1. Jeremy decides to make some Macaroni and Cheese from a box. He notices the directions ask him to add salt to water before bringing it to a boil. The next day, Jeremy asks his science teacher “How does adding salt to water affect the way it boils?” They plan an experiment to find out the answer. The following graph summarizes Jeremy’s findings. List all of the materials and equipment that Jeremy would have to use in his experiment.

2. Using Jeremy’s experiment, identify: 1. the independent variable. 2. the dependent variable. 3. the experimental control group. 4. Jeremy’s probable conclusion.

3. Which formula represents a molecular compound? (1) HI(3) KCl (2) KI (4) LiCl

4. Which type of matter is composed of two or more elements that are chemically combined in a fixed proportion? (1) solution (2) compound (3) homogeneous mixture (4) heterogeneous mixture

5. EX 1: Convert 1006051 to scientific notation. 1006051 Decimal will move here The natural decimal point is here 1.006051 x 10 6 6 because the decimal moved 6 times

6. Determine the number of protons, neutrons, electrons, and the mass number Zn 65 30 2+

7. 30 protons, 35 neutrons, 28 electrons, mass number = 65

8. EX 2: Convert 0.0052300 to scientific notation. 0 0052300 Decimal will move here The natural decimal point is here 5.2300 x 10 -3 Negative because the original number is less than 1 and 3 because the decimal moved 3 times

9. EX: Determine the number of significant figures in a) 4 b) 4.0 c) 40 d) 0.0400 e) 4004 f) 0.0004 1 2 1 3 4 1

10. Practice EX 1: Determine the number of significant figures in: a)2 b)5.0 c)10 d)0.0400 e)8005 f)3.00 x 10 3 1 2 1 3 4 3

11. EX 2: Convert each of the values into scientific notation while retaining the same number of sig figs a)60000 b)20 c)4004 d)0.0900 6 x 10 4 2 x 10 1 4.004 x 10 3 9.00 x 10 -2

12. Lets practice together… Round the following numbers to 3 sig figs a) 51.234 b) 51.38 c) 51.3587 d) 51,358 e) 0.050554 51.2 51.4 51,400 0.0506 Or 5.12 x 10 1 Or 5.14 x 10 1 Or 5.14 x 10 4 Or 5.06 x 10 -2

13. YOUR Practice EX: Round the following numbers to 3 sig figs a)51.23451.2 b)51.38 c)51.3587 d)51,358 e)0.050554 f)5,135,593 51.2 51,400 51.4 0.0506 51.4 5,140,000

14. Example: It is expected that you will always report all sig figs on any laboratory reading! 1 2 3 4 5 6 7 8 9 10 2.8

15. Example: It is expected that you will always report all sig figs on any laboratory reading! 1 2 3 4 5 6 7 8 9 10 2.71

16. Which Lewis electron-dot diagram represents calcium oxide?

17. Explain which of the following represent pure substances and which represent mixtures.

18. Practice 1)22.101 mL – 0.9307 mL = 2)2.5 g / 3.42 g = 3)2.33 cm x 6.085 cm x 2.1 cm = 4)23.1 in + 4.77 in + 125.39 in + 3.581 in = 21.170 mL 0.73 g 30. cm 3 156.8 in

19. EX: 37.24 mL + 10.3 mL = 27.87 g – 2.2342 g = 47.5 mL 25.64 g

20. Rules for Math Operations with Significant Figures Addition and Subtraction Ex. 37.24mL + 10.3 mL 47.54mL Reported as 47.5mL

21. Rules for Math Operations with Significant Figures Addition and Subtraction Ex. 27.87 g - 21.2342 g 6.6358 g Reported as 6.64g

22. 2. Multiplication and Division The measurement with the fewest sig figs determines the number of sig figs in the answer EX: 12.34 cm X 0.23 cm = 2.8 cm 2

23. Practice 2. Determine the number of g in 0.03455 kg wantgiven 0.03455 kg1000 g g 1 kg = 34.6 1 Relationship 1000g = 1kg Start with what’s given

24. 1.06 qt. Ex. 2 Convert 323 mL to cups wantgiven 323 mL1 L cups 1000 mL = 1.37 1 Relationships 1000 mL = 1L 1L = 1.06 quarts 1 quart = 4 cups Start with what’s given 1 L 1 qt. 4 cups

25. 2.54 cm Practice 1: Convert 7.005 ft to mm wantgiven 7.005 ft 12 in mm 1 ft = 2135 1 Relationships 1 foot = 12 inches 2.54cm = 1 in 100 cm = 1 m 1 m = 1000 mm Start with what’s given 1 in100 cm 1 m 1000 mm 1 m

26. 1 hr EX 1: Convert 0.083 km/h to m/s wantgiven 0.083km 1000m m/s 1 km = 2.31 X 10 -2 1hr Relationships 1km = 1000m 1h = 60 min 1 min = 60 s Start with what’s given 60 min60 s 1 min

27. 1 ft 1. Convert 3.56 cm/s to ft/h want given 3.56 cm 1 in ft/hr 2.54 cm = 420 1 s Relationships 2.54 cm = 1 in 12 in = 1 ft 60 s = 1 min 1 hr = 60 min Start with what’s given 12 in 1 min 60 s 1 hr 60 min

28. 1 ft 2. Convert $25.00/feet to cents/cm wantgiven $ 25.00 100 cents cents/cm $1 = 82.0 1 ft Relationships $1 = 100 cents 2.54 cm = 1 in 12 in = 1 ft Start with what’s given 12 in 2.54 cm 1 in

29. Determine the number of centimeters in 1.76 kilometers (Show all dimensional analysis.)

30. Determine the number of inches in 697 mm. Note: 2.54 cm = 1 inch (Show all dimensional analysis.)

31. Determine the number of atoms in 5.20 moles of C 6 H 12. (Show all dimensional analysis.)

32. How many significant figures do the following numbers contain? A) 4,250.00 B) 4040 C) 0.009 D) 325.08 E) 6.02 x 10 23

33. Find the answer to the following using the correct number of significant figures. A) 4,250.38 + 25.1 B) 4040 x 32

34. Read the following to the correct number of significant figures.

35. Which statement describes a chemical property of bromine? (1) Bromine is soluble in water. (2) Bromine has a reddish-brown color. (3) Bromine combines with aluminum to produce AlBr 3. (4) Bromine changes from a liquid to a gas at 332 K and 1 atm.

36. An atom of aluminum in the ground state and an atom of gallium in the ground state have the same - (1) mass (2) electronegativity (3) total number of protons (4) total number of valence electrons

37. In an atom of argon-40, the number of protons – (1) equals the number of electrons (2) equals the number of neutrons (3) is less than the number of electrons (4) is greater than the number of electrons

38. Which type of substance can conduct electricity in the liquid phase but not in the solid phase? (1) ionic compound (2) molecular compound (3) metallic element (4) nonmetallic element

39. Why is a molecule of CO 2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar? (1) The shape of the CO 2 molecule is symmetrical. (2) The shape of the CO 2 molecule is asymmetrical. (3) The CO 2 molecule has a deficiency of electrons. (4) The CO 2 molecule has an excess of electrons.

40. The relatively high boiling point of water is due to water having- (1) hydrogen bonding (2) metallic bonding (3) nonpolar covalent bonding (4) strong ionic bonding

41. Matter is classified as a - (1) substance, only (2) substance or as a mixture of substances (3) homogenous mixture, only (4) homogenous mixture or as a heterogeneous mixture

42. Which substance can not be decomposed by a chemical change? (1) ammonia (3) propanol (2) copper (4) water

43. A beaker contains both alcohol and water. These liquids can be separated by distillation because the liquids have different (1) boiling points (3) particle sizes (2) densities (4) solubilities

44. A sample of an element is malleable and can conduct electricity. This element could be - (1) H (3) S (2) He (4) Sn

45. Identify the element in Period 3 of the Periodic Table that reacts with oxygen to form an ionic compound represented by the formula X 2 O.

46. Based on data collected during a laboratory investigation, a student determined an experimental value of 322 joules per gram for the heat of fusion of H 2 O. Calculate the student’s percent error. Your response must include a correct numerical setup and the calculated result.

47. Calculate the density of a 129.5- gram sample of bronze that has a volume of 14.8 cubic centimeters. Your response must include a correct numerical setup and the calculated result. 8.75 g/cm 3

48. Atomic Structure Questions Answers

49. Determine the number of protons, neutrons, and electrons in an ion of magnesium with a 2+ charge and a mass number of 25.

50. p + = 12 n 0 = 13 e - = 10

51. True or False? Elements cannot be created, divided, or destroyed

52. False Elements can be divided (particle accelerators/ atom smashers)

53. Determine the element’s identity: Element – 28 92.23% Element – 29 4.67% Element – 30 3.10% Relative Abundance

54. Silicon

55. The Gold Foil experiment resulted in the discovery of the ______

56. Nucleus!

57. Europium has two naturally- occurring isotopes: europium- 151 with an abundance of 47.82% and europium-153 with an abundance of 52.18%. Determine the average atomic mass for europium.

58. 152.0436 amu

59. Who developed the plum pudding model?

60. JJ Thompson

61. How can you determine the mass number?

62. Protons + neutrons

63. What is fluorine’s most abundant isotope?

64. Fluorine - 19

65. All atoms of an element are ________ from another element

66. All atoms of an element are different from another element

67. Who discovered the electron?

68. JJ Thompson

69. Determine the number of protons, neutrons, and the mass number H 3131

70. 1 proton, 2 neutrons, mass number = 3

71. If 3 protons could be removed from the nucleus of an Nitrogen atom, what nucleus remains?

72. Beryllium 7p – 3p = 4p

73. Determine which element has a mass number of 45 and has 14 neutrons.

74. Gallium

75. Determine the number of protons, neutrons, and electrons in an atom of silicon-29.

76. protons = 14 neutrons = 15 electrons = 14

77. Write the isotope for the element given that it has 12 protons and 14 neutrons. Show the isotope in both ways.

78. Magnesium – 26 Mg 26 12

79. What part of the atom takes up the most amount of space?

80. electrons

81. What element is used as the standard for atomic mass units?

82. carbon

83. The end of an electron configuration says 4d 4. What element is represented?

84. What does n represent?

85. Why can’t we have two up spins next to each other?

86. What is the roman numeral of the group found at np 3 ?

87. How many orbitals have electrons in the configuration: 1s 2 2s 2 2p 6 3s 1 ***hint*** you probably want to write out the orbital notation.