classification of matter this well-known molecule is a compound because it contains more than one...

MATTER

Can it be physically separated?

Homogeneous Mixture

(solution)

Heterogeneous Mixture Compound Element

MIXTURE PURE SUBSTANCE

yes no

Can it be chemically decomposed?

noyesIs the composition uniform?

noyes

Colloids Suspensions

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Elements

only one kindof atom; atomsare bonded itthe element

is diatomic orpolyatomic

Compounds

two ormore kindsof atoms

that are chemicallybonded

substancewith

definitemakeup

andproperties

Mixtures

two or moresubstances

that arephysically

mixed

two ormore

kinds ofand

Both elements and compounds have a definite makeup and definite properties.

Packard, Jacobs, Marshall, Chemistry Pearson AGS Globe, page (Figure 2.4.1)

Matter Flowchart

Examples:

– graphite

– pepper

– sugar (sucrose)

– paint

– soda

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element

hetero. mixture

compound

solution homo. mixture

hetero. mixture

Pure Substances

Element– composed of identical atoms– EX: copper wire, aluminum foil

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Pure Substances

Compound

– composed of 2 or more elements in a fixed ratio

– properties differ from those of individual elements

– EX: table salt (NaCl)

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Pure Substances

Law of Definite CompositionLaw of Definite Composition

– A given compound always contains the same, fixed ratio of elements.

Law of Multiple ProportionsLaw of Multiple Proportions

– Elements can combine in different ratios to form different compounds.

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Pure Substances

For example…

Two different compounds, each has a definite composition.

Carbon, C Oxygen, O Carbon monoxide, CO

Carbon, C Oxygen, O Oxygen, O Carbon dioxide, CO2

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Mixtures

Variable combination of two or more pure substances.

Heterogeneous Homogeneous

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Mixtures

Solution– homogeneous– very small particles– no Tyndall effect Tyndall Effect

– particles don’t settle– EX: rubbing alcohol

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Mixtures

Colloid– heterogeneous– medium-sized particles– Tyndall effect– particles don’t settle– EX: milk

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Mixtures

Suspension– heterogeneous– large particles– Tyndall effect– particles settle– EX: fresh-squeezed

lemonade

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Mixtures

Examples:

– mayonnaise

– muddy water

– fog

– saltwater

– Italian salad dressing

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colloid

suspension

colloid

solution

suspension

Classification of Matter

Materials

HomogeneousHeterogeneous

Heterogeneousmixture

Homogeneousmixture

Substance

Element Compound Solution Mixture

Speci

fic /

Gen

eral

Order / Disorder

Smoot, Smith, Price, Chemistry A Modern Course, 1990, page 43

Classification of Matter

MATTER(gas. Liquid,

solid, plasma)

PURESUBSTANCES MIXTURES

HETEROGENEOUSMIXTURE

HOMOGENEOUSMIXTURESELEMENTSCOMPOUNDS

Separated by

physical means into

Separated by

chemical means into

Kotz & Treichel, Chemistry & Chemical Reactivity, 3rd Edition , 1996, page 31

Classification of Matter

uniformproperties?

fixedcomposition?

chemicallydecomposable?

no

no

no

yes

hetero-geneousmixture

solution

element

compound

http://antoine.frostburg.edu/chem/senese/101/matter/slides/sld003.htm

Elements, Compounds, and Mixtures

(a)an element(hydrogen)

(b)a compound(water)

(c)a mixture(hydrogen and oxygen)

(d)a mixture(hydrogenand oxygen)

Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 68

hydrogenatoms hydrogen

atoms

oxygen atoms

Elements, Compounds, and Mixtures

(a)an element(hydrogen)

(b)a compound(water)

(c)a mixture(hydrogen and oxygen)

(d)a mixture(hydrogenand oxygen)

Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 68

hydrogenatoms hydrogen

atoms

oxygen atoms

Mixture vs. Compound

Mixture

FixedComposition

Bonds between

components

Can ONLY beseparated by

chemical means

VariableComposition

No bondsbetween

components

Can beseparated by

physical means

Alike Different

Contain two or more

elements

Can beseparated

intoelements

Involvesubstances

Compound

Different

Topic Topic

Compounds vs. Mixtures

• Compounds have properties that are uniquely different from the elements from which they are made. – A formula can always be written for a compound

– e.g. NaCl Na + Cl2

• Mixtures retain their individual properties.– e.g. Salt water is salty and wet

Diatomic Elements, 1 and 7H2

N2 O2 F2

Cl2

Br2

F2

Products made from Sulfur

Magazines and printing papersWriting and fine papersWrapping and bag papersSanitary and tissue papersAbsorbent papers

RayonCellophaneCarbon TetrachlorideRuber processing chemicals

Containers and boxesNewsprintPulp for rayon and film

PULP 3%

OTHER 3%

NONACID 12%

InsecticidesFungicidesRubber vulcanizingSoil sulfur

Specialty steels Magnessium Leather processing PhotographyDyestuffs

Bleaching Soybean extraction

Aluminum reductionPaper sizingWater treatmentPharmaceuticalsInsecticidesAntifreeze

Superphosphates Ammonium phosphate Ammonium sulfate Mixed fertilizers

AutosAppliancesTin and other containersGalvanized products

Explosives Nonferrous metals Synthetic rubber Storage batteries Textile finishing

Tire cords Viscose textiles Acetate textiles Blended fabrics Cellophane Photographic film

Paints and enamels Linoleum and coated fabrics Paper Printing inks

Aviation Gasoline

Lubricants

Other Refinery products

SULFURICACID 88%

CARBONDISULFIDE 3%

GROUND &DEFINED 3%

IRON & STEEL 1%

PETROLEUM 2%

CHEMICAL 17%

OTHER INDUSTRIES 6%

RAYON & FILM 3%

TITANIUM AND O

THER

PIGM

ENTS 5%

Synthetic detergents Feed additives Anti-knock gasoline Synthetic resins Protective coating Dyestuffs Oil well acidizingPetroleum catalysts

• Rhombic sulfur– “Brimstone” (when

molten)– Polyatomic (S8)– Forms SO2

Amorphous sulfur – (without shape)

Sulfur

The sudden cooling of -sulfur produces amorphous sulfur.

Amorphous(Glass)Crystalline

The Haber Process

MatterMatter

SubstanceDefinite composition

(homogeneous)

SubstanceDefinite composition

(homogeneous)

Element(Examples: iron, sulfur,

carbon, hydrogen,oxygen, silver)

Element(Examples: iron, sulfur,

carbon, hydrogen,oxygen, silver)

Mixture ofSubstances

Variable composition

Mixture ofSubstances

Variable composition

Compound(Examples: water.

iron (II) sulfide, methane,Aluminum silicate)

Compound(Examples: water.

iron (II) sulfide, methane,Aluminum silicate)

Homogeneous mixtureUniform throughout,also called a solution

(Examples: air, tap water,gold alloy)

Homogeneous mixtureUniform throughout,also called a solution

(Examples: air, tap water,gold alloy)

Heterogeneous mixtureNonuniform

distinct phases(Examples: soup, concrete, granite)

Heterogeneous mixtureNonuniform

distinct phases(Examples: soup, concrete, granite)

Chemicallyseparable

Physicallyseparable

The Organization of Matter

MATTER

PURESUBSTANCES

HETEROGENEOUSMIXTURE

HOMOGENEOUSMIXTURES

ELEMENTS COMPOUNDS

Physical methods

Chemical methods

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 41

Top Ten Elements in the Universe

Top Ten Elements in the Universe

Percent

Element (by atoms) 1. Hydrogen 73.92. Helium 24.03. Oxygen 1.14. Carbon

0.465. Neon 0.136. Iron 0.117. Nitrogen

0.0978. Silicon 0.0659. Magnesium 0.05810.Sulfur 0.044

A typical spiral galaxy(Milky Way is a spiral galaxy)

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 26

The Composition of Air

AirAir

NitrogenNitrogen

OxygenOxygenHeliumHelium

Watervapor

Watervapor

NeonNeon

Carbondioxide

Carbondioxide ArgonArgon

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 34

Chart Examining Some Components of Air

Nitrogen consists of molecules consisting of two atoms of nitrogen:

Oxygen consists of molecules consisting of two atoms of oxygen:

Water consists of molecules consisting of twohydrogen atoms and one oxygen atom:

Argon consists of individual argon atoms:

Carbon dioxide consists of molecules consistingof two oxygen atoms and one carbon atom:

Neon consists of individual neon atoms:

Helium consists of individual helium atoms:

N2

O2

H2O

Ar

CO2

Ne

HeZumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 35

Reviewing ConceptsReviewing ConceptsClassifying Matter

• Why does every sample of a given substance have the same properties?

• Explain why the composition of an element is fixed.

• Describe the composition of a compound.• Why can the properties of a mixture vary?• On what basis can mixtures be classified as

solutions, suspensions, or colloids?