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Transcript of Classification of CLASSIFICATON OF MATTER Copy flowchart below leaving space below each for notes...
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