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Chapter 3 Matter & Its Properties
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Volume and Mass Volume: amount of 3-D space an object occupies; all matter has volume Mass: measure of the amount of matter; measure with a balance
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Matter Matter: anything that has mass and takes up space
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Basic Building Blocks of Matter Atom: smallest unit of an element that maintains the properties of that element C C C Carbon Atoms
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Elements Element: pure substance made of only 1 kind of atom Carbon Oxygen DIATOMIC MONATOMIC
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Compound Compound: substance made from the atoms of two or more elements chemically bonded Water
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Properties Chemists use properties to distinguish between substances and to separate them.
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Properties Entire group of substances: example – metals’ distinguishing property is conductivity Unknown substance conducts electricity well – probably a metal
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Properties Subgroups of substances: Sugars can be reducing or nonreducing Something called Fehling’s solution can be used to test the sugar
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Extensive Properties Depend on the amount of substance present Examples: mass, volume, amount of energy in a substance
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Intensive Properties Do not depend on the amount of matter present (independent) Examples: melting point, boiling point, density, ability to conduct electricity and heat
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Intensive vs. Extensive Imagine heating 100 mL and 400 mL of water, respectively Boiling point? Heat absorbed? Time to boil?
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Physical Property Physical Property: characteristic can be observed or measured without changing the identity of the substance Example: melting or boiling point; color, size, etc.
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Physical Change Physical Change: change in a substance that does not involve a change in the identity of the substance Example: grinding, cutting, melting, etc.
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Special Physical Changes: CHANGES OF STATE Changes of State: special physical changes in which a substance changes from one state to another The 3 common states are solid, liquid, and gas
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SOLID Solid: 1. definite volume and shape 2. particles packed together in fixed positions 3. particles vibrate about a fixed position
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LIQUID Liquid: 1. definite volume but indefinite shape 2. takes shape of container 3. particles close but flow around one another
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GAS Gas: 1. no definite shape or volume 2. particles a great distance from each other
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SOLIDS, LIQUIDS, & GASES
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Change of State Processes Solid to Liquid: Liquid to Gas: Gas to Liquid: Liquid to Solid: Solid to Gas: Gas to Solid:
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Chemical Property Chemical property relates to a substance’s ability to undergo changes that transform it into different substances Ex: iron rusting, silver tarnishing, match burning, etc.
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Chemical Change/Reaction Chemical change or chemical reaction: change in which one or more substances are converted into different substances
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Chemical Equations Reactants: substances that react in a chemical change (left side of chemical equation) Products: substances that are formed in a chemical change (right side of chemical equation) Reactants Products
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Law of Conservation of Matter (Add this to outline) In a chemical reaction, matter cannot be lost nor gained. Matter may rearrange but cannot be created nor destroyed. Mass of reactants = mass of products
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Evidence of chemical change (Add this to outline) Ideas?
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Energy and Changes in Matter Energy is involved in both physical and chemical changes. Different forms include heat and light.
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Energy Uses include: 1. provide energy for a physical change (i.e. melting) 2. provide energy for a chemical change (i.e. decomposition of water)
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Energy Energy in physical and chemical changes may be released or absorbed, but it is not created or destroyed! Law of Conservation of Energy
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Classification of Matter All matter can be classified as: 1. pure substances OR 2. mixtures
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Mixtures Mixtures: (def.) blend of two or more kinds of matter, each of which retains its own properties and identity
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Mixtures Properties of a Mixture: are a combination of the properties of its components Composition of a Mixture: must be specified (in a % of mass or volume)
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Homogeneous v. Heterogeneous Homogeneous: uniform in composition; same proportion of components throughout (ex. Salt water solution) Heterogeneous: not uniform throughout (ex. Mixture of clay and water)
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Separating Mixtures 1. Filtration 2. Paper Chromatography 3. Centrifuge
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Pure Substances Pure substances: (def.) has a fixed composition and differs from a mixture in the following ways:
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Pure Substances 1. Every sample of a given pure substance has exactly the same characteristic properties (unlike mixtures whose properties depend upon the relative amounts of mixture’s components)
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Pure Substances 2. Every sample of a given pure substance has exactly the same composition Ex. All pure water is always 11.2% H and 88.8% O by mass.
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Pure Substance Examples Water Sucrose Pure substances are compounds or elements
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Laboratory Chemicals and Purity Chemicals in lab treated like pure chemicals BUT all have some impurities Impurities can sometimes affect the results of a reaction
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The End of Section 1-2!!!!!
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