipitation, gas evolution, water production, and changes in energy to the system. SC6.a. Compare and contrast atomic/molecular motion in solids, liquids, gases, and plasmas.
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• Extensive property is a property that depends on the amount of matter in a sample
• Example: weight, volume
• Intensive properties depends on the type of matter in a sample not the amount of matter
• Example: phase, temperature
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Describing Matter
• Matter is anything that has mass and takes up space
• Mass of an object is the measure of the amount of matter the object contains and is affected by gravity.
• Mass of an object changes depending on location, the amount of matter does NOT change.
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4 States of Matter
• Solid is a form of matter that has DEFINITE shape and volume
• The shape of a solid doesn’t depend on the shape of a container
• The particles in a solid are packed tightly together and often in an orderly arrangement
• Solids have vibrational kinetic energy (the atoms vibrate around a fixed position)
• Solid cannot be compressed
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4 States of Matter• Liquid is a form of matter that has a DEFINIE
volume but NOT a definite shape• a liquid takes the shape of it’s container• The volume of the liquid doesn’t change as it’s
shape changes, it is constant• in a liquid the particle are free to flow past one
another and have more space between the atoms• Liquids have vibrational and rotational kinetic
energy• Liquids are slightly compressible
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4 States of Matter
• Gas is a form of matter that takes both the shape and volume of its container
• The particles in a gas are much farther apart than the particles in a liquid.
• Gases are easily compressed into smaller volumes• Gases have vibrational, rotational and
translational kinetic energy• The atoms in gases have the most space between
them
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4 States of Matter
• plasma is a state of matter similar to gas in which a certain portion of the particles are ionized
• Plasma does only exist on earth for very short periods of time [lighting bolt]
• Closes LARGE source of plasma is the sun
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4 States of Matter
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4 States of Matter Summary States of matter
Shape Volume Type of Energy
Solid Definite Definite Vibrational
Liquid Indefinite Definite Vibrational and Rotational
Gas Indefinite Indefinite Vibrational, Rotational and translational
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09/4/13 Warm-UpComplete table below.
Phase of
matter
Volume Shape Distance between particle
Compressibility Type and Amount of Energy
Solid
Liquid
Gas
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09/4/13 Warm-UpPhase
of matter
Volume Shape Distance between particle
Compressibility Amount and Type of Energy
Solid Definite DefiniteSmall
(none)NOT
compressibleLow energy
Vibrational KE only
Liquid Definite Indefinite Medium (slight)
SLIGHTLYCompressible
Medium energyVibrational and Rotational KE
Gas Indefinite Indefinite Large HIGHLYCompressible
High energyVibrational,
rotational, and translational KE
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Classifying Matter
• Mixture is a physical blend of two or more components (substances)
• Most samples of matter are mixtures• Based on the distribution of their
components, mixtures can be classified as heterogeneous mixtures or as homogeneous mixtures.
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Classifying Matter
• Heterogeneous mixture is a mixture in which the composition is NOT uniform throughout.– Examples: salad, pizza, beach sand
• Homogeneous mixture is a mixture in which the composition IS uniform throughout.– Example: vinegar, soda, tap water– Solution is a homogenous mixture where solutes are
dissolved in a solvent (kool-aid)– most solutions are liquids but some can be solid (steel,
bronze) and some are gases (air)– all homogeneous mixtures consist of a single phase
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Classifying Matter• Pure Substance is a sample of matter, either an
element or a compound, that consists of only one component with definite physical and chemical properties and a definite composition.– Element is the simplest form of matter that has a unique
set of properties– Element cannot be broken down into simpler substances
• Examples: oxygen, nitrogen, sodium
– Compound is a substance that contains two or more elements chemically combined in a fixed proportion.
– Compounds can be chemically separated in to simpler substances• Examples: water, sugar, oil
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Classifying Matter
• You can use their general characteristics to distinguish substances from mixtures
• If the composition of a material is fixed, the material is a pure substance. If the composition of a material may vary, the material is a mixture.
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End 9/6/12
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Physical/Chemical Properties
• Properties of matter can be classified in two ways.• Physical property is a quality or condition of a
substance that can be observed or measured without changing the substance’s composition. – Physical properties include hardness, color,
conductivity, malleability, melting point and boiling point.
• Physical properties can help chemists identify substances
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Physical/Chemical Properties• Chemical property is a quality or condition of a
substance that can be observed or measured only by changing the substance’s composition. – Flammability, reactivity, non-reactive, combustibility
• Chemical properties can help chemists identify substances
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Physical/Chemical Properties Practice1. Blue Liquid2. Gold is unreactive3. Lemon are sour4. Ice is cold5. Baseballs are round6. Mrs. Raines is 6th tall7. Gas will explode8. Neon is inert
1. Physical2. Chemical3. Chemical4. Physical5. Physical6. Physical7. Chemical8. chemical
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Separation Techniques • differences in physical properties can be used to separate mixtures1. Manual separation is the process of picking out pieces of a mixture.
Example: picking mushrooms off pizza2. Evaporation is the process of separating a dissolved solid from a liquid.
Involved heating up the liquid and leaving the solid behind.Example: getting drinking water from salt water.
3. Filtration is the process of separating a solid from a liquid in a heterogeneous mixture example: using a colander to separate noodles from water, coffee
filter and coffee grinds 4. Distillation is the process of separating two or more liquids due to a
difference in boiling pointsexample: used to make moonshine separates alcohol from slag.
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Separation Techniques• How would you separate1. Beans from broth2. Salt from water3. Sand from water4. Pickles from hamburger5. Sugar from water6. Pebbles from sand7. Alcohol and water8. Tea leaves from tea
1. Filtration (colander)2. Evaporation3. Filtration (filter)4. Manual5. Evaporation6. Manual7. Distillation8. Filtration (filter)
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Physical Changes• Physical change a change during which some
properties of a material change, but the composition of the material does not change– Boil, melt, freeze, condense, breaking, splitting , grind,
and cut are used to describe physical changes.• Physical changes can be classified as reversible or
irreversible.– Phase changes (Melting, freezing and boiling) are
examples of reversible physical changes (can be changed back)
– Cutting, grinding, and breaking are example of irreversible physical changes (cannot be changed back)
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Types of Physical Changes• Melting is the phase change as a substance changes from a solid
to a liquid. • Freezing is the phase change as a substance changes from a liquid
to a solid. • Vaporization is the phase change as a substance changes from a
liquid to a gas. • Condensation is the phase change as a substance changes from a
gas to a liquid. • Sublimation is the phase change as a substance changes from a
solid to a gas without passing through the intermediate state of a liquid.
• Deposition is the phase change as a substance changes from a gas to a solid without passing through the intermediate state of a liquid.
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Energy of Phase Changes• heat of fusion the energy needed to melt or
freeze a substance• heat of vaporization the energy needed to
vaporize or condense a substance
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Chemical Changes• Chemical change is a change that produces matter
with a different composition than the original matter– Heating a substance can be used to break down
compound into simpler substances.– Reacting substances to form new substances
• Examples: heating sugar with give you carbon and water. An acid and a base make a salt and water
• Possible clues to chemical changes include a transfer of energy, a change in color, the production of a gas, or the formation of a precipitate– Precipitate is a solid that forms and settles out of a liquid
mixture• Every chemical change involves a transfer of energy
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Physical/Chemical Changes
• Summary–Physical changes the composition of
substance stays the same. The phase or shape may change
–Chemical changes involve a change in the CHEMICAL composition of a substance
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Identify as Physical/Chemical Change1. Silver tarnishing2. Crushing slate3. Dry ice sublimating4. Milk spoiling5. Fermenting grape juice6. Evaporating water7. Cooking bread8. Steal turns red when heated9. Grinding coffee10. Potatoes rotting
1. Chemical2. Physical3. Physical4. Chemical5. Chemical6. Physical7. Chemical8. Physical9. Physical10. Chemical
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Phase Change Diagrams• Most common type of phase change diagram
show the temperature of a substances versus the amount of energy added to a substance
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Phase Change Diagrams• At the low temperatures all substances are a solid
Solid
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• As heat is added the object begins to melt and both solid and liquid phases are present
Solid
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• As heat is added the object begins to melt and both solid and liquid phases are present
Solid
Solid & Liquid
Notice that during the phase change the temperature does NOT changeAt green dot the Heat of fusion is reached The object is MELTING
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• As heat is added the object finishes melting and is in the LIQUID phase
Solid
Solid & Liquid
Notice that the temperature starts to rise again.
Liquid
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• As heat is added the object begins to form a vapor and both liquid and gas phases are present
Solid
Solid & Liquid
Notice that during the phase change the temperature does NOT changeAt blue dot the Heat of Vaporization is reached The object is Vaporizing
Liquid
Liquid and Gas
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• As heat is added the object finishes vaporizing and is in the gas phase
Solid
Solid & Liquid
Notice that the temperature increases again
Liquid
Liquid and Gas
Gas ONLY
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• What is heat is removed from the GAS?
Solid
Solid & Liquid
The gas cools and forms a liquid called CONDENSATIONBoth liquid and gas are present until ALL gas becomes a liquidCircled point
Liquid
Liquid and Gas
Gas ONLY
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• What is heat is removed from the GAS?
Solid
Solid & Liquid
The liquid cools until it starts to reform the solid.
Liquid
Liquid and Gas
Gas ONLY
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• What is heat is removed from the GAS?
Solid
Solid & Liquid
The liquid cools and both solid and liquid phases are presentAt this stage the substance is FREEZINGCircled point
Liquid
Liquid and Gas
Gas ONLY
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Phase Change Diagram Combined
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Phase Change Diagram Practice• What is occurring at the following pointsAB• What phase is present at the following pointsABCDE
Object is vaporizing or condensingObject is melting or freezing
A. Liquid & GasB. Solid & LiquidC. Liquid ONLYD. Solid ONLYE. Gas ONLY
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Triple Point Diagram
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