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Properties of MatterWhat is matter?

Matter is anything that has mass and volume.

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Measuring MatterVolume of a liquid

– Graduated cylinder- read from bottom of meniscus

Volume of solid– Length X Width X Height

Volume of Irregular Shaped Objects– Water Displacement

Indirect Measuring– Large objects-take a core sample and use a formula– Small objects-weigh 100 and then divide weight by

100 to get one small objects weight

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Classification of Matter

MATTERHas mass and

volume

PHASESSolid, liquid, gas or plasma

MADE UP OFElement, compound

or mixture

PROPERTIESPHYSICAL

CHEMICAL

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Phases of Matter

SOLID, LIQUID, GAS, or PLASMA

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Solids - definite shape and volume Atoms are held close together by strong bonds Movement is slow

Crystalline Solids (crystals) - atoms are arranged in regular fashion (geometric)

• Ex. - ice, salt, diamonds

Amorphous Solids - atoms LACK a regular arrangement

• Ex. - rock, glass, wax

Phases of Matter

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Phases of Matter - ContinuedLiquids - NO definite shape but definite volume

Bonds are weaker and atoms are spaced apart They take the shape of container they are inExamples: oil, water, syrup, OJ, milk

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Phases of Matter - ContinuedGases - NO definite shape OR volume

Bonds are weakest and atoms far apart Expands to fill the container they are in

• Examples - air, oxygen, smoke

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Plasma• Gas like mixture of + and – charged particles Movement very rapid (10,000˚C) 99% of mass of our solar system Examples: Sun, Stars and Lightning

Phases of Matter - Continued

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Classifying Matter

• Physical Properties are those that can be observed without changing the identity of the substance

• Chemical Properties are those that describe how a substance changes into other new substances

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PROPERTIES OF MATTERPHYSICAL CHEMICAL

• Size• Shape• Texture• Color• Phase• Conductor• Ductile• Malleable• Shiny/luster• Density• Mass• Tasteless

• Flammability• Changes color• Reacts with• Combustible• Corrosive• Volatile• Explosive

DissolvesOdorlessHardnessBrittleTensile strengthFluidViscosityElasticityBuoyantMelting pointFreezing pointBoiling point

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Physical Properties of Matter• Viscosity –

• Measure of the material’s resistance to flow• High-viscosity liquids take longer to flow

• Example: Ketchup when comparing to water

• Low-viscosity liquids flow easier• Example: Tomato Juice flows easier than ketchup

• Temperature raising-viscosity decreases except in gases.

                  

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Physical Properties of Matter – Cont.

• Elasticity – • Measure of ability to be stretched and then return to its original size.• Example:Rubber Bands, Elastic, and Playground Balls

Question: Which ball would you rather play basketball?

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• Malleability – • Ability to be hammered into sheets• Example: Gold &Silver Coins, Aluminum Foil and Soda Cans

Physical Properties of Matter – Cont.

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• Brittleness – • measures a material’s tendency to shatter upon impact• Example: Sulfur, Calcium and Glass

• Hardness –• Resistance to breaking or scratching• Example: diamonds

Physical Properties of Matter – Cont.

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• Luster – • shininess• Example: Gold, Silver, Mercury

• Ductility – • ability to be pulled into wires• Example: Most metals (Copper, Silver)

Physical Properties of Matter – Cont.

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Physical Properties of Matter – Cont.

Tensile Strength-• Measure of how much

pulling, or tension, a material can withstand before breaking

• Property of fibers, ropes, cables, girders

• DuPont Kevlar-5 times tensile strength of steel

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Melting Point – • Temperature at which a solid changes to a liquid• Example: Ice water

Freezing Point – • Temperature at which a liquid changes to a solid• Example: Water Ice (0°C)

Physical Properties

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Boiling Point –• Temperature at which a liquid changes into a gas• Example: Water vapor (100˚ C)

Physical Properties

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• Density – • The amount of mass in a given volume• How tightly packed the atoms or molecules

are in a substance• Formula to calculate density is:

Density = Mass Volume

• Units are expressed as:• g/mL or g/L for liquids (remember the graduated

cylinder)• g/cm3 for solids

Physical Properties of Matter – Cont.

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Density of a Fluid

Fluid-• Any matter that is able to flow• Liquids and gases• Density of a liquid might be different from the

density of the same solid• Most materials are denser in solid phase

than their liquid phase• Exception- Water-freezes with air spaces so

it is less dense and floats.• Density of liquid water is 1 g/ml

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• Buoyancy – • Upward force a fluid exerts on an object•Determines whether the object will sink or float• Example: Buoyancy of water keeping you afloat while swimming

Physical Properties of Matter – Cont.

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Buoyancy

Buoyancy force is LESS then object’s weight, object will SINK

Buoyancy force is EQUAL to the object’s weight, object will FLOAT

Buoyancy force is MORE then object’s weight, object will FLOAT IN AIR

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Archimedes's Principle• Greek mathematician, 3rd century BC• Principle states-The buoyancy force on an object in a

fluid is equal to the weight of the fluid displaced by the object

Buoyancy of Gasses• Balloon floats because it displaces a very large

volume of air• Volume of air displaced weighs more than the balloon

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Classification of Matter

E L E M E N TO n ly 1 K in d

o f A tom

C O M P O U N DTwo o r M ore

K in d s o fA tom s

S U B S TA N C E SD efin ite C om p os it ion

H O M O G E N E O U SS olu tion even ly

m ixed

H E TE R O G E N E O U SS olu tion

U n even ly m ixed

M IX TU R E SV ariab le C om p os it ion

M A TTE RH as m ass an d

takes u p sp ace.

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Classification of Matter

Matter can be divided into 2 categories:SUBSTANCES & MIXTURES

• Substances can NOT be separated into different kinds of matter by physical means.

• Mixtures can be separated into different kinds of matter by physical means.

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What are substances?

– Elements • Any substance in which all the atoms in a sample are alike, one kind of matter• Examples: Carbon, Sodium and Oxygen

– Compounds• 2 or more elements chemically combined in a fixed ratio (subscript)• Usually has different appearance from elements that make it up• Examples: Water – H2O and Salt - NaCl

Classification of MatterIn science, substances are limited to elements and compounds.

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Classification of Matter

• Atom-smallest possible particle of an element

• Molecule- smallest possible particle of a compound

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What are mixtures? 2 or more substances that can be separated by

physical meansDo not always contain the same amounts of the different substances that make them up

–Homogeneous• same throughout, particles so tiny that cannot be seen, don’t settle out or scatter light • Examples: milk, salt water and cola

–Heterogeneous• a mixture in which different materials can be easily distinguished•Suspension-visible particles settle-muddy water• Examples: Sand/water, Italian salad dressing, pizza and dry soups

Classification of Matter

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Changes in Matter

MATTER

PHYSICAL CHANGES

NUCLEAR CHANGESCHEMICAL

CHANGES

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Changes in Matter

• Melting• Freezing• Boiling• Evaporation• Cutting• Splitting• Chopping• Sublimation

• Chemical reaction• Photosynthesis• Respiration• Digestion of food

Physical Chemical

Nuclear•Fission

•Fusion

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Physical vs. Chemical ChangePhysical Change - Does NOT create a new substance, affects only the physical properties.

Appearance changes – not chemical makeup

A change in size, shape or form (phases of matter).

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Physical Change

Vaporization-• process at which a liquid

changes to a gas by increasing the temperature to the liquids boiling point

• Example: water boils to form steam at 100° C

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Physical Change

Evaporation-• process at which a liquid

changes to a gas. The liquid is not boiling.

Example: A puddle drying up or sweat drying

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Physical ChangeCondensation –

• Process at which a gas becomes a liquid•Gas cooled below its boiling point• Example: water vapor water, dew in the morning, glass of ice tea in hot weather.

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Physical changeSublimation –

• When a solid changes directly to a gas•The matter doesn’t melt• Example:snow, dry ice

and glaciers

Deposition-

•Gas changes directly into a solid

•Ex. Fire extinguisher

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Chemical Change - A change in which a NEW substance is created

End products are chemically different from the original.

Chemical Change

Corrosive-dissolving away of a metal-rusting

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Four Signs or Evidence of a Chemical Change

• Gas forms• Permanent color change• Heat/or light energy is given off• Precipitate forms. A precipitate is an

insoluble substance that forms out of solution.

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Identify the following as physical or chemical change.

Ice cube melting.

Slicing an apple into pieces.

Physical vs. Chemical Change

Wood burning.

People eating.

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Changes in Matter - Continued

Exotic Super Hot• Nucleus of atom

comes apart• Particle accelerates

Exotic Super Cold• Below -270˚ C• Superfluids from gases

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Charles’ Law

Jacques Charles, French scientist (1742-1823)

• Law states-volume of a gas increases when temperature increases and reverse, volume of gas decreases when temperature decreases.

• V1 / T1 = V2 / T2 – Temperature must be in Kelvin degrees (+273)

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Boyle’s Law

Robert Boyle-British scientist (1627-1691)• Law states-as pressure of a gas increases,

its volume decreases proportionately and reverse pressure of gas decreases, its volume increases proportionately.

• P1 V1 = P2 V2

• Pascal-unit for pressure (Pa) (kPa)