Classification of

CLASSIFICATON OF MATTERCopy flowchart below leaving space below each for notes

physically

separable

chemically

separable

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Classification of matter• Matter is classified as a:

– Something that has mass and occupies space– It can be perceived by one or more senses– Exists as a solid, liquid, gas, or plasma

• Can be a Substance or a Mixture

Substances– cannot be broken down into simpler components by physical means.– matter that has a fixed (constant) composition and unique properties. – Contains only 1 type element or compound; homogeneous

• Examples

Elements : only 1 type of atom (see Periodic Table) Calcium (Ca), Nitrogen (N), and Oxygen (O),

Compounds: 2 or more CHEMICALLY combined elements (separated from each other by chemical means) Water H2O, Carbon Dioxide CO2

Pure Substances: (elements(elements oror compounds)compounds)

Have 1 capital Have 1 capital letterletter

Have 2 or more capital Have 2 or more capital letterslettersElements:

composed of one type of atomcomposed of one type of atom

copper wire copper wire (Cu)(Cu)

aluminum foil aluminum foil (Al)(Al)

Silver (Ag)Silver (Ag) Gold (Au)Gold (Au)

CompoundCompounds:s: composed of 2 or more elements

that are chemically bonded together.

they can be broken down only through chemical changes.

Water Water (H(H22O)O)

salt salt (NaCl)(NaCl)

carbon dioxide (COcarbon dioxide (CO22)) sand (SiOsand (SiO22))

Elements in compounds have Elements in compounds have different properties from pure different properties from pure elementselements

3 classes of Elements1) Metals: shiny (high luster), conduct electricity,

malleable, ductile

2) Nonmetals: dull, don’t conduct, brittle

3) Metalloids: properties of both

2 Classes of Compounds1) Inorganic: do not

contain carbon; ex: NO2, H2O

2) Organic: contain carbon ex: CO2, CH4

What is a Mixture?

What_is_a_Mixture_.asf

Mixtures– Material made up of two or more substances that can be easily separated by physical means.– Contains at least 2 PHYSICALLY combined compounds; can be homogeneous or

heterogeneous– Physical Separation of Mixtures: distillation/evaporation, filtration, centrifugation/gravity,

magnetic extraction, chromatography, or sorting

Separation of a MixtureComponents of dyes such as ink may be separated by paper chromatography.

Separation of a MixtureDistillation: takes advantage of different boiling points.

NaCl boils at 1415 oC

Mixtures:

composed of two or more different pure substances

cannot be identified by chemical formulas

can be separated through physical means

can be homogeneous mixtures or heterogeneous mixtures

solutions, suspensions and colloids

Types of mixtures:

Four states (phases) of matter:

solids liquids gases

** Mixtures can be composed of any combination of these!

heterogeneous mixtureheterogeneous mixturehomogeneous mixturehomogeneous mixture

plasma

Test Your KnowledgePure Substance or Mixture?!?!

1. Kool-aid

2. distilled water

3. tap water

4. chocolate chip cookie

5. oxygen gas

6. atmosphere

7. Glucose (C6H12O6)

mixture

mixture

mixture

mixture

Pure substance

Pure substance

Pure substance

Composition of Matter• Heterogeneous Mixture

– A mixture in which different materials can be distinguished easily with the naked eye

– 2 or more PHYSICALLY combined substances (elements/compounds)

– Examples: Pizza, Concrete,

blood, fog, muddy water

Composition of Matter• Homogeneous Mixtures

– Contains two or more gaseous, liquid, or solid substances blended evenly throughout.

– Also known as a solution: a special kind of mixture 2 phases/parts (SOLUTE dissolves & SOLVENT does the dissolving)

– Examples:• Kool aid (Sugar, Water, Food Color)• Scuba Tank (Oxygen and Nitrogen)• sterling silver (alloy: 92.5% Ag and 7.5% Cu) • Brass (Copper and Zinc )

• Air is a mixture of gases, 78% N2 and 21% O2 with traces of H2O, CO2, Ar, and various other components...

Heterogeneous vs Homogeneous Mixtures

Classification of Matter

Compound vs. MixtureCompound Mixture

Made of one kindof material

Made of more thanone kind of material

Made by a chemical change

Made by a physical change

Definitecomposition

Variablecomposition

Which is it?

ElementCompoundMixture

Test Your KnowledgeElement, Compound or Mixture?!?!

1. silver

2. pine tree

3. orange juice

4. phosphorus

5. iced tea

6. Acetaminophen (aspirin) C8H9O2N

element

element

mixture

mixture

mixture

compound

Heterogeneous vs. Homogenous Substances

HomogeneousHomogeneous HeterogeneousHeterogeneous

The Tyndall Effect The Tyndall Effect can be seen in mixtures

whose particles are large enough to scatter light.~ can see a beam of light passing through the

mixture~ can be observed in both colloids and suspensions

Solutions.asf

Suspensions.asf

Colloids.asf

Heterogeneous MixturesHeterogeneous Mixtureshas two sub groupshas two sub groups

• 1. Colloids1. Colloids

• Type of mixture that never settles

• ExampleExample

• Mayonnaise

• ketchup

• Paint

• Jell-O

• milk

• fog

• 2. Suspensions• Mixture in which

visible particles settle• Example • Pond Water• River deltas• Blood• Salad dressing

3 classes of MIXTURESSolution Colloid Suspension

Heterogeneous or Homogeneous

Homo Hetero Hetero

Examples salt water, air

Soot, fog, mayonnaise

Muddy water, Italian dressing

Particle Type ions, atoms Small Clusters Large Clusters

Particle Size

Scatter Light? (TYNDALL EFFECT)

Settle while standing?

Separate by filtration?

BROWNIAN MOTION- chaotic movement of particles

small medium large

No

No

No

No

No

yes yes

yes

yes

Properties of

Matter

Chemistry

Properties of Matter

• The properties of a substance are those characteristics that are used to identify or describe it. 

• When we say that water is "wet", or that silver is "shiny", we are describing materials in terms of their properties.

Properties of Matter Observable properties of matter fall into two catergories.

1. An intensive property is a property that depends on the type of matter in a sample, not the amount of matter.

• boiling point: water boils at the same temperature no matter if you have 1 gram, 10 grams or 100,000 kilograms of water

2. An extensive property is a property that depends on the amount of matter in a sample• volume: 100 grams of water takes up more

volume than 1 gram of water.

Extensive Properties– Depends on the amount of matter in the

sample• Mass

• Volume

• Calories

• Concentration

• Weight

2.1

Intensive Properties• Depends on the type of matter, not the

amount present– Hardness– Density– Solubility– Luster– Taste – Color

2.1

More Intensive Properties– Reactivity – Malleability– Conductivity – Flammability– Boiling/Condensation

Point– Melting/ Freezing Point

2.1

Intensive vs. Extensive Properties• Will all samples of the same substance have

the same extensive properties? – No. Extensive properties depend on the

AMOUNT of matter, not what the matter is composed of.

• Will all samples of the same substance have the same intensive properties? – Yes. Intensive properties depend on what the

matter is composed of.

2.1

Classify each of the following as an intensive property or an extensive property.

1. Mass

2. Density

3. Volume

4. Melting point

5. Length

6. Color

1. Extensive

2. Intensive

3. Extensive

4. Intensive

5. Extensive

6. Intensive

Properties are…• Words that describe matter (adjectives)• Physical Properties- a property that can be

observed and measured without changing the material’s composition.

• Examples- color, hardness, m.p., b.p.• Chemical Properties- a property that can

only be observed by changing the composition of the material.

• Examples- ability to burn, decompose, ferment, react with, etc.

States of matter1) Solid- matter that can not flow (definite

shape) and has definite volume.

2) Liquid- definite volume but takes the shape of its container (flows).

3) Gas- a substance without definite volume or shape and can flow.

– Vapor- a substance that is currently a gas, but normally is a liquid or solid at room temperature. (Which is correct: “water gas”, or “water vapor”?)

States of MatterStates of Matter

Solid

Liquid

Gas

Definite Volume

YES

YES

NO

Definite Shape

YES

NO

NO

Result of a TemperatureIncrease

Small Expans.

Small Expans.

Large Expans.

Compressible

NO

NO

YES

Three Main Phases

Solid Liquid Gas

Melt Evaporate

CondenseFreeze

Copper Phases - Solid

Copper Phases - Liquid

Copper Phases – Vapor (gas)

4th state: Plasma - formed at high temperatures; ionized phase of matter as found in the sun or borealis

Physical vs. Chemical Change• Physical change will change the visible

appearance, without changing the composition of the material.

– Boil, melt, cut, bend, split, crack

– Is boiled water still water?

• Can be reversible, or irreversible

• Chemical change - a change where a new form of matter is formed.

– Rust, burn, decompose, ferment

Chemical ChangeA change in which one or more substances are converted into different substances.

Heat and

light are often evidence of a chemical change.

Chemical Changes• The ability of a substance to undergo a

specific chemical change is called a chemical property.

• iron plus oxygen forms rust, so the ability to rust is a chemical property of iron

• During a chemical change (also called chemical reaction), the composition of matter always changes.

Chemical Reactions are…• When one or more substances are changed

into new substances.

• Reactants- the stuff you start with

• Products- what you make

• The products will have NEW PROPERTIES different from the reactants you started with

• Arrow points from the reactants to the new products

Recognizing Chemical Changes1) Energy is absorbed or released (temperature

changes hotter or colder)

2) Color changes

3) Gas production (bubbling, fizzing, or odor change; smoke)

4) formation of a precipitate - a solid that separates from solution (won’t dissolve)

5) Irreversibility - not easily reversed

But, there are examples of these that are not chemical – boiling water bubbles, etc.

Conservation of Mass • During any chemical reaction, the mass of

the products is always equal to the mass of the reactants.

• All the mass can be accounted for:

– Burning of wood results in products that appear to have less mass as ashes; where is the rest?

• Law of conservation of mass

Law of Conservation of Mass

• Mass of all substances that are present before a chemical change equals the mass of all the substances that remain after the change.

- Page 55

reactants = product

43.43 g Original mass = 43.43 g Final mass

• Example Problem:

• In the following reaction, 18g of hydrogen react completely with 633 g of chlorine. How many grams of HCl are formed?

H2+Cl2=>2HCl

18g +633g =651g

Practice problem• In the following reaction, 24g of CH4 react

with 96g of O2 to form 66g of CO2. How many grams of H2O are formed?

CH4 + 2O2 => CO2 + 2H2O24g + 96g = 66g + ______

120g = 66g + ___?___

120g - 66g = 54g