page 64 nov. 5, 2012 focus : chemical and physical properties / changes
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Page 64 Nov. 5, 2012 Focus : Chemical and Physical Properties / Changes Objective : pre-test, define physical and chemical property, physical and chemical change HW : article, data – analysis - graph due Warm-Up : Is Humpty Dumpty falling off the wall and cracking on the ground a - PowerPoint PPT PresentationTRANSCRIPT
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Page 64 Nov. 5, 2012
Focus: Chemical and Physical Properties / Changes
Objective: pre-test, define physical and chemical property, physical and chemical change
HW: article, data – analysis - graph dueWarm-Up:• Is Humpty Dumpty falling off the wall
and cracking on the ground a physical or chemical change? • Explain your answer.
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Pre-Assessment / Formative• Name
• November 5, 2012
• Block
• Title: Formative of Objectives 6.P.2.3, 6.P.3.1, 6.P.3.3
No more than 25 minutes
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Homework pg. 63
• Science Fair Project
• Article and questions
• Bring back card for My Energy Kit
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Physical versus Chemical Properties
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• Matter: anything that has mass and takes up space– Mass – the amount of matter in something– Volume – the amount of space something
occupies
• Which of the following is matter?– A car?– A box?– You?
Reviewing MATTER
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What is a property?
• Property: a characteristic of a substance that can be observed
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http://www.gpb.org/chemistry-physics/chemistry/201
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States, Boiling Point, Melting Point, and Solubility
Solid GasLiquid
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Defining States of Matter
• States of matter are NOT defined by what they are made of.– Example: solids can be elements (gold), compounds
(Salt = NaCl), or mixtures (butter)
Element (Au) Compound (NaCl) Mixture (Milk, Salt, etc)
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Defining States of Matter
• States of matter are defined by whether they hold SHAPE and VOLUME
Element (Au) Compound (NaCl) Mixture (Milk, Salt, etc)
ALL KEEP THE SAME SHAPE AND VOLUME = Solids
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Defining States of Matter
• Solids – have a definite SHAPE and VOLUME.
Element (Au) Compound (NaCl) Mixture (Milk, Salt, etc)
ALL KEEP THE SAME SHAPE AND VOLUME
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Particle View of a Solid
• Particles in a solid are PACKED CLOSELY together and they are in a FIXED POSITION.
Particles vibrate in place
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Liquids
• Liquids – has definite VOLUME but no defined SHAPE
100 ml
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Particle View of a Liquid
• Packed CLOSELY (like a solid), but move FREELY around each other (must stay in contact).
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Gases
• Gases - do NOT have definite SHAPE or VOLUME.
Bromine gas fills up the entire volume of the container
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Particle view of a Gas
• Particles can MOVE FREELY and will either fill up or squeeze into available space.
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Changes in States of Matter
• Thermal Energy – heat energy.
• More thermal energy = More particle movement
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Changing States
Solid GasLiquid
Increase Thermal Energy (Heat up)
Decrease Thermal Energy (Cool off)
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Melting point
• Melting - change from solid to liquid• Melting point - SPECIFIC temperature when
melting occurs. • Each pure substance has a SPECIFIC melting
point.– Examples:– M.P. of Water = 0°C (32°F) – M.P. of Nitrogen = -209.9 °C (-345.81998 °F)– M.P. of Silver = 961.93 °C (1763.474 °F) – M.P. of Carbon = 3500.0 °C (6332.0 °F)
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Melting Point
• Particles of a solid vibrate so fast that they break free from their fixed positions.
Solid Liquid
Increasing Thermal Energy
Melting point
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Vaporization
• Vaporization – change from liquid to gas
• Vaporization happens when particles in a liquid gain enough energy to form a gas.
GasLiquid
Increasing Thermal Energy
Boiling point
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Two Kinds of Vaporization
• Evaporation – vaporization that takes place only on the surface of the liquid
• Boiling – when a liquid changes to a gas BELOW its surface as well as above.
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Boiling Point
• Boiling Point – temperature at which a liquid boils
• Each pure substance has a SPECIFIC boiling point.– Examples:– B.P. of Water = 100°C (212°F) – B.P. of Nitrogen = -195.79 °C (-320.42 °F)– B.P. of Silver = 2162 °C (3924 °F) – B.P. of Carbon = 4027 °C (7281 °F)
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Boiling Point and Melting Point
Melting point
Boiling point
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Solubility
• Maximum amount of a substance that can be dissolved in a liquid (at a specific temperature).
Salt (NaCl) Water (H20) at 20°C
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Solubility
• Solute – substance being dissolved
• Solvent – liquid substance that solute is dissolved into
Salt (NaCl) Water (H20) at 20°C
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Solubility
• Solute – ??????
• Solvent – ?????
Salt (NaCl) Water (H20) at 20°C
SaltWater
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Solubility can change
• Increased Temp = Increased Solubility
• Different substances have different solubility curves
Solubility of Unknown Substance at different temperatures
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Physical Property
Physical property: a property that can be observed without changing the identity of the substance.
Examples:
• luster
• malleability: the ability to be hammered into a thin sheet
• ductility: the ability to be stretched into a wire
• melting point
• boiling point
• density
• solubility
• specific heat
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Special Physical Properties
• Melting point: the temperature at which a substance changes from a solid to a liquid at a given pressure
water = 0oC
• Boiling point: the temperature at which a substance changes from a liquid to a gas at a given pressure
water = 100oC
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Chemical Properties
• Chemical property: a property that can only be observed by changing the identity of the substance
Examples:
•flammability
•ability to rust
•reactivity with vinegar
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Chemical Properties & Physical and
Chemical Changes
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Physical changes are those changes that do not result in the
production of a new substance. If you melt a block of ice, you still
have H2O at the end of the
change.
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If you break a bottle, you still have glass. Painting your nails will not stop them from being fingernails. Some common
examples of physical changes are: melting, freezing,
condensing, breaking, crushing, cutting, and bending.
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Some, but not all physical changes can be reversed. You could
refreeze the water into ice, but you cannot put your hair back together
if you don’t like your haircut!
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Special types of physical changes where any object changes state, such as when water freezes or
evaporates, are sometimes called change of state operations.
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CHEMICAL PROPERTIES
Chemical properties can ONLY be observed AS the substances are changing into different substances.
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Chemical changes, or chemical reactions, are changes that result
in the production of another substance.
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FLAMMABILITY: A material’s ability to BURN in the presence of OXYGEN
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REACTIVITY:How readily (easily) a substance combines chemically with other
substances.
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When you burn a log in a fireplace, you are carrying out a chemical reaction that releases carbon. When you light your Bunsen burner in lab, you are
carrying out a chemical reaction that produces water and carbon
dioxide.
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Common examples of chemical changes that you may be
somewhat familiar with are; digestion, respiration,
photosynthesis, burning, and decomposition.
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Physical or Chemical Change?
•Painting Wood
•PHYSICAL
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Physical or Chemical Change?
•Burning Paper
•CHEMICAL
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Physical or Chemical Change?
•Digestion of food
•CHEMICAL
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Physical or Chemical Change?
•Sugar dissolving in water
•PHYSICAL
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Physical or Chemical Change?
•Iron turning red when heated
•PHYSICAL
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Physical or Chemical Change?
•Evaporation
•PHYSICAL
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Physical or Chemical Change?
•A pond freezing in winter
•PHYSICAL
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Physical or Chemical Change?
•Melting ice
•PHYSICAL
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Physical or Chemical Change?
•Cutting wire
•PHYSICAL
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Physical or Chemical Change?
•Painting fingernails
•PHYSICAL
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Physical or Chemical Change?
•Cutting fabric
•PHYSICAL
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Physical or Chemical Change?
•Baking muffins
•CHEMICAL
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Physical or Chemical Change?
•Shattering glass
•PHYSICAL
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Physical or Chemical Change?
•Decomposition of old leaves
•CHEMICAL
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Physical or Chemical Change?
•Wrinkling a shirt
•PHYSICAL
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Physical or Chemical Change?
•An old nail rusting
•CHEMICAL
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Density
• Density is the amount of mass per unit of volume.
• Density can be used to identify a substance.
• The density of water is 1.0g/mL
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Density Calculations
• Calculations:D = m/V = g/mL = g/cm3
• Ex: A cube has a mass of 2.8 g and occupies a volume of 3.67 ml. Would this object float or sink in water?
Mass = 2.8 g Volume = 3.67 mLD = 2.8g/3.67 mL= 0.76 g/mL
– This object would float in water because its density is less than water (1.0 g/mL).
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More Density Calculations
• Ex: A liquid has a mass of 25.6 g and a volume of 31.6 mL. Use the table below to identify the substance.
Substance Density (g/ mL)
Mercury 13.6
Water 1.00
Ethanol 0.81
M=25.6 g V=31.6 mL
D = 25.6 g/31.6 mL
D= 0.81 g/mL
The substance is ethanol.
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• Bingo
• clickr