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Matter – Properties and Changes

Matter – Properties and Changes. Properties of Matter Changes of Matter Mixtures of Matter Elements and Compounds. PROPERTIES OF MATTER Types of Properties. Physical Properties - properties that can be observed and measured without changing the composition

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Matter – Properties and Changes

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  1. Matter – Properties and Changes Properties of Matter Changes of Matter Mixtures of Matter Elements and Compounds

  2. PROPERTIES OF MATTERTypes of Properties Physical Properties - properties that can be observed and measured without changing the composition examples – color, texture, hardness) types of physical properties 1) intensive - do not depend upon amount of the substance 2) extensive - depend upon amount of the substance

  3. Properties- Physical • Examples: length color mass volume density phase conductivity texture

  4. Properties Phases • A physical property Solid – particles very close together particles vibrate in a fixed position

  5. Properties- Phases Liquid – particles are intermediate in distance particles glide past each other

  6. PropertiesPhases Gas – particles are far apart particles are separated from eachother particles move quickly STOP

  7. PROPERTIES OF MATTERTypes of Properties Chemical Properties - properties relating to the ability of substances to combine with or change into other substance (has a uniform and unchanging composition) examples 1) reaction with water 2) ability to combine with oxygen 3) reaction with acids

  8. Properties- Chemical • Describes ability of substance to change into another substance • Examples: rust, burn, bubbles, precipitate

  9. Changes Physical

  10. CHANGES IN MATTERTypes of Changes 1. physical - changes in which a substance is altered without changing composition a. examples- phase changes, cut into pieces 2. chemical - changes in which one or more substances change into new substances with new properties a. reactants – substances that react b. products - substances that are produced

  11. Changes Chemical • Changes that result in a new substance • a.k.a chemical reaction Word equation: hydrogen + oxygen water reactants product copper + silver nitratesilver + copper nitrate reactants product

  12. Changes Chemical Formula Equation Cu + 2AgNO3 Cu(NO3)2 + 2Ag Pb(NO3)2 + 2KI  PbI2 + 2KNO3 (be able to identify reactants and products)

  13. Chemical changes Examples of chemical changes 1) digestion of food 2) burning (combustion) 3) fermentation 4) rusting 5) tarnishing of silver

  14. CHANGES IN MATTER Evidence of Chemical Changes 1. change in color and/or appearance 2. change in energy 3. change in odor 4) formation of a precipitate or a gas

  15. Energy changes related to chemical changes (reactions) • exothermic - energy is released (given off in the form of heat or light) - burning, explosion • endothermic - energy must be continuously added to keep the reaction going - electrolysis of water or salt

  16. MIXTURES A. Definitionof Mixture - combination of pure substances that retain their properties B. Types of Mixtures 1. heterogeneous - individual substances are distinct (composition is not uniform throughout) a. examples – sand, vegetable soup 2. homogeneous - individual substances are not distinct (uniform composition throughout) a. examples - solutions

  17. MIXTURES Types – homogeneous __________________________________________________________________________________________________________ type of solution examples __________________________________________________________________________________________________________ solid – liquid sugar water, salt water ___________________________________________ gas – liquid carbonated beverages ________________________________________________________ liquid – liquid alcohol, vinegar ________________________________________________________ gas – gas air _______________________________________________________ solid - solid alloys (metal + metal) ________________________________________________________

  18. MIXTURES Separating Mixtures 1. Filtration 2. Distillation 3. Crystallization 4. Chromatography

  19. ELEMENTS AND COMPOUNDSElement-a pure substance that cannot be broken down by simple means The periodic table organizes the 91 naturally occurring elements and scientifically created elements • A. Mendeleev created the original periodic table.

  20. ELEMENTS AND COMPOUNDSCompounds definition - a compound is a pure substance that is the combination of two or more different elements ie: NaCl – table salt Na- combustible solid and Cl – poisonous gas examples of compounds a. sodium bicarbonate NaHCO3 b. hydrochloric acid HCl c. sulfur dioxide SO2

  21. ELEMENTS AND COMPOUNDSCompounds examples of formation of compounds from elements (synthesis reactions) a. 2 Na + Cl2 -----> 2 NaCl b. 2 H2 + O2 ------> 2 H2O c. N2 + 3H2 ------> 2NH3

  22. ELEMENTS AND COMPOUNDSCompounds examples of decomposition of compounds to form elements a. 2NaCl  2Na + Cl2 b. 2 H2O  2H2 + O2

  23. The organization of Matter

  24. PURE SUBSTANCE MIXTURE yes no yes no Is the composition uniform? Can it be decomposed by chemical means? Matter Flowchart MATTER yes no Can it be separated by physicalmeans? Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element

  25. The Law Conservation of Mass States that mass can neither be created nor destroyed. Mass of reactants = mass of products 28 g of Na + 28 g of Cl = 56 g of NaCl

  26. Law of Conservation of Mass and chemical changes- Mass reactants = Mass products (mass is neither created nor destroyed in chemical reactions) Lavoisier (1743 - 1794) experiment [ 216 g of HgO --> 200 g Hg + 16g O2 ] 216 grams of mercury oxide when heated will produce 200 grams of mercury and 16 grams of oxygen

  27. Law of Definite Proportions 1.Definition - a compound is always composed of the same elements in the same proportions by mass 2. examples a. water- H2O (always has a ratio of 1 gram of hydrogen to 8 grams of oxygen) b. ammonia - NH3 (always combine in a ratio of 14 grams of nitrogen to 3 grams of hydrogen)

  28. Law of Multiple Proportions 1. definition - when different compounds are formed by a combination of the same elements, different masses of one element will combine with the same relative mass of the other element in a ratio of small whole numbers

  29. Law of Multiple Proportions WATER (H2O) 2 grams of hydrogen combine with 16 grams of oxygen PEROXIDE (H2O2) 2 grams of hydrogen combine with 32 grams of oxygen The ratio that compares the amount of oxygen in water and peroxide is 1:2

  30. Law of Multiple Proportions SULFUR DIOXIDE (SO2) 32 grams of sulfur combine with 32 grams of oxygen SULFUR TRIOXIDE (SO3) 32 grams of sulfur combine with 48 grams of oxygen The ratio that compares the amount of oxygen in sulfur dioxide and sulfur trioxide is 2:3

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