Matter Chapter 3. I. Properties of Matter A. Physical B. Chemical C. Phases II. Changes of Matter A....

MatterMatter

Chapter 3Chapter 3

I. I. Properties of MatterProperties of MatterA. PhysicalA. PhysicalB. ChemicalB. ChemicalC. PhasesC. Phases

II. II. Changes of MatterChanges of MatterA. Physical A. Physical B. ChemicalB. ChemicalC. Law of ConservationC. Law of Conservation

III.III. Classifying MatterClassifying MatterA. Pure SubstanceA. Pure SubstanceB. MixturesB. Mixtures

IV.IV. Overview of the Periodic TableOverview of the Periodic TableA. MetalsA. MetalsB. Non MetalsB. Non MetalsC. MetalliodsC. MetalliodsD. Noble GasesD. Noble Gases

I.I. PropertiesPropertiesA. PhysicalA. Physical

Property that can be observed or Property that can be observed or measured without altering identity measured without altering identity of matterof matter

examples: blue, soft, 78˚C, smelly, examples: blue, soft, 78˚C, smelly, 10L10L

1.1. Intensive – does not change with Intensive – does not change with amountamount

2.2. Extensive – changes with amountExtensive – changes with amount

Examples:Examples:lengthlengthcolorcolormassmassvolumevolumedensitydensityphasephaseconductivityconductivitytexturetexture

I.I. PropertiesPropertiesA. PhysicalA. Physical

I.I. PropertiesPropertiesB. ChemicalB. Chemical

Describes ability of substance to Describes ability of substance to change into another substancechange into another substance

Examples: rust, burn, bubbles, Examples: rust, burn, bubbles, precipitateprecipitate

I.I. PropertiesPropertiesC. PhasesC. Phases

A physical propertyA physical property

1.1. Solid – Solid –

particles very close togetherparticles very close together

particles vibrate in a fixed positionparticles vibrate in a fixed position

2.2. Liquid – Liquid –

particles are intermediate in particles are intermediate in distancedistance

particles glide past each otherparticles glide past each other


3.3. Gas – Gas –

particles are far apartparticles are far apart

particles are separated from particles are separated from eachothereachother

particles move quicklyparticles move quickly


STOP

Clip 1: Physical ChangesClip 1: Physical Changes

II.II. ChangesChangesA. PhysicalA. Physical


Changes which do not result in a new Changes which do not result in a new substancesubstance

Ice Ice water water Start with HStart with H22O, end with HO, end with H22OO Examples: all phase changes, rip, cutExamples: all phase changes, rip, cut

Solid Liquid Gas

Melt Vaporize (boil or evaporate)

CondenseFreeze

Clip 2 – Chemical changes in matterClip 2 – Chemical changes in matter

II.II. ChangesChangesB. ChemicalB. Chemical

Changes that result in a new Changes that result in a new substancesubstance

a.k.a chemical reactiona.k.a chemical reaction

1.1. Word equation:Word equation:

hydrogen + oxygenhydrogen + oxygen waterwater

reactantsreactants productproduct

copper + silver nitratecopper + silver nitrate silver + copper silver + copper nitratenitrate


2.2. Formula EquationFormula Equation

Cu + 2AgNOCu + 2AgNO33 Cu(NO Cu(NO33))22 + 2Ag + 2Ag

AgNOAgNO33 + KCrO + KCrO KNO KNO33 + AgCrO + AgCrO


(be able to identify reactants and products)(be able to identify reactants and products)

3.3. Indications of chemical changes:Indications of chemical changes:– New substances formNew substances form– Color change (sometimes)Color change (sometimes)– Odor resultsOdor results– Release of Release of light and heatlight and heat– Release of gas bubbles Release of gas bubbles – Formation of a precipitate (solid that forms Formation of a precipitate (solid that forms

when two liquids are mixed)when two liquids are mixed)KI and KI and

Pb(NOPb(NO33))22


II.II. ChangesChangesC. Law of Conservation of C. Law of Conservation of MassMass

Mass is neither created nor Mass is neither created nor destroyed during a chemical or destroyed during a chemical or physical changephysical change

Mass Reactants = Mass ProductsMass Reactants = Mass Products All chemical reactions follow the Law All chemical reactions follow the Law

of Cons. of Mass….that’s why we of Cons. of Mass….that’s why we balance thembalance them

20g of lithium reacts with chlorine to 20g of lithium reacts with chlorine to form 244g of lithium chloride. How form 244g of lithium chloride. How much chlorine reacted?much chlorine reacted?

Write a word equation:Write a word equation:

lithium lithium + + chlorine chlorine lithium lithium chloridechloride

20g20g ++ xx == 244g244g

x =224gx =224g

224g of chlorine reacted224g of chlorine reacted


A 2.4g sample of X reacts with 12.8g A 2.4g sample of X reacts with 12.8g of Y to form Xof Y to form X22Y. What mass of Y. What mass of product forms? product forms?

XX ++ YY XX22Y Y

2.4g2.4g++ 12.8g =12.8g = xx

X = 15.2gX = 15.2g


III. Classification of MatterIII. Classification of Matter

Matter

Pure Substance Mixtures

Element Compound Homogeneous Heterogeneous

Combine to form

Combine to form

Composition is always the same, Composition is always the same, whatever the source…never varieswhatever the source…never varies

1.1. Element – Element – – Simplest form of matterSimplest form of matter– Made up of identical atomsMade up of identical atoms– All listed on PTOE (92 natural)All listed on PTOE (92 natural)

– Au, Na, OAu, Na, O22, S, S88 are all elements are all elements

– Cannot be broken downCannot be broken down

III.III. Classification of MatterClassification of MatterA. Pure SubstanceA. Pure Substance

2.2. CompoundsCompounds– Combination of more than one type of Combination of more than one type of

element joined by bonds (COelement joined by bonds (CO22, NaCl), NaCl)

– Components separated by chemical Components separated by chemical rxnrxn

– Represented with a chemical formulaRepresented with a chemical formula Letters indicate type of elementLetters indicate type of element Subscripts tell how manySubscripts tell how many


CaCOCaCO33

1 calcium atom3 oxygen atoms

1 carbon atom

Chemical Formulas:Chemical Formulas:

5 atoms total

1.1. Molecule – combination of more that one Molecule – combination of more that one atom held by covalent bonds (all elements atom held by covalent bonds (all elements in a molecule are nonmetals)in a molecule are nonmetals)

OO22 is a molecule of the oxygen element is a molecule of the oxygen element

OO33 is a molecule of the oxygen element is a molecule of the oxygen element

COCO22 is a molecule and a compound is a molecule and a compound

NaCl is NOT a molecule but a compoundNaCl is NOT a molecule but a compound


Clip: elements and compoundsClip: elements and compounds

– Law of Definite Composition (1779) by Law of Definite Composition (1779) by Joseph L. ProustJoseph L. Proust

– In any compound, the elements are In any compound, the elements are present in a fixed proportion by weight.present in a fixed proportion by weight.

– According to the Law of Definite According to the Law of Definite Composition (aka Definite Proportions):Composition (aka Definite Proportions):

– Water, by mass, is always 11.2% Water, by mass, is always 11.2% hydrogen and 88.8% oxygen no matter hydrogen and 88.8% oxygen no matter what the source is.what the source is.

Water = HWater = H22OO

Mass of hydrogen = 1.01 Mass of hydrogen = 1.01

Mass of oxygen = 16.00Mass of oxygen = 16.00

% hydrogen % hydrogen = = mass of hydrogenmass of hydrogen

mass of watermass of water

==(2) (1.01)(2) (1.01) x 100% x 100%

18.0218.02

= 11.2%= 11.2%

– Given CHGiven CH44 (methane), determine the (methane), determine the percent compositionpercent composition

% C = % C = 12.0112.01 x 100 x 100

16.0616.06

= 74.8%= 74.8%

III.III. Classifying MatterClassifying MatterB. MixturesB. Mixtures

Combination of two or more pure Combination of two or more pure substancessubstances

Composition of mixtures varies from Composition of mixtures varies from source to sourcesource to source

Components can be separated by Components can be separated by physical means (magnet, filter, physical means (magnet, filter, distillationdistillation))

No chemical formulaNo chemical formula List of ‘ingredients’List of ‘ingredients’

1.1. Homogenous MixturesHomogenous Mixtures– Uniform composition throughout one Uniform composition throughout one

samplesample– Also known as solutionsAlso known as solutions– Solutions can be solid, liquid or gasSolutions can be solid, liquid or gas– Aqueous solutions have water as Aqueous solutions have water as

solventsolvent


Sometimes you need additional information

2.2. Heterogenous MixtureHeterogenous Mixture– Composition varies within one sampleComposition varies within one sample


AluminumAluminum PaperPaper GoldGold Orange juiceOrange juice Fruit on the bottom yogurtFruit on the bottom yogurt Iced teaIced tea DiamondDiamond BuckminsterfullereneBuckminsterfullerene AirAir Octane (COctane (C88HH1818)) GlucoseGlucose Oil and waterOil and water Hand lotionHand lotion

IV. The Periodic Table of IV. The Periodic Table of ElementsElements 18 columns (group or family) 18 columns (group or family)

containing elements with similar containing elements with similar propertiesproperties

7 rows (periods) containing elements 7 rows (periods) containing elements with same number of electron shellswith same number of electron shells

I abbreviate it…PTOEI abbreviate it…PTOE

IV.IV. PTOEPTOEA. MetalsA. Metals

1.1. TypesTypes– Alkali earth metals (group 1)Alkali earth metals (group 1)– Alkaline earth metals (group 2)Alkaline earth metals (group 2)– Transition metals (group 3-12)Transition metals (group 3-12)– Lanthanides (bottom period 6)Lanthanides (bottom period 6)– Actinides (bottom period 7)Actinides (bottom period 7)– Others (some in groups 13-16)Others (some in groups 13-16)

2.2. PropertiesProperties– LusterLuster– Conductors of heat and electricityConductors of heat and electricity– Solids (except Hg)Solids (except Hg)– MalleableMalleable– DuctileDuctile– Tensile strengthTensile strength

IV.IV. PTOEPTOEA. MetalsA. Metals

PropertiesProperties– Vary according to metalloidVary according to metalloid– All are semi-conductorsAll are semi-conductors– B, Si, Ge, As, Sb, Te, PoB, Si, Ge, As, Sb, Te, Po

IV.IV. PTOEPTOEB. MetalloidsB. Metalloids

PropertiesProperties– Poor conductorsPoor conductors– BrittleBrittle– Solids: C, P, S, Se, I, AtSolids: C, P, S, Se, I, At– Liquid: BrLiquid: Br– Gases: N, O, F, ClGases: N, O, F, Cl

IV.IV. PTOEPTOEC. Non MetalsC. Non Metals

PropertiesProperties– All are gasesAll are gases– Stable, do not react naturallyStable, do not react naturally

IV.IV. PTOEPTOED. Noble gasesD. Noble gases

Matter Chapter 3. I. Properties of Matter A. Physical B. Chemical C. Phases II. Changes of Matter A....

Documents

Transcript of Matter Chapter 3. I. Properties of Matter A. Physical B. Chemical C. Phases II. Changes of Matter A....