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Chapter 3

Chapter 3. Matter – Properties and Change. Vocabulary. pure substance states of matter solid liquid gas vapor plasma physical properties chemical properties extensive property intensive property physical change chemical change evidence of chemical reaction

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Chapter 3

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  1. Chapter 3 Matter – Properties and Change

  2. Vocabulary pure substance states of matter solid liquid gas vapor plasma physical properties chemical properties extensive property intensive property physical change chemical change evidence of chemical reaction Law of Conservation of Mass mixture heterogeneous homogeneous solution alloy filtration distillation crystallization chromatography element compound Law of Definite Proportions Law of Multiple Proportions

  3. 3.1 States of Matter • Pure substance – matter with a uniform and unchanging composition • NaCl • H20 • Tap water

  4. States of Matter

  5. Solids • Definite shape • Definite volume • Particles tightly packed • Incompressible -

  6. Liquid • Indefinite shape – • Definite volume • Can flow • Less closely packed • Can move past one another • incompressible

  7. Gas • Indefinite shape • Indefinite volume – • Flows • Very far apart • Easily compressed • Vapor -

  8. Plasma • Particles have electric charges • Can conduct electricity

  9. 3.2 Physical & Chemical Properties and Changes

  10. Physical Properties • Characteristic that can be observed or measured without changing the samples composition • Color • Odor • Melting point • Boiling point • Density

  11. Extensive properties – depends on amount of substance present • Ex: • Intensive properties – do not depend on amount of substance • Ex:

  12. Chemical Properties • The ability of a substance to combine with or change into one or more other substances • Magic word: • Examples: • Burning • Iron rusting • Inert gasses

  13. Physical vs. Chemical Properties of Cu

  14. Changes in Matter

  15. Physical Changes • Alters a substance without changing its composition • Ex:

  16. Phase change – PHYSICAL CHANGE • Examples: • Boiling • Freezing • Condensing • Vaporizing • melting

  17. Chemical Changes • One or more substances changing into new substances • Chemical reactions • New substances have different composition & properties • Decompose, explode, rust, oxidize, corrode, burn

  18. Evidence of chemical reactions • Transfer of energy (heat/light) • Change in color • Formation of a gas (bubbles) • Formation of a precipitate (solid forms from 2 liquids)

  19. KI + AgNO3 KNO3 + AgI

  20. Law of Conservation of Mass • Mass is neither created nor destroyed during a chemical reaction, it is conserved • Mass of reactants = mass of products

  21. 22.99 g of sodium with 35.45 g of chlorine, what mass of sodium chloride is produced? • In an experiment, 10.00 g of mercury (II) oxide is heated until it is converted to liquid mercury and oxygen gas. The liquid mercury has a mass of 9.26 g. What mass of oxygen was formed?

  22. 3.3 Mixtures of Matter • Mixture = combination of 2 or more pure substances in which each pure substance retains its original chemical properties • Most everyday matter occurs as mixtures

  23. Heterogeneous mixture • Composition not uniform • Not evenly mixed • Not the same throughout • Examples:

  24. Homogeneous mixture • Constant composition throughout • Every sample is the same

  25. Solution – a type of homogeneous mixture • Solute • Solvent • Ex: Carbon dioxide dissolved in pop

  26. Alloy – a homogeneous mixture of metals or of a metal and nonmetal • Examples • Brass • Steel • Gold jewelry

  27. Separating Mixtures • PHYSICAL CHANGE • Based on the differences in physical properties of substances

  28. Filtration – uses a porous barrier to separate a solid from a liquid

  29. Distillation – separates 2 things with different boiling points

  30. Crystallization – formation of pure solid particles of a substance from a solution containing the dissolved substance

  31. Chromatography – separates the parts of a mixture based on the ability of each part to travel across the surface of another material

  32. 3.4 Elements & Compounds • Element – pure substance that cannot be separated into simpler substances • Earth = 92 natural elements • Not equally abundant

  33. Compounds – made up of two or more elements that are chemically combined • Represented by chemical formulas • NaCl • H2O • CO2

  34. Separating compounds – chemical process • Compounds that occur naturally are hard to separate because they are very stable

  35. Properties of a compound are different from the properties of the elements that make it up • Hydrogen & oxygen vs. water

  36. Law of Definite Proportions • A compound is always composed of the same elements in the same proportion by mass, regardless of size of the sample

  37. Percent by mass = ratio of the mass of each element to the total mass of the compound

  38. 1.0 g of hydrogen reacts with 19.0 g of fluorine, what is the percent by mass of each element in the resulting compound: HF?

  39. Law of Multiple Proportions • When different compounds are formed by a combination of the same elements, different masses of one element combine with fixed mass of the other element in a ratio of small whole numbers • CO vs CO2

  40. What is the correct formula for sample 3? Gas Samples Sample Volume of Nitrogen (L) Volume of Oxygen (L) 1 2.00 3.02 2 1.01 1.99 3 1.98 4.99 4 1.98 1.02

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