CH. 3CH. 3Matter- Properties Matter- Properties
and Changesand Changes
MondayMonday
Physical and Chemical ChangePhysical and Chemical Change WorksheetWorksheet
3.2 Changes in Matter3.2 Changes in MatterTEKSTEKS
(8) Science concepts. The student can (8) Science concepts. The student can quantify the changes that occur during quantify the changes that occur during chemical reactions. The student is chemical reactions. The student is expected to:expected to:
E. Determine mass relationships between E. Determine mass relationships between reactants and products reactants and products
3.1 Properties of Matter3.1 Properties of Matter Substance -Substance - composition is uniform, composition is uniform,
does not change between samples does not change between samples and is “pure”.and is “pure”.
Pure substances:Pure substances:1. Elements – Na, H, He1. Elements – Na, H, He
2. Compounds – NaCl (salt) 2. Compounds – NaCl (salt)
HH22O (water)O (water)
3.2 Changes in Matter3.2 Changes in Matter
Physical Change-Physical Change- changes which alter changes which alter a substance without changing the a substance without changing the composition.composition.
(Does not change the identity of the (Does not change the identity of the substance)substance) Ex: ice to waterEx: ice to water
Examples of Physical ChangesExamples of Physical Changes
Change in Size or ShapeChange in Size or Shape such as: such as:
Bend, break, cut, grind, crumple, split, or crushBend, break, cut, grind, crumple, split, or crush Change in StateChange in State such as: such as:
Melting, freezing, vaporization, boiling, Melting, freezing, vaporization, boiling, condensation, or sublimationcondensation, or sublimation
Chemical Change-Chemical Change- involves one or involves one or more substances changing into more substances changing into another substanceanother substance
(also called a Chemical Reaction)(also called a Chemical Reaction)
Ex: steel to rustEx: steel to rust
Chemical ReactionsChemical ReactionsThe The newnew substances formed in the substances formed in the
reaction have different reaction have different compositions and different compositions and different properties from the substances properties from the substances present before the reaction present before the reaction occurred.occurred.
Reactant – starting material in a Reactant – starting material in a reactionreaction
Product – ending material in a Product – ending material in a reactionreaction
Reactant(s) Reactant(s) turn into Product(s) turn into Product(s)Na + Cl = NaCl (Salt)Na + Cl = NaCl (Salt)
Examples of Chemical ChangesExamples of Chemical Changes
Fermentation, Fermentation, rusting, rusting, explode, explode, oxidize, oxidize, corrode, corrode, tarnish, tarnish, burn, burn, or rot.or rot.
C. Conservation of Mass – C. Conservation of Mass – By carefully By carefully
measuring the mass before and after measuring the mass before and after
many chemical reactions, it was observed many chemical reactions, it was observed
that the total mass involved in the reaction that the total mass involved in the reaction
stayed the same. stayed the same.
Law of Conservation of Mass-Law of Conservation of Mass- states that states that matter is neither created nor destroyed matter is neither created nor destroyed during a reaction– it is conservedduring a reaction– it is conserved
Total mass of the reactants must equal the Total mass of the reactants must equal the total mass of the products.total mass of the products.MassMassreactants = reactants = MassMassproductsproducts
4. According to the law of conservation of mass, how much zinc was present in the zinc carbonate?
A 40 g B 88 gC 104 D 256 g
Antoine Lavoisier used an analytical Antoine Lavoisier used an analytical balance to help prove this law.balance to help prove this law.
Conservation of Mass problemsConservation of Mass problems
Ex: Ex: 23 g of Na reacts with 35 g of 23 g of Na reacts with 35 g of Cl, what is the mass of the product, Cl, what is the mass of the product, sodium chloride?sodium chloride?
23 g Na+ 35 g Cl = ______ g NaCl23 g Na+ 35 g Cl = ______ g NaCl
Ex: #2Ex: #2 10 g HgO = 9.26 g Hg + _____ g of O10 g HgO = 9.26 g Hg + _____ g of O
TuesdayTuesday
Lab on Physical and Chemical ChangeLab on Physical and Chemical Change
WednesdayWednesday
Screaming gummi bears demoScreaming gummi bears demo Answer follow-up questionsAnswer follow-up questions Physical and Chemical properties matterPhysical and Chemical properties matter
TEKSTEKS
(4) Science concepts. The student knows the (4) Science concepts. The student knows the characteristics of matter and can analyze the characteristics of matter and can analyze the relationships between chemical and physical relationships between chemical and physical changes and properties. changes and properties.
The student is expected to: The student is expected to: (A) differentiate between physical and chemical (A) differentiate between physical and chemical
changes and properties; changes and properties; (B) identify extensive and intensive properties; (B) identify extensive and intensive properties;
Chemical Property-Chemical Property- the ability of a the ability of a substance to combine with or substance to combine with or change into one or more change into one or more substancessubstances
Na + Cl = NaCl (Salt)Na + Cl = NaCl (Salt)
Examples of Chemical Examples of Chemical PropertiesProperties
Ability to rustAbility to rust Formation of precipitateFormation of precipitate Reacts with water, oxygen, Reacts with water, oxygen,
acids, bases, or other acids, bases, or other substancessubstances
FlammabilityFlammability
Physical Properties of MatterPhysical Properties of Matter
Physical property-Physical property- characteristic that can be characteristic that can be observed or measured observed or measured without changing the without changing the sample’s compositionsample’s composition
Qualitative!!Qualitative!!
Examples of Physical PropertiesExamples of Physical Properties
DensityDensity ColorColor OdorOdor TasteTaste HardnessHardness Melting PointMelting Point Boiling PointBoiling Point
Extensive PropertiesExtensive PropertiesDependent upon amount of Dependent upon amount of
substance presentsubstance presentMass, Length, VolumeMass, Length, VolumeIt It changeschanges if you take away if you take away
some of the substance.some of the substance.
Intensive propertiesIntensive properties Independent of amount of Independent of amount of
substance presentsubstance present Examples: Density, color, Examples: Density, color,
odor, boiling point.odor, boiling point. Intensive properties Don’t Intensive properties Don’t
changechange and can be used to and can be used to identifyidentify the substance. the substance.
Miners often got Pyrite (fool’s gold) Miners often got Pyrite (fool’s gold) and real gold mixed up. But Density and real gold mixed up. But Density could be used to correct the error.could be used to correct the error.
The density of gold is 19.3 g/mL The density of gold is 19.3 g/mL and the density of pyrite is 5 g/mLand the density of pyrite is 5 g/mL
Pyrite – fools gold Gold
Properties of CopperProperties of CopperPhysical PropertiesPhysical Properties Chemical PropertiesChemical Properties
Reddish brown, shinyReddish brown, shiny Forms green copper carbonate Forms green copper carbonate compoundcompound
Malleable, ductileMalleable, ductile Forms new substances with nitric Forms new substances with nitric acid and sulfuric acid.acid and sulfuric acid.
Good conductorGood conductor Forms a deep blue solution with Forms a deep blue solution with ammonia.ammonia.
Density = 8.92 g/mLDensity = 8.92 g/mL
Melting pt = 1085 Melting pt = 1085 ooCC
Boiling pt = 2570 Boiling pt = 2570 ooCC
So changing States of Matter So changing States of Matter are PHYSICAL properties!!are PHYSICAL properties!!
Both are copperBoth are copper
Properties of MatterProperties of Matter
Chemical PropertiesChemical Properties
Reactions in the presence of
Water, Air, Acid, Base
What happens when heated
Reactions in the presence of
Water, Air, Acid, Base
What happens when heated
Physical PropertiesPhysical
Properties
Intensive Properties
Do NOT depend on the amount
________________
E.G Color, Taste, Melting/Boiling Point, Luster, Hardness
Intensive Properties
Do NOT depend on the amount
________________
E.G Color, Taste, Melting/Boiling Point, Luster, Hardness
Extensive Properties
Depends on the amount
_______________
Mass, Volume, Length, Shape
Extensive Properties
Depends on the amount
_______________
Mass, Volume, Length, Shape
http://www.roomd113.com/TAKS%20PP/matterclass_pres.ppt
Evidence of a Chemical ReactionEvidence of a Chemical Reaction
The observation that the product has different The observation that the product has different properties than the reactant(s).properties than the reactant(s).
Clues:Clues:• If something can burnIf something can burn• Production of energy, such as light, heat, or Production of energy, such as light, heat, or
soundsound• Formation of a gas Formation of a gas • Formation of a solid – called a precipitate Formation of a solid – called a precipitate • Change in odorChange in odor• Change in colorChange in color
MATTER
Can it be physically separated?
Homogeneous Mixture
Heterogeneous Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be chemically decomposed?
noyesIs the composition uniform?
noyes
Colloids
SuspensionsSolutions
ThursdayThursday
Chromatography labChromatography lab Methods of separationMethods of separation
3.3 Mixtures of Matter3.3 Mixtures of Matter
TEKSTEKS 2.(E) plan and implement investigative 2.(E) plan and implement investigative
procedures, including asking questions, procedures, including asking questions, formulating testable hypotheses, and formulating testable hypotheses, and selecting equipment and technology selecting equipment and technology
4. (D) Classify matter as pure substances 4. (D) Classify matter as pure substances or mixtures through investigation of their or mixtures through investigation of their properties. properties.
3.3 Mixtures of Matter3.3 Mixtures of Matter
Mixture-Mixture- combination of two or combination of two or more pure substances in more pure substances in which each retains its which each retains its individual chemical properties.individual chemical properties.
Examples of MixturesExamples of Mixtures
Sand and waterSand and water
Salt and WaterSalt and Water
If the substances do not react and If the substances do not react and can be separated by physical can be separated by physical means, it is a mixture.means, it is a mixture.
Types of MixturesTypes of Mixtures
Heterogeneous Mixture-Heterogeneous Mixture- does not does not blend smoothly and individual blend smoothly and individual substances remain distinct. (can substances remain distinct. (can see the different parts)see the different parts)
Ex: salad, pizzaEx: salad, pizza
Homogeneous Mixture-Homogeneous Mixture- constant composition constant composition throughout (looks the same throughout (looks the same throughout)throughout)Also known as Also known as solutionssolutionsEx: Koolaid, air, sea water, Ex: Koolaid, air, sea water,
sodas, vinegar, steelsodas, vinegar, steel
Types of Solution SystemsTypes of Solution Systems
SYSTEMSYSTEM EXAMPLEEXAMPLE
Gas-GasGas-Gas Air is primarily an example of nitrogen, oxygen and Air is primarily an example of nitrogen, oxygen and argon gases.argon gases.
Gas- LiquidGas- Liquid Carbonated beverages contain carbon dioxide gas in Carbonated beverages contain carbon dioxide gas in solution.solution.
Liquid- GasLiquid- Gas Moist air contains water droplets in air.Moist air contains water droplets in air.
Liquid- LiquidLiquid- Liquid Vinegar contains acetic acid in water.Vinegar contains acetic acid in water.
Solid- LiquidSolid- Liquid Sweetened powder drink contains sugar and other Sweetened powder drink contains sugar and other solid ingredients in water.solid ingredients in water.
Solid- SolidSolid- Solid Steel is an Steel is an alloy alloy of iron containing carbon.of iron containing carbon.
ColloidColloid
A heterogeneous mixture with particles A heterogeneous mixture with particles larger than those in a solutionlarger than those in a solution
Example : milkExample : milk
SuspensionSuspension
A heterogeneous mixture whose particles A heterogeneous mixture whose particles settle out over time and can be separated settle out over time and can be separated from the mixture by filtrationfrom the mixture by filtration
Example lead paintExample lead paint
Separating MixturesSeparating MixturesBecause mixtures are physically Because mixtures are physically
combined, combined,
the processes are the processes are
used to separate them areused to separate them are
based on the difference in physical based on the difference in physical properties of the substances.properties of the substances.
4 methods for separation4 methods for separation
FiltrationFiltration
Uses a Uses a porous porous barrier to barrier to separate a separate a solid from solid from a liquida liquid
DistillationDistillation Based on differences Based on differences
in boiling points of the in boiling points of the substancessubstances
Heat mixture until Heat mixture until substance with lowest substance with lowest boiling point boils to a boiling point boils to a vapor which is then vapor which is then condensed into a condensed into a liquidliquid
CrystallizationCrystallizationResults in formation Results in formation
of pure solid of pure solid particles of a particles of a substance from a substance from a solution containing solution containing the dissolved the dissolved substancesubstance
ChromatographyChromatography Separates the components Separates the components
of a mixture (called the of a mixture (called the mobile phase) on the basis mobile phase) on the basis of the tendency of each to of the tendency of each to travel or be drawn across travel or be drawn across the surface of another the surface of another material (called the material (called the stationary phase)stationary phase)
FridayFriday
10-bottle lab and finish notes on 10-bottle lab and finish notes on methods of separationmethods of separation
States of matterStates of matter
3.4 Elements and Compounds3.4 Elements and Compounds
TEKSTEKS 4. (D) Classify matter as pure substances 4. (D) Classify matter as pure substances
or mixtures through investigation of their or mixtures through investigation of their properties. properties.
3.4 Elements and Compounds3.4 Elements and CompoundsElement-Element- Pure substance that Pure substance that
can not be separated into can not be separated into simpler substances by simpler substances by physical or chemical meansphysical or chemical means
Examples: Copper, Oxygen, Examples: Copper, Oxygen, IodineIodine
Each element has a unique Each element has a unique chemical name and symbol.chemical name and symbol.
The first letter is always The first letter is always capitalized, the rest are capitalized, the rest are lowercase.lowercase.Ex: Ex:
• OxygenOxygen OO• Carbon Carbon CC• IronIron FeFe
Periodic TablePeriodic Table
In 1869 Dmitri Mendeleev devised In 1869 Dmitri Mendeleev devised a chart which organized all of the a chart which organized all of the known elements into rows and known elements into rows and columns based on their columns based on their similarities and masses.similarities and masses.
Rows are called periodsRows are called periodsColumns are called groups or familiesColumns are called groups or families
Can be broken down into Can be broken down into simpler substances by chemical simpler substances by chemical means (ex: using heat or means (ex: using heat or energy)energy)
CompoundsCompoundsCompound-Compound- a pure substance a pure substance
that is a combination of two or that is a combination of two or more elements that are more elements that are combined chemically.combined chemically.
Common CompoundsCommon Compounds There are 10 MILLION known compounds!There are 10 MILLION known compounds! Ex: Water, Sodium chloride (salt), sucrose Ex: Water, Sodium chloride (salt), sucrose
(sugar), aspirin, etc.(sugar), aspirin, etc. Chemical compounds are represented by Chemical compounds are represented by
formulas.formulas.
Ex: Ex: Water is HWater is H22OO
Sodium chloride is NaClSodium chloride is NaCl
Sucrose is CSucrose is C1212HH2222OO1111
Properties of a compound are Properties of a compound are different than the elements that different than the elements that make it up.make it up.
MondayMonday
States of MatterStates of Matter http://www.youtube.com/watch?v=V9WYw
eBA6vA&feature=related OobleckOobleck http://www.youtube.com/watch?http://www.youtube.com/watch?
v=V9WYweBA6vA&feature=relatedv=V9WYweBA6vA&feature=related
Ex: Hydrogen and Oxygen are Ex: Hydrogen and Oxygen are tasteless, odorless gases. They make tasteless, odorless gases. They make water which is a clear liquidwater which is a clear liquid
Hydrogen + Oxygen Water
Ex: Chlorine is a poisonous green gas. Ex: Chlorine is a poisonous green gas. Sodium is an explosive metal. They Sodium is an explosive metal. They make sodium chloride which is a white make sodium chloride which is a white crystal that tastes salty.crystal that tastes salty.
Stop pg 74Stop pg 74
States of matter-States of matter- physical forms physical forms of all matter on Earth.of all matter on Earth.
States of MatterStates of Matter SolidSolid- definite shape and volume. - definite shape and volume. Particles vibrate in place.Particles vibrate in place. Particles are tightly packed.Particles are tightly packed. This make a solid This make a solid incompressibleincompressible – can’t – can’t
be pressed into a smaller volume.be pressed into a smaller volume.
LiquidLiquid- form of matter that flows, - form of matter that flows, has constant volume, and takes has constant volume, and takes the shape of its container. the shape of its container.
LiquidsLiquids
Particles can Particles can move past move past each othereach other
Particles are Particles are close together.close together.
virtually virtually incompressibleincompressible
GasGas- form of matter that flows to - form of matter that flows to conform to the shape of its container conform to the shape of its container and fills the entire volume of its and fills the entire volume of its container.container.
GasesGases Particles of gases move freely.Particles of gases move freely. Particles are very far apart. Particles are very far apart. Easily compressed.Easily compressed. Is normally in the gaseous state at Is normally in the gaseous state at
room temperature.room temperature.
Movement of particlesMovement of particles
Microscopic view of a gas.
Microscopic view of a liquid.
Microscopic view of a solid.
Characteristics of Gases, Liquids and Solids and the Characteristics of Gases, Liquids and Solids and the Microscopic Explanation for their BehaviorMicroscopic Explanation for their Behavior
GasGas LiquidLiquid SolidSolidflows easily flows easily particles can move past particles can move past one another one another
flows easily flows easily particles can particles can move/slide past one move/slide past one another another
does not flow easily does not flow easily rigid - locked into place rigid - locked into place
particles cannot move/slide particles cannot move/slide past one anotherpast one another
compressible compressible lots of free space lots of free space between particles between particles
not easily compressible not easily compressible
little free space little free space between particles between particles
not easily compressible not easily compressible little free space between little free space between particles particles
assumes the shape and assumes the shape and volume of its container volume of its container
assumes the shape of assumes the shape of its container, but its container, but volume is constantvolume is constant
retains a fixed volume retains a fixed volume
and shape and shape
VaporVapor – refers – refers to the gaseous to the gaseous state of a state of a substance that substance that is usually a is usually a solid or liquid solid or liquid at room at room temperature.temperature.
PlasmaPlasma Plasma Plasma - the fourth- the fourth
state of matter and the state of matter and the
most common one.most common one.
Found in Stars, and occurs Found in Stars, and occurs
naturally on the Earth in naturally on the Earth in
lightning bolts.lightning bolts.