1. PLC-Unit 1B Unit 1B Matter Properties & Changes

2. PLC-Unit 1B Section I Classification of Matter

3. PLC-Unit 1B

4. A. Mixture 1)DEF: a combination of two or more substances in which the basic identity of each substance is not changed NaCl+H2OH2O = Salt water Pure substance+ = Mixture 2)can be separated by physical means 3)retains its own properties 4)can be classified as heterogeneous or homogeneous

5. PLC-Unit 1B 1)DEF: a mixture that does not have a uniform composition and in which the individual substances remain distinct 2)can see individual substances (phases) Heterogeneous Mixture granitesaladbanana split

6. PLC-Unit 1B 1)DEF: a mixture that has a uniform composition throughout and always has a single phase 2)also called a solution steel Saline solution pure air Homogeneous Mixture

7. PLC-Unit 1B 3)Consists of two (2) parts solute – DEF: the substance that is being dissolved solvent – DEF: the substance that dissolves the solute salt water - salt (solute), water (solvent) 4)Aqueous solution (aq) DEF: solvent is water universal solvent

8. PLC-Unit 1B 5)can be solid, liquid, or gas G-GAir G-LCarbonated beverage S-SSteel (iron & carbon), alloy S-LSalt water L-LVinegar L-GWater vapor

9. PLC-Unit 1B 1)Filtration DEF: a technique that uses a porous barrier (filter paper) to separate a solid from a liquid sand and water Separating Mixtures

10. PLC-Unit 1B 2)Based on unique physical properties Magnetism – can separate a sand-iron mixture

11. PLC-Unit 1B 3)Sieve DEF: a technique that uses a screen with different pore sizes that separate solids of different sizes sand and rocks

12. PLC-Unit 1B 4)Evaporation DEF: a technique that removes the liquid from a solution, usually to leave a solid salt and water

13. PLC-Unit 1B 5)Distillation DEF: a technique that is based on differences in the boiling points of the substances involved alcohol (bp = 80 o C) and water (bp = 100 o C)

14. PLC-Unit 1B 6)Chromatography DEF: technique that separates the components of a mixture on the basis of the tendency of each to travel or be drawn across the surface of another material colors in ink

15. PLC-Unit 1B B. Pure Substances 1)DEF: matter with the same fixed composition and properties 2)two (2) types of Pure Substances Elements Compounds

16. PLC-Unit 1B 1)DEF: a substance that cannot be broken down into simpler substances 2)Building block of all matter 3)composed of one type of atom (EX: copper) 4)only 92 elements occur naturally on earth Elements

17. PLC-Unit 1B 1)Periodic Table DEF: a chart that organizes all known elements into horizontal rows (periods) and vertical columns (groups or families) 2)Each element has a unique chemical name and symbol Chemical name (named after) people (Einsteinium) countries (Germanium) states (Californium) mythological figures (Plutonium) Latin name (Iron-ferrum [Fe]) Organizing the Elements

18. PLC-Unit 1B Symbol contains 1,2 or 3 letters 1st letter is capitalized; others are lower case K (Potassium) Na (Sodium) Uun (Ununnilium)

19. PLC-Unit 1B 1)DEF: a chemical combination of two or more elements joined together in a fixed proportion 2)can be broken down into simpler substances by chemical means EXAMPLE: water (H 2 O), salt (NaCl), sugar (C 6 H 12 O 6 ) 3)Has properties that are different from those of its elements Compounds

20. PLC-Unit 1B 4)Formula DEF: combination of the chemical symbols that show what elements make up a compound and the number of atoms of each element EXAMPLE: C 12 H 22 O 11 12 atoms carbon 22 atoms hydrogen 11 atoms oxygen

21. PLC-Unit 1B 1)DEF: states that, regardless of the amount, a compound is always composed of the same elements in the same proportions by mass H2OH2O2 H1 O NaCl1 Na1 Cl 2)Percent by mass (%) % by mass=Mass of elementx100 Mass of compound Law of Definite Proportions

22. PLC-Unit 1B % by mass=Mass of elementx100 Mass of compound Percent by Mass A 78.0 g sample of an unknown compound contains 12.4 g of hydrogen. What is the percent by mass of hydrogen in the compound? % Hydrogen=12.4 gx100 78.0 g 15.9%

23. PLC-Unit 1B Percent by Mass What is the percent by mass of carbon in glucose (C 6 H 12 O 6 )? % Carbon=72 gx100 180 g 40.0% C=6x12 g= 72 g H=12x1 g= 12 g O=6x16 g= 96 g 180 g (mass of compound)

24. PLC-Unit 1B 1)DEF: states that when different compounds are formed by the combination of the same elements, they combine in small-whole number ratios Law of Multiple Proportions

25. PLC-Unit 1B Section II Properties and Changes of Matter

26. PLC-Unit 1B A. Physical Properties 1)DEF: characteristics of a sample of matter that can be observed or measured without any change in its identity EXAMPLE: color, electrical conductivity, boiling point, melting point, density, state of matter (solid, liquid, or gas)

27. PLC-Unit 1B 1)DEF: physical forms of matter 2)Four (4) states of matter Solid Liquid Gas Plasma 3)state of matter is based upon: particle arrangement energy of particles distance between particles States of Matter

28. PLC-Unit 1B 1)DEF: a form of matter that has a definite shape and definite volume 2)particles vibrate in place SOLID

29. PLC-Unit 1B 1)DEF: a form of matter that has a definite volume but takes the shape of its container 2)particles vibrate in place are able to slip past each other which allows liquid to flow LIQUID

30. PLC-Unit 1B 1)DEF: a form of matter that has no definite shape and no definite volume; takes the shape of its container 2)Particles are far apart and constantly moving 3)Gas vs. Vapor Gas – a substance that is naturally in the gaseous state at room temperature EXAMPLE: Helium GAS

31. PLC-Unit 1B Vapor – the gaseous state of a substance that is a solid or liquid at room temperature EXAMPLE: Steam

32. PLC-Unit 1B PLASMA 1)DEF: a form of matter that does not have a definite shape or volume and whose particles have broken apart 2)composed of electrons and positively charged ions 3)conducts an electric current (gases do not) 4)affected by electric and magnetic fields which is used to contain plasma (gases are not)

33. PLC-Unit 1B 5)Artificial plasma – created by passing electric current through gases EXAMPLE: fluorescent lights, plasma TV

34. PLC-Unit 1B STATES OF MATTER SOLID LIQUID GAS PLASMA Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

35. PLC-Unit 1B B. Chemical Properties 1)DEF: a property that can be observed only when there is a change in the composition of a substance 2)Describes the ability or inability of a substance to react with other substances or to decompose EXAMPLE: ability to rust, unreactive, flammable

36. PLC-Unit 1B C. Physical Change 1)DEF: a change in matter that does not involve a change in the identity of the substance 2)same substance remains after change EXAMPLE: change of state, dissolving

37. PLC-Unit 1B Melting is an example of a reversible change. For example, when chocolate is warmed until it melts, the melted chocolate can be changed back into solid chocolate by cooling.

38. PLC-Unit 1B D. Chemical Change 1)DEF: the change of one or more substances into other substances 2)also called a chemical reaction 3)evidence of a chemical change precipitate gas formation color change energy change Odor

39. PLC-Unit 1B 4)Law of Conservation of Mass (LOCOM) DEF: matter is neither created nor destroyed during a chemical reaction Mass reactant = Mass product

40. PLC-Unit 1B Law of Conservation of Mass From a laboratory process a student collected 10.0 g hydrogen and 79.4 of oxygen. How much water was originally involved? 89.4 g Mass reactant = Mass product Mass water = Mass hydrogen + Mass oxygen Mass water = 10.0 g + 79.4 g

41. PLC-Unit 1B Law of Conservation of Mass A 10.0-g sample of magnesium reacts with oxygen to form 16.6 g of magnesium oxide. How many grams of oxygen reacted? 6.6 g Mass reactant = Mass product Mass magnesium + Mass oxygen = Mass MgO 10.0 g + Mass oxygen = 16.6 g

42. PLC-Unit 1B DEF: capacity to do work all physical and chemical changes require energy can be exothermic or endothermic Energy

43. PLC-Unit 1B DEF: chemical reaction that gives off heat energy EXAMPLE: burning wood in a fireplace Exothermic

44. PLC-Unit 1B DEF: chemical reaction that absorbs heat energy EXAMPLE: photosynthesis absorbs light energy from sun and produces sugars from carbon dioxide and water Endothermic