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Chapter 3
Matter – Properties & Changes
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Introduction:
What is matter?
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Introduction Matter – anything that has mass and
volumeThe atom is the building block of all
matter
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States of Matter
What are the 3 main states of matter?
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States of Matter
SolidHas definite shape & volumeParticles are tightly packedCan expand when heated
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States of Matter
LiquidHas constant volume but takes the shape
of its containerFluidLess closely packed particles than solid
particlesCan expand when heated
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States of Matter
GasExpands to fill its container & takes the
shape of its containerFluidMuch less closely packed than solid
particlesExpands when heated
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States of Matter 1)
2)
3)
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States of Matter - Plasma
PlasmaDoes not naturally occur on Earth (except in
lightning) Present in the Sun
An ionized gas Sufficient energy is provided to
free electrons from atoms or molecules and to allow both ions and electrons to coexist
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Phase Changes
When a substance freezes, boils, evaporates, or condenses, it undergoes a phase changeThe addition or removal of energy is
what causes phase changesThis change is also a physical change
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Phase Changes
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Matter
Mixtures Pure Substances
Heterogeneous
Homogeneous
Element
Compound
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Types of Matter Mixtures
1. Physical combinations of 2 or more substances
2. Components do not chemically react with each other
Pure Substances1. Elements
2. Compounds
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Mixtures
Mixture – a combination of two or more pure substances in which each pure substance retains its individual chemical properties
2 kinds: Heterogeneous Homogeneous
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Heterogeneous Mixtures
Mixture that does not blend smoothly throughout – individual substances remain distinct
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Homogeneous Mixtures Mixture that has constant composition
throughoutExamples: salt water, soda water, brass
A.k.a. a solutionSolute in a solvent (salt dissolved in water)
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Separating Mixtures Filtration – separates undissolved solids
from liquidsUsed to separate heterogeneous mixtures
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Separating Mixtures Distillation – separates a solution of liquids
or a homogeneous mixture
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Separating Mixtures Crystallization
Separates dissolved solids from liquids
Crystallization Demo & Explanation
Crystallization Demo
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Separating Mixtures Chromatography – separates components of a
solution into its components based on tendency to travel on another surface
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Elements
Elements – pure substance that cannot by separated into simpler substances by physical or chemical meansMade of only 1 type of atomAll elements are found on the Periodic Table
of ElementsEach has a unique name & symbol
Ex.) Carbon (C), oxygen (O), platinum (Pt)
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Elements All elements have a unique symbol
Each symbol is either 1 or 2 letters One letter = capitalized Two letters = first is capitalized, second is not
Symbols are often similar to the name but sometimes they are derived from the Latin name Ex.) Mercury’s symbol = Hg (from Latin hydrargyrum)
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Compounds Compound – combination of 2 or more
elements chemically bonded together or combinedWritten with a chemical formula
Letters indicate the elements in the compound Subscripts indicate the # of each type of atom in
the molecule
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Compounds The properties of a compound are VERY
DIFFERENT from the properties of the individual elements they contain
Ex.) Sodium Chloride (NaCl) vs. Sodium & Chlorine
Sodium: Sodium in Pond
Sodium in 40 Gallon Trashcan
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Compounds A molecule is the smallest particle of a
compound Compounds have constant composition
from one sample to another
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Matter
Mixtures Pure Substances
Heterogeneous
Homogeneous
Element
Compound
In Review…
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Classify the following as element, compound, heterogeneous mixture, or homogeneous mixture:
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Law of Definite Proportions
Elements in a compound combine in definite proportions by massAll samples of a compound have the same
proportion by mass of the elements present.
100compound of mass total
element of mass massby percent
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Example – Law of Definite Proportions
If 1.0 g of hydrogen reacts completely with 19.0 g of fluorine, what is the percent by mass of hydrogen in the compound that is formed?
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Example – Law of Definite Proportions
If you have a sample of sucrose (a type of sugar), you will always have 42.2% of carbon, 6.50% of hydrogen, and 51.30% of oxygen, no matter where you find that sample. Therefore, if you are given 50.0 g of sucrose, how many grams of each element will you have?
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Law of Multiple Proportions
When different compounds are formed by the combination of the same elements, they will combine in small whole number ratiosEx.) H2O & H2O2 ; CuCl & CuCl2 ; CO & CO2
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Properties of Matter
When talking about the properties of matter, there are two types:
PHYSICAL properties
OR
CHEMICAL properties
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Physical Properties of Matter
Characteristic that can be observed or measured without changing the sample’s composition (or identity)Ex.) color, boiling point, state of matter,
density
Physical properties describe appearance or behavior
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Physical Properties of Matter
Extensive propertyDepends on the amount of substance presentExamples:
Mass Length Volume
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Physical Properties of Matter
Intensive property Independent of the amount of substance
presentExamples:
Color Density Smell Boiling point
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Physical Properties of Matter
Intensive or Extensive?1. Phase
2. Size
3. Odor
4. Flammability
5. Energy
6. Melting point
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Chemical Properties of Matter
Chemical property – the ability of a substance to combine with or change into one or more other substances Examples: rusting, flammability, light sensitivity
2 H2O2 (l) 2 H2O (l) + O2 (g)
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Observing Properties of Matter
When recording physical or chemical changes, note the conditions. Many properties of substances can depend on temperature or pressure!
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Physical Changes
Physical changes – altering a substance without changing its identity or composition
Examples:CuttingBreakingPhase changes (evaporation, condensation,
sublimation, etc.)
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Chemical Changes
Chemical changes - one or more substance changes into a new substance i.e. a new substance is formed
Examples: burning, rotting, rusting
4 Fe + 3 O2 2 Fe2O3
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Evidence of a Chemical Change Properties of new substance formed does
not have the same properties as the original substance
Signs a chemical change has occurred:HeatCoolingFormation of bubbles (gas produced)Formation of solidsColor change
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Chemical or Physical Change?
1) Butter melting
2) Hot glass cracking when placed in cold water
3) Dissolving sugar in water
4) Burning sugar (like on crème brulee)
5) Wood rotting
6) Burning gasoline in your car
7) Silver tarnishing
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Weathering of the Earth – Chemical or Physical Changes?
Physical changes include:The splitting of rocks by freeze thaw cycles does
not change the make up of the rock
The cutting through and wearing away of softer rock by the actions of water
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Weathering of the Earth – Chemical or Physical Changes?
Chemical changes include:The dissolving of rock by slightly acidic waterLimestone easily dissolves in acidic water
When acidic water seeps through limestone and
some other minerals, it
dissolves some of the material and
takes it away.
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Conservation of Mass
Law of conservation of mass:Mass is not created or destroyed in a
chemical reaction (mass is conserved)
Mass products = mass reactants
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However, is mass conserved when a log burns in a fire??
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By observing a burning log turn to ash, you may be tempted to think that during the chemical change that occurred, some mass was lost. It was not!!!
If you gathered all of the gases that formed, soot that was carried away, and water that evaporated out when the log was hot, you would find that there is exactly the same amount of mass after the log was burned as before the log was burned
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Conservation of Mass Problems 68.5 grams of H2S contains 4.06 g of hydrogen
What mass of sulfur is in 68.5 grams of H2S?
What mass of hydrogen is in 200 grams of H2S?
What mass of sulfur is in 200 grams of H2S?