2. Aug. 14 th 2013Wednesday – #1 Chemsitry Aug. 14 th 2013Wednesday – #1 Chemsitry Objective: Understand the safety expectations in a chemistry lab/classroom environment

3. Aug. 16 th 2013 #2 Chemsitry Aug. 16 th 2013 #2 Chemsitry Objectives: 1.Understand the safety expectations in a CHS chemistry lab environment 2.Determine what you already know about chemistry.

4. Aug. 19 th / 20 th 2013 #3 Chemsitry Aug. 19 th / 20 th 2013 #3 Chemsitry Objectives: 1.Define chemistry and describe several ways in which chemistry affects your life. 2.Be able to differentiate between a chemical and physical change What did the teacher say when oxygen, hydrogen, sulfur, sodium, and phosphorous walked into his classroom? OH SNaP!

5. Aug. 21 st / 22 nd 2013 #4 Chemsitry Aug. 21 st / 22 nd 2013 #4 Chemsitry Objectives: 1.Distinguish between quantitative and qualitative observations. 2.Distinguish between accuracy and precision.

8. Aug. 23 rd 2013 #5 Chemistry Aug. 23 rd 2013 #5 Chemistry Objectives: 1.Distinguish between accuracy and precision. 2.Write numbers in scientific measurements with the correct significant figures

9. What does someone say when they’ve been shot?

10. Aug. 26 th / 27 th 2013 #6 Chemistry Aug. 26 th / 27 th 2013 #6 Chemistry Objectives: 1.Write numbers in scientific measurements with the correct significant figures

11. What do you say when a police man shows up at your bank robbery?

13. Cobalt 8.86 Nickel 8.912 Copper 8.933 Erbium 9.066 Polonium 9.32 (g/cm 3 )

14. Aug. 28 th / 29 th 2013 #7 Chemistry Aug. 28 th / 29 th 2013 #7 Chemistry Objectives: 1.Apply the technique of dimensional analysis to solving conversion problems. 2.Convert measurements in regular notation to scientific notation and vice versa.

15. What do you say if your bank robbery gets interupted?

16. Aug. 30 th 2013 #8 Chemistry Aug. 30 th 2013 #8 Chemistry Objectives: 1.Apply the technique of dimensional analysis to solving conversion problems. 2.Convert measurements in regular notation to scientific notation and vice versa.

17. We all have ___ fingers and toes.

18. Sep. 3 rd, 4 th 2013 #9 Chemistry Sep. 3 rd, 4 th 2013 #9 Chemistry Objectives: 1.Apply the technique of dimensional analysis to solving conversion problems. 2.Convert measurements in regular notation to scientific notation and vice versa.

19. I just got back from summer break. All of my math skills _____.

20. Sep. 6 th, 7 th 2013 #10 Chemistry Sep. 6 th, 7 th 2013 #10 Chemistry Objectives: 1.Calculate the density of pennies minted before 1982 and after 1983 2.Identify the metals in the cores of pennies minted after 1983. 3.Understand uncertainty of measurements and the use of significant figures

21. What do you do with a science teacher if he dies?

22. Objectives: 1.“See candle lab procedure”

24. I just hit my _____ the table…ouch!

25. Pee Wee Herman kept the other inmates laughing because he was a _____?

26. Objectives: 1.Determine what you know and don’t know in Unit 1 (UNIT ONE – sig figs, scientific notation w/ calculations, metric conversions, density, slope, graphing)

27. What should I do with the dirty beakers? O, just put them in the _____.

28. Warm Up

29. Sep. 16 th, 17 th 2013 #13 Chemistry Sep. 16 th, 17 th 2013 #13 Chemistry Objectives: 1. Be able to discuss the history of the atomic theory and explain early models of the atom

30. Peyton Manning ____ the Broncos to the 2014 Super Bowl!

31. Sep. 18 th, 19 th 2013 #14 Chemistry Sep. 18 th, 19 th 2013 #14 Chemistry Objectives: 1. Describe Rutherford’s concept of the atom. 2. Calculate atomic mass.

32. I will email you the instructions but first I need to _______ into the computer.

33. The actual mass of a proton is 1.673 x 10 -27 kg 1.) What is the mass of 6300 protons? 1.054 x 10 -23 kg 2.) Covert the mass of a proton from kg to decigrams 1.673 x 10 -23 dg 3.) Convert the mass of a proton from kg to megagrams 1.673 x 10 -30 Mg

34. Sep. 20 th 2013 #15 Chemistry Sep. 20 th 2013 #15 Chemistry Objectives: 1. Describe the Bohr Model

36. Sep. 23 rd, 24 th 2013 #16 Chemistry Sep. 23 rd, 24 th 2013 #16 Chemistry Objectives: 1. Be able to distinguish between atomic number and mass number, explain what makes elements and isotopes different from each other, and calculate average Atomic Mass

38. Calculate the molar mass of the following molecules 1.) CuSO 4 159.5 g/mol 2.) Cr 4 (P 2 O 7 ) 3 729.8 g/mol

39. Sep. 30 th, Oct 1 st 2013 #18 Chemistry Sep. 30 th, Oct 1 st 2013 #18 Chemistry Objectives: 1. Be able to convert grams to moles to particles.

40. Oct 4 th 2013 #19 Chemistry Oct 4 th 2013 #19 Chemistry Objectives: 1. Be able to convert grams to moles to particles. Homework 1.Study for your EXAM (10-9, 10-10) 2.Coulumbic Attraction, Unit 2 Review, Gram to Mole Conversion

42. Oct 7 th and 8 th 2013 #19 Chemistry Oct 7 th and 8 th 2013 #19 Chemistry Objectives: 1. Determine what you know and don’t know in Unit 2. (History of atomic theory, atomic structure, ions, isotopes, bohr model, molar mass, % abundance, molar conversion)

43. Score yourself on the following question. Give yourself a score from 1 – 5 on based on your comfort level. (1 = low, 5 = high) ANSWER: Atomic Weight = 10.811

44. Score yourself on the following question. Give yourself a score from 1 – 5 on based on your comfort level. (1 = low, 5 = high) ANSWER: 0.180 mol

47. Oct 21 st and 22 nd 2013 #20 Chemistry Oct 21 st and 22 nd 2013 #20 Chemistry Objectives: 1. Explain what the electromagnetic spectrum is.

48. The more you take the more you leave behind.

51. Oct 22 nd and 23 rd 2013 #21 Chemistry Oct 22 nd and 23 rd 2013 #21 Chemistry Objectives: 1. Explain the concepts regarding the electromagnetic spectrum.

52. Light as a feather, there is nothing in it, the strongest man can't hold it for much more than a minute. Light as a feather, there is nothing in it, the strongest man can't hold it for much more than a minute.

53. I went into the woods and I got it, I sat down to find it, I went home with it because I couldn’t get it. I went into the woods and I got it, I sat down to find it, I went home with it because I couldn’t get it.

54. Oct 28 th and 29 th 2013 #22 Chemistry Oct 28 th and 29 th 2013 #22 Chemistry Objectives: 1. Be able to describe the quantum processes that allow us to see color/light. 2. Be able to identify professions, on a global scale, that might use this information.

59. Nov 4 th & 5 th 2013 #23 Chemistry Nov 4 th & 5 th 2013 #23 Chemistry Today’s Objectives: 1. Apply the Aufbau principle, Pauli Exclusion principle, and Hund’s rule to write the electronconfiguration of atoms. 2. Compare s, p, d, and f orbitals in terms of size, shape, and energy.

60. Remove the outside, cook the inside, eat the outside, throw away the inside.

62. Nov 6 th & 7 th 2013 #24 Chemistry Nov 6 th & 7 th 2013 #24 Chemistry Today’s Objectives: 1.Write electron configurations for ions. 2.Relate the position of an element in the periodic table to its electron configuration

64. Nov 11 th & 12 th 2013 #25 Chemistry Nov 11 th & 12 th 2013 #25 Chemistry Today’s Objectives: 1.Determine what you know and don’t know in Unit 3

65. If a rooster laid a brown egg and a white egg, what kind of chicks would hatch?.

66. Nov 18 th & 19 th 2013 #26 Chemistry Nov 18 th & 19 th 2013 #26 Chemistry Unit 4 – Periodic Trends Objectives: 1. Describe the organization of the elements by Mendeleev. 2. Describe the revision of the periodic table by Mosely. 3. Relate the position of an element in the periodic table to its atomic number and atomic mass. 4. Describe the concept of ionization energy. 5. Use ionization energies to describe stabilities for atoms. Identify stability in terms of number of electrons in a shell. 6. Recognize periods and groups of the periodic table. 7. Identify the characteristics metals, nonmetals and metalloids. Identify where each is found on the periodic table. 8. Identify the representative elements, transition elements, and the inner transition elements on the periodic table. 9. Identify alkali metals, alkaline earth metals, halogens, noble gases, lanthanide and actinide elements on the periodic table. 10. Identify valence electrons. Use the group number to determine the number of valence electrons and predict the charge for the stable ion. 11. Describe and explain the trends in atomic size, ionization energy, electronegativity, chemical and physical properties within a group and period. 12. Explain how the periodic law can be used to predict the physical and chemical properties of elements.

67. Nov 18 th & 19 th 2013 #26 Chemistry Nov 18 th & 19 th 2013 #26 Chemistry Today’s Objectives: See objective list