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Matter
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Matter Stuff that objects are made of
Anything that has mass and volume 3 Types Elements Compounds Mixtures
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Phases of Matter Solids Liquids Gases Animation
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Solids Definite Shape and Volume Strong Intermolecular Forces
Particles are close together Particles are arranged in neat, orderly lines Particles do move – shake, vibrate Animation High melting and boiling points Designated by (s) Examples: Au(s), Fe(s) , H2O(s)
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Liquids Indefinite Shape Definite Volume
Midrange Intermolecular Forces Particles are somewhat close together Flow freely Designated by (l) Examples: Br(l), Hg(l), H2O(l)
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Gases NO definite Shape or Volume Weak Intermolecular Forces
Particles will spread out to fill the shape and volume of a container Weak Intermolecular Forces Particles are far apart Particles are very disorganized Particles quickly move all over Low melting and boiling points Designated by (g) Examples: Ne(g), O2(g) , H2O(g)
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Melting and Boiling Points
Use Reference Table S to find the melting and boiling points of a solid, a liquid, and a gas Element Melting Point Boiling Point
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Physical Properties Physical Changes
Characteristics that can be observed without changing the identity of the substance (no new substance is formed) Examples: Color, Hardness, melting point Physical Changes Changes that occur without changing the identity of the substance Examples: Cutting, Ripping, Phase Changes
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Physical/Chemical Change Song
Chemical Properties Characteristics that canNOT be observed without changing the identity of the substance (a new substance is formed) Examples: Reactivity, Flammability Chemical Changes A change that results in a new substance Examples: Burning, Rusting Physical/Chemical Change Song
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Physical/Chemical Examples
Indicate if each of the following is physical or chemical The boiling point of water is 100oC. Antacids will neutralize stomach acid. Diamonds will cut glass. Most metals conduct electricity. The density of NH3 is 0.77g/L. Solution A and B are reacted together and a precipitate (solid) is formed.
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Classification of Matter
All matter can be classified as one of the following: Elements Compounds Mixtures
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All matter can be described as:
Homogeneous – uniform throughout Heterogeneous – different throughout Classify the following as homogeneous or heterogeneous A glass of water Italian salad dressing Turkey and gravy Milk Orange juice with pulp Orange juice without pulp
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Substances Type of Matter – Element, Compound
All samples have identical properties and composition They are homogeneous
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Elements Composed entirely of atoms with the same atomic number
Cannot be decomposed Found on the Periodic Table Begin with a capital letter Homogeneous Examples: Cu, Fe, O2, Ne Diatomic Element = contains two of the same atoms (O2, H2)
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Compounds Composed of at least 2 different elements
Elements are chemically combined (bonded) Homogeneous
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Compounds Can be decomposed (by chemical means) into 2 or more elements Electrolysis, Reactions The properties of the component elements are usually very different from the properties of the compound Combined in a definite ratio In Sodium Chloride (NaCl) the Na and Cl must combine in a 1:1 ratio Examples: MgO, H2O, NaCl Binary Compound = contains 2 different elements
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Mixtures Combination of 2 or more substances
No chemical change occurs (No bond is formed)
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Mixtures Parts retain their individual properties
Can be separated by physical means Filtering, Magnetism, Distillation, Density Can combine in varying ratios The amount of salt in salt water can vary
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Mixtures Can be heterogeneous Can be homogeneous
Concrete, Dirt, Chocolate Chip Cookie Can be homogeneous Gases (Air) Aqueous Solutions – a solution made with water NaCl(aq) = salt is dissolved in water
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Law of Conservation of Matter
Matter cannot be created or destroyed
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Law of Conservation of Mass
Mass cannot be created or destroyed The mass before a reaction must be equal to the mass after the reaction
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Law of Conservation of Energy
Energy cannot be created or destroyed The amount of energy remains constant, however it may transfer forms
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