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.