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Matter and Change: Properties, Phases, and Separation Methods

This chapter discusses the different phases of matter, physical and chemical properties, separation methods for mixtures, and the classification of matter into elements, compounds, and mixtures.

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Matter and Change: Properties, Phases, and Separation Methods

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  1. Chapter 3“Matter and Change”

  2. Matter • Matter is anything that has mass, and takes up space

  3. Copper Phases - Solid

  4. Copper Phases - Liquid

  5. Copper Phases – Vapor (gas)

  6. definite indefinite indefinite definite indefinite definite compact Spread Out Loosely Spaced

  7. 4th state:Plasma - formed at high temperatures; ionized phase of matter as found in the sun

  8. Properties are… • Physical Properties- a property that can be observed and measured without changing the material’s composition.

  9. Condense Freeze Evaporate Melt Gas Liquid Solid

  10. Chemical Properties- a property that can only be observed by changing the composition of the material. • Examples- ability to burn, decompose, ferment, react with, etc.

  11. Physical vs. Chemical Change • Physical change will change the appearance, without changing the composition of the material. • Boil, melt, freeze, cut, bend, split, crack • Can be reversible, or just changes shape • Chemical change - a change where a new substance is produced and is not reversible • Rust (iron oxidation), burn, decompose, ferment, explode, tarnish (silver oxidation)

  12. Quiz Time • Which of the following are physical changes. • A. making caramel from sugar • B. Carving a wooden figurine • C. Freezing mercury • D. Dissolving salt in water • Classify each of the following as a substance or a mixture. • A. silver • B. alphabet soup • C. Textbook • D. Table salt (sodium chloride)

  13. Evidence of a chemical reaction • Product is different than reactants • Ex: • Color change • Temperature change • Gas Produced (bubbles) • Light produced

  14. Law of Conservation of Mass • “Mass is neither created or destroyed” • Mass of the reactants (the stuff being put into the reaction) must equal the mass of the products (the stuff made once the reaction has taken place). • Reactants Products Mass = Mass

  15. Law of conservation of mass • Example: A 5 g sample of A reacts with a B to form 25 g of AB. What was the mass of B that reacted?

  16. Law of Conservation • 8 g of hydrogen react completely with 64 g of oxygen, how much water is produced?

  17. Elements, Mixtures, and Compounds • EQ: How is matter separated?

  18. Element: Simplest form of matter that has a unique set of properties

  19. Compound: A substance that contains two or more elements chemically combined or more elements chemically combined in a fixed proportion.

  20. Mixture: A physical blend of two or more substances.

  21. Homogeneous Mixture: A mixture in which the composition is uniform throughout. Another name for a homogeneous mixture is solution.

  22. Heterogeneous Mixture: A mixture in which the composition in not uniform throughout.

  23. Separating Mixtures Differences in physical properties can be used to separate mixtures. In our chemistry class we will examine filtration, distillation and evaporation.

  24. Physical Sorting • Separates Large solids using your hands

  25. Magnetic • Separates magnetic metals like iron using a magnet

  26. Filtration: The process of separating a solid from a liquid using a filter.

  27. Paper Chromatography Pigments are separated from liquid using paper.

  28. Distillation: Liquids can be separated based on their differences in boiling point

  29. Crystalizaion: Separates solids from liquids using evaporation.

  30. Breaking down compounds: Involves a chemical change. Heating is one of the processes used to break down compounds into simpler substances.

  31. Mixtures are a physical blend of at least two substances; have variable composition. They can be either: • Heterogeneous – the mixture is not uniform in composition • Chocolate chip cookie, gravel, soil. • Homogeneous - same composition throughout; called “solutions” • Kool-aid, air, salt water • Every part keeps it’s own properties.

  32. Separating Mixtures • Some can be separated easily by physical means: rocks and marbles, iron filings and sulfur (use magnet) • Filtration - separates a solid from the liquid in a heterogeneous mixture (by size)

  33. Separation of a Mixture Distillation:takes advantage of different boiling points.

  34. Made of one kind of material Made of more than one kind of material Made by a chemical change Made by a physical change Definite composition Variable composition Compound or Mixture? Compound Mixture

  35. Element Compound Mixture Which is it?

  36. Elements vs. Compounds • Compounds can be broken down into simpler substances by chemical means, but elements cannot. • A “chemical change” is a change that produces matter with a different composition than the original matter.

  37. Classification of Matter

  38. Symbols & Formulas • An element’s first letter always capitalized; if there is a second letter, it is written lowercase: B, Ba, C, Ca, H, He

  39. Chemical Changes • The ability of a substance to undergo a specific chemical change is called a chemical property. • iron plus oxygen forms rust, so the ability to rust is a chemical property of iron • During a chemical change (also called chemical reaction), the composition of matter always changes.

  40. Chemical Reactions are… • When one or more substances are changed into new substances. • Reactants- the stuff you start with • Products- what you make • The products will have NEW PROPERTIES different from the reactants you started with • Arrow points from the reactants to the new products

  41. Recognizing Chemical Changes • Energy is absorbed or released (temperature changes hotter or colder) • Color changes • Gas production (bubbling, fizzing, or odor change; smoke) • formation of aprecipitate- a solid that separates from solution (won’t dissolve) • Irreversibility- not easily reversed But, there are examples of these that are not chemical – boiling water bubbles, etc.

  42. Conservation of Mass • During any chemical reaction, the mass of the products is always equal to the mass of the reactants. • All the mass can be accounted for: • Burning of wood results in products that appear to have less mass as ashes; where is the rest? • Law of conservation of mass

  43. - Page 55 43.43 g Original mass = 43.43 g Final mass reactants = product

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