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Honors Chemistry Chapter 2
Matter and Change
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Matter – anything that has mass and takes up space
Mass- amount of matter an object contains Materials – differ in type of matter they are composed of
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The Properties of Matter
Extensive properties – depend on the amount of matter that is present Example – volume, mass, amount of energy in the substance Intensive properties – do not depend on the amount of matter that is present Example – melting point, boiling point, density
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Substance – matter that is uniform and has a definite composition
All samples of an identical substance have the identical physical and chemical properties Physical property – quality or condition of a substance that can be observed or measured without changing the substance’s composition
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Properties of Matter When a substance undergoes a physical change, its physical appearance changes. Ice melts: a solid is converted into a liquid. Physical changes DO NOT result in a change of composition.
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Examples of Physical Properties
Color Odor Hardness Density Solubility Melting point, boiling point, freezing point Physical state – solid, liquid, gas
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Page 40 Table 2.1 Physical properties of some substances
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States of matter Solid (s) Liquid (l) Gas (g)
Plasma – we don’t deal with
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Classification of Matter
States of Matter Matter can be a gas, a liquid, or a solid. Gases have no fixed shape or volume. Gases can be compressed to form liquids. Liquids have no shape, but they do have a volume. Solids are rigid and have a definite shape and volume.
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Gas and vapor not the same
Gas – normally exists that way at room temperature Vapor – gas state of a substance that is normally a liquid or solid at room temperature
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Physical change A change which alters a material without changing its composition Cutting, grinding, melting, boiling, freezing, dissolving
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Physical and Chemical Changes
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Mixtures Physical blend of two or more substances Composition can vary
2 types: Heterogeneous Homogeneous
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Heterogeneous Mixture
Not uniform in composition Has 2 or more phases Phase – any part of a system with uniform composition and properties Dirt, salad, paper, rocky road ice cream
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Homogeneous Mixture Has a completely uniform composition
All components are evenly distributed Consists of a single phase Called a SOLUTION
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Solution – what do you think of?
Can be gas, liquid, or solid!!!!!
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Separating mixtures Use PHYSICAL methods Magnet, sifting,
Liquid mixtures – distillation Page 47
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Organic distillation Distillation
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Substances Can be elements or compounds Element – definition
Compound – 2 or more elements that have been CHEMICALLY combined. Can only be separated by CHEMICAL means
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Sugar + heat carbon + water
Water + electric current hydrogen + oxygen
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Properties of compounds
MUCH DIFFERENT THAN THE PROPERTIES OF THE ELEMENTS FROM WHICH THEY ARE COMPOSED!!!!! NaCl
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Flow chart – Pg. 50 Elements represented by symbols Compounds represented by formulas Pg. 52 Table 2.2
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Chemical Change A change that produces matter with a different composition than the original matter
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Properties of Matter When a substance changes its composition, it undergoes a chemical change: When pure hydrogen and pure oxygen react completely, they form pure water.
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Is iron transforming into rust a physical or chemical change
Does the substance change composition or just change appearance?
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The color of sulfur is yellow..
Physical Chemical Does the substance change composition or just change appearance?
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Dynamite explodes to form a mixture of gases
Physical Chemical Does the substance change composition or just change appearance?
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Aluminum melts at 933 K Physical Chemical
Does the substance change composition or just change appearance?
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Plants use CO2 to make sugar
Physical Chemical Does the substance change composition or just change appearance?
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Chemical Reactions One or more substances change into new substances
REACTANT(S) PRODUCT(S) means “change into”, “produce”, “yields”
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Chemical Property The ability of a substance to undergo chemical reactions and to form new substances Rusting, burning, fermenting, exploding, rotting, decomposing Iron and sulfur example
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Indications that a chemical reaction has occurred
Energy released or absorbed Color change Odor released Production of a gas Irreversibility Production of light
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Law of Conservation of Mass
During any chemical reaction, the mass of the products is always equal to the mass of the reactants.
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