matter and change 2.1 properties of matter 2.2 mixtures 2.3 elements and compounds 2.4 chemical...
TRANSCRIPT
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Matter and Change2.1 Properties of Matter2.2 Mixtures2.3 Elements and Compounds2.4 Chemical Reactions
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2.1 Properties of Matter
Objectives: Identify properties of matter as extensive and intensive Define physical and chemical properties Differentiate between the 3 states of matter
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KEY TERMS
Mass
Volume
Extensive Property
Intensive Property
Substance
Physical Property
Solid
Liquid
Gas
Vapor
Physical Change
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DefinitionsMass (m) – the amount of matter an object contains (a numerical value of its inertia)Volume(V) – the amount of space an object occupiesExtensive property - a property that depends on the amount of matter an object containsIntensiveproperty – a property that depends on type of matter an object containsSubstance – matter with uniform propertiesPhysicalproperty - a quality or condition of a substance that can be observed without changing the composition of the substanceChemicalproperty – a quality or condition of a substance that can be observed with changing the composition of the substancePhysical change - a change that do not affect the composition of a substanceChemicalchange – a change that does affect the composition of a substance
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Some Criteria for the Classification of Matter
Properties
State (solid, liquid, gas)
Composition
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Intensive and Extensive Properties
Sulfur
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Examples of Physical Properties
Color, odor, hardness, density, melting point, boiling point, state, solubility.
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Substance State Color Melting
Point (C°)
Boiling Point (C°)
Density (g/cm3)
Oxygen O2 Gas Colorless -218 -183 0.0014
Mercury Hg Liquid Silvery-white
-39 357 13.5
Bromine Br2 Liquid Red-brown -7 59 3.12
Water H2O Liquid Colorless 0 100 1.00
Sodium Chloride
NaCl Solid White 801 1413 2.17
Example: Physical Properties
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States of Matter
Solid fixed shape and volume,
incompressibleLiquid
fixed volume, takes the shape of its container
Gastakes the volume and shape of
its container
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Solid Liquid Gas
http://www.chem.purdue.edu/gchelp/atoms/states.html
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Bromine
Gas (Vapor)
Liquid
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Change of Phase
Melting solid liquidCondensation gas liquid
Freezing liquid solid
Evaporation liquid gasSublimation solid gas
Boiling: Evaporation occurring beneath the liquid’s surface.
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Is changing phase a physical or chemical change?
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Classification of Matter(by composition)
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(Pure) Substance
Matter that has a uniform and definite composition.
Elements
Compounds
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2.2 MIXTURES
Objectives: Categorize samples of matter into substance or mixture Differentiate between homogeneous and heterogeneous Describe two ways that components of mixtures can be
separated
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KEY TERMS Mixture - physical blend of 2 or more substances Heterogeneous – mixture in which the composition is not uniform
throughout Homogeneous – mixture with a uniform composition throughout Phase – a part of a mixture with uniform composition Solution – another name for homogeneous mixture Filtration - a process that separates a solid from a liquid Distillation - a process that separates a solid dissolved in a liquid/
separation of 2 miscible liquids with different boiling
temperatures Miscible - 2 or more liquids that can form a homogeneous mixture
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MixtureA physical blend of two or more
substances.
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Copper II Sulfate and its solution in water.
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Example: Stainless Steel
A homogeneous mixture of:
-Iron (Fe)
-Chromium (Cr)
-Nickel (Ni)
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Example: Gaseous Mixture
Elements argon and nitrogen and a compound (water vapor).
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Heterogeneous Mixtures
Non-uniform composition throughout the mixture
Two or more phases.
Example:
Oil and vinegar
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Note:
Mixtures can be physically separated.
Mixtures exhibit physical properties similar to the components of the mixture.
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Separation Methods
Use differences in the physical properties of the components of the mixture.
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Example: Separate iron filings from sulfur using a magnet.
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Filtration: separates a solid from a liquid in a heterogeneous mixture
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Distillation: -separate dissolved solids from a liquid -uses boiling and condensation.
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Distillation of Crude Oil (Refining)
Crude Oil is a mixture of Hydrocarbons
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Distillation of Crude Oil
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c) Elements and Compounds
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ElementsThe simplest substances.Can not be separated into simpler
substances.Building blocks of all matter. More than 100 known elements.Represented by chemical
symbols.
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Chemical Symbols of Elements
System started by Jons Berzelius (Sweden, 1779-1848)
One or two first letters of name of the element.
Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.
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Examples:
Americium, Am
Einsteinium, Es
Bromine, Br
Helium, He
Lead(Plumbum), Pb
Niobium, Nb
Iron (Ferrum), Fe
Mendelevium, Md
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CompoundA substance that contains two or more
elements chemically combined.
Compounds have different properties from the individual substances.
(Ex: H2O)
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Example: H2O
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Substance or mixture?
If composition is fixed and may not changesubstance
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d) Chemical Properties and Chemical Changes
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H2O composition is fixed- compound
Gaseous Phase Liquid Phase
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Chemical Properties
The ability of a substance to transform into a new substance (to undergo a chemical change).
Example: Magnesium reacts with oxygen to form magnesium
oxide.
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Magnesium Mg
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Burning of Magnesium2Mg+ O2 2MgO
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Physical ChangesPhysical change: a change in the
physical properties of a substance.
Composition does not change.
May be reversible or irreversible.Examples:
Reversible:Irreversible:
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Chemical Change
A change that produces matter with a different composition than the original matter.
Atoms rearrange themselves into new combinations.
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Burning of MethaneCH4 +2O2 CO2 + 2H2O
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Burning of MethaneCH4 + 2O2 CO2 + 2H2O
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Recognizing a Chemical Change
energy exchange production of a gascolor changeformation of a precipitate
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Formation of a Precipitate
Cu(OH)2
Precipitate
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The Law of Conservation of Mass (Antoine Lavoisier)
In any chemical or physical change, mass is neither created or destroyed
Mass is CONSTANT