Matter – Properties Matter – Properties and Changesand Changes
Properties of MatterProperties of MatterChanges of MatterChanges of MatterMixtures of MatterMixtures of Matter
Elements and CompoundsElements and Compounds
PROPERTIES OF MATTERPROPERTIES OF MATTERTypes of PropertiesTypes of Properties
Physical PropertiesPhysical Properties - properties that can be - properties that can be observed and measured without changing observed and measured without changing the compositionthe composition
examples – color, texture, hardness)examples – color, texture, hardness) types of physical propertiestypes of physical properties 1) 1) intensiveintensive - do not depend upon amount of - do not depend upon amount of the substancethe substance 2) 2) extensiveextensive - depend upon amount of - depend upon amount of the substancethe substance
Examples:Examples:lengthlengthcolorcolormassmassvolumevolumedensitydensityphasephaseconductivityconductivitytexturetexture
Properties- PhysicalProperties- Physical
Properties of MatterProperties of Matter
chemists use characteristic chemists use characteristic properties to tell substances apart properties to tell substances apart and to separate themand to separate them
some properties define a group of some properties define a group of substancessubstances
Types of PropertiesTypes of Properties
PhysicalPhysical- characteristics that can be - characteristics that can be observed or measured without observed or measured without changing the identity of a substancechanging the identity of a substance
Ex. melting point, boiling ptEx. melting point, boiling pt ChemicalChemical- relates to a substances - relates to a substances
ability to undergo changes that ability to undergo changes that transform it into a different substancetransform it into a different substance
Easiest to see when a chemical is Easiest to see when a chemical is reactingreacting
Physical Changes in MatterPhysical Changes in Matter change in a substance that doesn’t change in a substance that doesn’t
change the identity of the substancechange the identity of the substance Ex. grinding, cutting, melting, boilingEx. grinding, cutting, melting, boiling Includes all changes of state Includes all changes of state
(physical changes of a substance (physical changes of a substance from one state to another)from one state to another)
SolidSolid
•definite volumedefinite volume•definite shapedefinite shape•atoms are packed atoms are packed
together in fixed together in fixed positionspositions
•strong attractive strong attractive forces between forces between atomsatoms
•only vibrate in placeonly vibrate in place
LiquidLiquid
•definite definite volumevolume
•indefinite indefinite shapeshape
•atoms are atoms are close close together together
•atoms can atoms can overcome overcome attractive attractive forces forces to flowto flow
GasesGases
•indefinite indefinite volumevolume•indefinite shapeindefinite shape•atoms move very atoms move very
quicklyquickly•atoms are far atoms are far
apartapart•pretty weak pretty weak
attractive forcesattractive forces
PlasmaPlasma
high temperature state in which high temperature state in which atoms lose their electronsatoms lose their electrons
Ex. the sunEx. the sun
CHANGES IN MATTERCHANGES IN MATTERTypes of ChangesTypes of Changes
1. 1. physicalphysical - changes in which a substance is - changes in which a substance is altered without changing compositionaltered without changing composition
a. examples- phase changes, cut into piecesa. examples- phase changes, cut into pieces
2. 2. chemical chemical - changes in which one or more - changes in which one or more substances change into new substances with substances change into new substances with
new propertiesnew properties
a. a. reactants reactants – substances that react– substances that react
b. b. productsproducts - substances that are produced - substances that are produced
PROPERTIES OF MATTERPROPERTIES OF MATTERTypes of PropertiesTypes of Properties
Chemical PropertiesChemical Properties - properties relating - properties relating to the ability of substances to combine to the ability of substances to combine with or change into other substance with or change into other substance (has a uniform and unchanging (has a uniform and unchanging composition)composition)
examplesexamples
1) reaction with water1) reaction with water
2) ability to combine with oxygen2) ability to combine with oxygen
3) reaction with acids3) reaction with acids
Changes that result in a new substanceChanges that result in a new substance a.k.a chemical reactiona.k.a chemical reaction
Word equation:Word equation:
hydrogen + oxygenhydrogen + oxygen waterwater
reactantsreactants product product
copper + silver nitratecopper + silver nitrate silver + copper silver + copper nitratenitrate
reactantsreactants product product
Changes ChemicalChanges Chemical
Formula EquationFormula Equation
Cu + 2AgNOCu + 2AgNO33 Cu(NO Cu(NO33))22 + + 2Ag2Ag
Pb(NOPb(NO33))22 + 2KI + 2KI PbI PbI22 + 2KNO + 2KNO33
ChangesChangesChemicalChemical
(be able to identify reactants and products)(be able to identify reactants and products)
Chemical changesChemical changes
Examples of chemical changes Examples of chemical changes
1) digestion of food1) digestion of food
2) burning (combustion)2) burning (combustion)
3) fermentation3) fermentation
4) rusting4) rusting
5) tarnishing of silver5) tarnishing of silver
CHANGES IN MATTER CHANGES IN MATTER Evidence of Chemical ChangesEvidence of Chemical Changes
1. change in color and/or appearance 1. change in color and/or appearance
2. change in energy 2. change in energy
3. change in odor3. change in odor
4) formation of a precipitate or a gas 4) formation of a precipitate or a gas
Energy Changes in MatterEnergy Changes in Matter
when any change occurs, energy when any change occurs, energy is always involvedis always involved
energy can be in different forms energy can be in different forms (light, heat, etc.) (light, heat, etc.)
energy is never destroyed or energy is never destroyed or created (law of conservation of created (law of conservation of energy)energy)
Energy changes related Energy changes related to chemical changes to chemical changes
(reactions)(reactions)1.1. exothermicexothermic - energy is released - energy is released
(given off in the form of heat or light)(given off in the form of heat or light)
- burning, explosion- burning, explosion
2.2. endothermicendothermic - energy must be - energy must be continuously added to keep the continuously added to keep the reaction goingreaction going
- electrolysis of water or salt- electrolysis of water or salt
Energy Changes in MatterEnergy Changes in Matter
Exothermic Reaction-Exothermic Reaction- reaction that reaction that gives off energy (feels warm on gives off energy (feels warm on outside)outside)
Endothermic ReactionEndothermic Reaction- reaction that - reaction that uses up energy (feels cold on outside)uses up energy (feels cold on outside)
MIXTURESMIXTURES
A. DefinitionA. Definition of Mixtureof Mixture - combination of - combination of pure substances that retain their propertiespure substances that retain their properties
B. Types of MixturesB. Types of Mixtures
1. 1. heterogeneous heterogeneous - individual substances are - individual substances are distinct (composition is not uniform distinct (composition is not uniform throughout)throughout)
a. examples – sand, vegetable soup a. examples – sand, vegetable soup
2. 2. homogeneoushomogeneous - individual substances are - individual substances are not distinct (uniform composition throughout)not distinct (uniform composition throughout)
a. examples - solutions a. examples - solutions
MIXTURES MIXTURES Types – homogeneousTypes – homogeneous
____________________________________________________________________________________________________________________________________________________________________________________________________________________
type of solution examplestype of solution examples__________________________________________________________________________________________________________ __________________________________________________________________________________________________________
solid – liquid sugar water, salt watersolid – liquid sugar water, salt water______________________________________________________________________________________ gas – liquid carbonated beveragesgas – liquid carbonated beverages________________________________________________________________________________________________________________
liquid – liquid alcohol, vinegarliquid – liquid alcohol, vinegar________________________________________________________________________________________________________________
gas – gas airgas – gas air______________________________________________________________________________________________________________
solid - solid alloys (metal + metal)solid - solid alloys (metal + metal)________________________________________________________________________________________________________________
MIXTURES MIXTURES Separating MixturesSeparating Mixtures
1. Filtration1. Filtration
2. Distillation2. Distillation
3. Crystallization3. Crystallization
4. Chromatography4. Chromatography
Separation TechniquesSeparation Techniques
FiltrationFiltration- solid part is - solid part is trapped by filter trapped by filter paper and the liquid paper and the liquid part runs through the part runs through the paperpaper
VaporizationVaporization- where - where the liquid portion is the liquid portion is evaporated off to evaporated off to leave solidleave solid
Separation TechniquesSeparation Techniques
DecantingDecanting- when - when liquid is poured off liquid is poured off after solid has settled after solid has settled to bottomto bottom
CentrifugeCentrifuge- machine - machine that spins a sample that spins a sample very quickly so that very quickly so that components with components with different densities different densities will separatewill separate
Separation TechniquesSeparation Techniques
Paper Paper Chromatography-Chromatography- used to separate used to separate mixtures because mixtures because different parts different parts move quicker on move quicker on paper than otherpaper than other
ELEMENTS AND COMPOUNDSELEMENTS AND COMPOUNDSElement-Element-a pure substance that cannot be a pure substance that cannot be broken down by simple meansbroken down by simple means
The periodic table organizes the 91 naturally The periodic table organizes the 91 naturally occurring elements and scientifically created occurring elements and scientifically created elementselements
A. Mendeleev created the original A. Mendeleev created the original periodic table.periodic table.
Mendeleev's Periodic Table (1869).htm
Periodic TablePeriodic Table
two rows below the periodic table are two rows below the periodic table are the the lanthanide and actinide serieslanthanide and actinide series
these rows fit after #57 and #89these rows fit after #57 and #89 they are only at the bottom to keep they are only at the bottom to keep
the width of the chart smallerthe width of the chart smaller
Types of Elements Types of Elements MetalsMetals
an element that is a good an element that is a good conductor of electricityconductor of electricity
at room temperature, most are at room temperature, most are solidssolids
malleablemalleable- can be rolled or - can be rolled or hammered into sheetshammered into sheets
ductileductile- can be made into wire- can be made into wire high high tensile strength-tensile strength- can resist can resist
breakage when pulledbreakage when pulled most have silvery or grayish most have silvery or grayish
white lusterwhite luster
Types of ElementsTypes of Elements
NonmetalsNonmetals an element that is a poor conductor of an element that is a poor conductor of
heat and electricityheat and electricity many are gases at room temperaturemany are gases at room temperature some are solids: usually brittle, not some are solids: usually brittle, not
malleablemalleable
Types of ElementsTypes of Elements
MetalloidsMetalloids an element that has some an element that has some
characteristics of metals and nonmetalscharacteristics of metals and nonmetals appear along staricase lineappear along staricase line B, Si, Ge, As, Sb, TeB, Si, Ge, As, Sb, Te all are solids at room temperatureall are solids at room temperature less malleable that metals but less less malleable that metals but less
brittle than nonmetalsbrittle than nonmetals are semiconductorsare semiconductors
Types of ElementsTypes of Elements
Noble GasesNoble Gases generally unreactive gasesgenerally unreactive gases in far right column of periodic tablein far right column of periodic table
ELEMENTS AND COMPOUNDSELEMENTS AND COMPOUNDSCompoundsCompounds
definition - a compound is a pure substance definition - a compound is a pure substance that is the combination of two or more that is the combination of two or more different elementsdifferent elements
ie: NaCl – table saltie: NaCl – table salt
Na- combustible solid and Cl – poisonous gasNa- combustible solid and Cl – poisonous gas
examples of compoundsexamples of compounds a. sodium bicarbonate NaHCOa. sodium bicarbonate NaHCO33
b. hydrochloric acid HClb. hydrochloric acid HCl c. sulfur dioxide SOc. sulfur dioxide SO22
ELEMENTS AND COMPOUNDSELEMENTS AND COMPOUNDSCompoundsCompounds
examples of formation of compounds examples of formation of compounds from elements (synthesis reactions)from elements (synthesis reactions)
a. 2 Na + Cla. 2 Na + Cl22 -----> 2 NaCl -----> 2 NaCl
b. 2 Hb. 2 H22 + O + O22 ------> 2 H ------> 2 H22OO
c. Nc. N22 + 3H + 3H22 ------> 2NH ------> 2NH33
ELEMENTS AND COMPOUNDSELEMENTS AND COMPOUNDSCompoundsCompounds
examples of decomposition of examples of decomposition of compounds to form elementscompounds to form elements
a. 2NaCl a. 2NaCl 2Na + Cl 2Na + Cl22
b. 2 Hb. 2 H22O O 2H 2H22 + O + O22
The organization of MatterThe organization of Matter
matter
mixtures Pure substances
ElementsOxygen, iron
heterogeneous homogeneous CompoundsSalt, sugar
Matter FlowchartMatter Flowchart
MATTER
Can it be separated by physical means?
Homogeneous Mixture
(solution)
Heterogeneous Mixture Compound Element
MIXTURE PURE SUBSTANCE
yes no
Can it be decomposed by chemical means?
noyesIs the composition uniform?
noyes
The Law Conservation of MassThe Law Conservation of Mass
States that mass can neither be States that mass can neither be created nor destroyed.created nor destroyed.
Mass of reactants = mass of productsMass of reactants = mass of products
28 g of Na + 28 g of Cl = 56 g of NaCl28 g of Na + 28 g of Cl = 56 g of NaCl
Law of Conservation of Law of Conservation of Mass and chemical Mass and chemical
changeschanges- - Mass reactants = Mass products Mass reactants = Mass products (mass is neither created nor (mass is neither created nor
destroyed in chemical reactions)destroyed in chemical reactions)
Lavoisier (1743 - 1794) experimentLavoisier (1743 - 1794) experiment [ 216 g of HgO --> 200 g Hg + 16g O[ 216 g of HgO --> 200 g Hg + 16g O22
]]216 grams of mercury oxide when heated 216 grams of mercury oxide when heated
will produce 200 grams of mercury and will produce 200 grams of mercury and 16 grams of oxygen16 grams of oxygen
Law of Definite Law of Definite ProportionsProportions
1.Definition - a compound is always composed of 1.Definition - a compound is always composed of the same elements in the same proportions by the same elements in the same proportions by massmass
2. examples 2. examples a. water- Ha. water- H22O (always has a ratio of 1 gram of O (always has a ratio of 1 gram of hydrogen to 8 grams of oxygen) hydrogen to 8 grams of oxygen) b. ammonia - NHb. ammonia - NH33 (always combine in a ratio of (always combine in a ratio of
14 grams of nitrogen to 3 grams of hydrogen)14 grams of nitrogen to 3 grams of hydrogen)
Law of Multiple Law of Multiple ProportionsProportions
1. definition - when different 1. definition - when different compounds are formed by a compounds are formed by a combination of the same elements, combination of the same elements, different masses of one element will different masses of one element will combine with the same relative mass combine with the same relative mass of the other element in a ratio of of the other element in a ratio of small whole numberssmall whole numbers
Law of Multiple Law of Multiple ProportionsProportions
WATER (HWATER (H22O) O) 2 grams of hydrogen combine with 16 2 grams of hydrogen combine with 16
grams of oxygen grams of oxygen PEROXIDE (HPEROXIDE (H22OO22) ) 2 grams of hydrogen combine with 32 2 grams of hydrogen combine with 32
grams of oxygen grams of oxygen The ratio that compares the amount of The ratio that compares the amount of
oxygen in water and peroxide is 1:2 oxygen in water and peroxide is 1:2
Law of Multiple Law of Multiple ProportionsProportions
SULFUR DIOXIDE (SOSULFUR DIOXIDE (SO22)) 32 grams of sulfur combine with 32 grams of 32 grams of sulfur combine with 32 grams of
oxygenoxygen
SULFUR TRIOXIDESULFUR TRIOXIDE (SO (SO33) ) 32 grams of sulfur combine with 48 grams of 32 grams of sulfur combine with 48 grams of
oxygenoxygen
The ratio that compares the amount of oxygen in The ratio that compares the amount of oxygen in sulfursulfur
dioxide and sulfur trioxide is 2:3dioxide and sulfur trioxide is 2:3
Periodic TablePeriodic Table
GroupsGroups also called familiesalso called families vertical columnsvertical columns numbered 1numbered 11818 have similar chemical propertieshave similar chemical properties
PeriodsPeriods horizontal rowshorizontal rows properties changes consistently across a properties changes consistently across a
periodperiod
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