1. 20 Mrs. Leinweber

2. Chemistry 20 Introduction What is science? What is chemistry?

3. Scientific Process

4. Chemical Changes Physical changes produce no new substances. Chemical changes produce new substances.

5. Observations & Interpretations Qualitative observations involve descriptions. Quantitative observations involve measurements. What would be some examples of qualitative and quantitative observation when vinegar is added to baking soda?

6. Interpretations (Inferences) is an indirect form of knowledge that builds on a concept or an experience to further describe or explain an observation. What would be a quantitative observations when observing the light bulb? What would be a qualitative observation when observing the light bulb? What would be an interpretation when observing the light bulb? Observations & Interpretations

7. Classifying Knowledge Empirical knowledge is observable. Theoretical knowledge is not observable, it explains and describes observations in terms of ideas. Metals are shiny. Electrons occupy energy levels.

8. Classifying Matter

9. Electrolysis of Water Classifying Matter

10. Review what you just learned Check your Knowledge 1.Questions pg 11 #1-5, 7, 8 2.Questions pg 13 #1-5

11. The Periodic Table Elements Song

16. How It Is Put Together

17. What are the parts ?

19. How To Use It

20. Atomic Theories Electron Energy Levels

21. Atomic Theories

27. Metals lose electrons to become cations (sodium ion) Nonmetals gain electrons to become anions (chloride ion) Carbon, boron, silicon and noble gas generally do not form ions. Atoms and Ions

28. PRACTICE :)

30. Energy Diagrams

31. Review what you just learned Check your Knowledge Read pg 14-17 Questions pg 16 #1-6,8,9

32. Ionic Compounds

33. Oxide Oxygen I onic compounds are formed when metals lose electrons to non-metals and then are attracted to each other, forming an ionic bond. Example: Magnesium and oxygen. 12p+ 8p + Magnesium Electrons Ionic Compounds

34. All ionic compounds are solids at SATP and form conducting solutions.

35. Practice Writing Names & formulas Magnesium and fluorine Magnesium and oxygen Magnesium and nitrogen Potassium and bromine Potassium and sulfur Potassium and nitrogen Calcium and phosphorus Sodium and chlorine

36. Multivalent Ionic Compounds Many metals can form more than one ion, iron for example can form Fe 2+ and Fe 3+ ions.

37. Naming Multivalent Ionic Compounds Example #1 FeO (s) Fe 2 O 3(s) Example #2 SnF 4(s) SnF 2(s) Example #3 BiP (s) Bi 3 P 5(s) Example #4 Chromium(III) sulfide Example #5 Technetium(VII) nitride Example #6 Copper (II) Sulfate

38. Polyatomic Ionic Compounds Polyatomic ions are composed of two or more elements covalently bonded with an overall negative or positive charge.

39. Predicting Polyatomic Ionic Compounds Example #1sodium hydroxide Example #2potassium sulfate Example #3calcium nitrate Example #4iron(III) dichromate Example #5cupric phosphate

40. Predicting Polyatomic Ionic Compounds Example #6NH 4 Cl (s) Example #7Co(IO 3 ) 3(s) Example #8RuPO 4(s)

41. Ionic Hydrates Some ionic compounds exist as hydrates; have water molecules attached. Example:CuSO 4* 5H 2 O

42. Ionic Hydrates

43. Review what you just learned Check your Knowledge Questions pg 32 Q 3,4,5,15,16

44. Molecular Compounds and Elements

45. Molecular Elements and Compounds Molecular molecules are formed between two nonmetals due to a sharing of electrons. P+P+ P+P+ Both hydrogen atoms need an extra electron to complete their outer energy levels. Since neither is strong enough to steal an electron away they share valence electrons. Forming a covalent bond. hydrogen atom

46. Molecular Elements Many nonmetals are diatomic, others come in groups of three, four, or eight

47. Binary Molecular Compounds For hydrogen compounds such as hydrogen sulfide, H 2 S (g), common practice is not to use the prefix system. Memorize the following table:

48. Acids and Bases Acids are molecular hydrogen compounds whose solutions conduct electricity. Ionic bases contain the hydroxide ion. Nomenclature Notes and Examples

49. Review what you just learned Check your Knowledge Questions pg 36 Q 1-3 Check your Knowledge Questions pg 32 Q 3,4,5,15,16

50. Balancing Equations

54. Classifying Reactions Combustion Formation Decomposition

55. Classifying Reactions

56. Assignment 1. Section 2.5 pg 59-60 Q 1 - 6

57. Classifying Reactions Single Replacement Double Replacement

58. Classifying Reactions

60. SOLUBILITY A SOLUTION is a homogeneous mixture of a SOLUTE (substance dissolved) and a SOLVENT (substance dissolving, usually a liquid). SOLUBILITY is the maximum amount of a substance that can be dissolved at a specific temperature.

61. Assignment 1. Section 2.6 pg 64 Q 1 - 5

62. Chemical Amount

63. 1. Molar Mass (M) - 2. Mass (m) - 3. Moles (n) - A measure of the amount of matter in an object. Mass is usually measured in grams or kilograms. molar mass, M e the mass of one mole of a substance in units of grams per mole (g/mol) mole t the SI base unit for the chemical amount or amount of a substance, where one mole is the number of entities corresponding to Avogadro’s constant; unit symbol, mol molecular Chemical Amount

64. Determine the molar mass of: a. H 2 O b.CuSO 4. 5H 2 O c.Ca(NO 3 ) 2 d.Iron(III) sulfate

65. Chemical Amount Determine the chemical amount for: a.1500g of CaCO 3 b. 50.0g of sucrose

66. Chemical Amount Determine the mass for the following: a.2.50 mol of K 2 CrO 4 b.3.45 mmol of sodium sulfate

67. Assignment 1. Pg 53-54 Q1-5 2. Pg 57 Q1-3 & 5 & 6