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SubstancesSubstances
A pure substance is an element or a compound.
Substances have the same characteristicsthroughout meaning that all samples have thesame characteristics.
An element is a substance composed of only onekind of atom.
Elements can not be broken down into a simplersubstance by ordinary chemical means.
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Elements and CompoundsElements and Compounds
Examples of elements:
oxygen, carbon, nitrogen
Compounds are homogeneous substancesformed by the chemical bonding of two ormore different kinds of atoms resulting
from achemical reaction.
Compounds have properties uniquelydifferent from the elements making it up.
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CompoundsCompounds
Examples of compounds:
water, carbon dioxide, sodium chloride
The Law of Definite Proportions states themass of the constituent elements alwaysremains the same.
In every 100. g sample of NaCl, 39.3 g is
sodium and 60.7 g of chlorine.
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CompoundsCompounds and Mixtures and Mixtures
When a compound is formed, evidence of achemical reaction is usually obvious.
Light is given off or heat is either absorbed or liberated.
Mixtures are physical combinations of two or
more substances.
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MixturesMixtures
In a mixture, the components can be presentin any proportion.
NaCl(aq) – a salt water solution can existin any proportion.
When a mixture is formed, there is noevidence of a chemical reaction taking place.
In a mixture, the components do not lose theiridentity.
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MixturesMixtures
Mixtures can be either homogeneous orheterogeneous.
Mixtures having uniform characteristics
are homogeneous.
Mixtures having varying characteristics throughout the sample are heterogeneous.
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ClassificationClassification of Matter of Matter
Matter
Pure Substance
Mixture
Element
Compound
Homogeneous
Heterogeneous
Matter
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Physical Physical PropertiesProperties
Characteristics that can be observed withoutproducing a new substance.
ExamplesExamples
color densityodormelting point
volume boiling point
compressibility mass
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Chemical Chemical PropertiesProperties
Characteristics that describe how asubstance reacts with another substance to form a new substance.
2H2(g) + O2(g) 2H2O(l)
The reactants hydrogen and oxygen havemuch different characteristics than theproduct water.
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PhysicalPhysical Changes Changes
No new substances are formed as a result of
a physical change.
In a physical change, one or more physicalproperties are changed.
Changes of state or phase such ascondensation or vaporization and changes
insize by tearing, breaking, grinding areexamples of physical changes.
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ChemicalChemical Changes Changes
A chemical change results in the formation of
one or more new substances.
The new substances differ in chemicalproperties and composition from the originalsubstance.
Examples of Chemical Changes
rusting of iron
burning of paper
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ChemicalChemical Changes Changes
When the following are not associated with achange of phase (state), they represent achemical change.
formation of a gas (bubbles)
formation of a solid (precipitate)
absorbing (endothermic) or giving (exothermic) off heat
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PropertiesProperties
Properties are characteristics that used todescribe substances.
Properties can be either extensive orintensive.
Extensive properties depend on the amountof substance present.
Examples are weight, mass, volume, and length.
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PropertiesProperties
Intensive properties are independent of theamount of substance present.
Examples are density, temperature, and boiling point.
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Law of Definite ProportionsLaw of Definite Proportions
Once a given compound is formed, itschemical composition is always constant.
2C(s) + O2(g) → 2CO(g)
The mass ratio is: C:O 12 g:16 g
The atom ratio is: C:O 1 C:1 O
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Law of Law of MultipleMultiple Proportions Proportions
Two elements combining with each other may
join in varying ratios to form differentcompounds (compare to the product
formedin previous slide).
C(s) + O2(g) → CO2(g)
The mass ratio is: C:O 12 g:32 g
The atom ratio is: C:O 1 C:2 O
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Dalton’s Dalton’s AtomicAtomic Theory Theory
All matter is composed of atoms and an atom
is the smallest particle of an element that takes
part in a chemical reaction.
All atoms of an element are alike.
Compounds are combinations of atoms of one
or more elements. The relative number ofatoms for each element is always the same.
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Dalton’s Dalton’s AtomicAtomic Theory Theory
Atoms can not be created or destroyed in achemical reaction.
Atoms can only change how they combine with
each other.