Semester Review Guide

1. Volume is an example of which of the following properties (check all that apply):a. _____ Quantitative Propertyb. _____ Qualitative Propertyc. _____ Extensive Property d. _____ Intensive Propertye. _____ Physical Propertyf. _____ Chemical Property

2. List the four possible indicators of a chemical reaction:

3. Chemistry is the study of ____________________ and the changes it undergoes.

4. Fill in the blanks below with the physical state of matter that applies to the description.

a. _______________ has a definite shape and a definite size

b. _______________ has a definite size, but not a definite shape

c. _______________ has an indefinite(changing) size and an indefinite shape

5. What is the simplest form of matter?

6. What is it called when a substance is made up of 2 or more of the answer to question five?

7. Check which of the following are heterogeneous mixtures:a. _____ Trail Mixb. _____ Chicken Noodle Soupc. _____ Pepsi colad. _____ Koolaide. _____ Ice Tea

8. What is the act of separating a liquid by evaporating it and condensing it back?

9. Conan O’Brien wanted to see how his choice in outfits would affect the show’s ratings. HE ran the following trials:

Trial 1: Conan wore a black suit with a red tie. He drank out of his blue coffee mug, while he hosted an actor from a popular tv show.

Trial 2: Conan wore a gray suit with a pink tie. He drank out of his blue coffee mug while he hosted an actor from a different a popular tv show.

In Conan’s experiment what were the following?

Dependent variable:

Independent variable:

Control:

10. Label the targets below as either: accurate; precise; both or neither.

11. You order a box of imported chocolates online and when you get it you weigh it to see how

much you received. The scale says that it weighs 1.4lbs, but the shipping receipt says that the box weighs 1.5lbs. What is your percent error?

12. Identify how many significant figures are in the following numbers:a. _____ 0.013

b. _____ 302.1

c. _____ 12.467

d. _____ 37.90

e. _____280

13. Convert the following numbers into scientific notation:a. 120045

b. .006301

14. Convert the following numbers out of scientific notation:

a. 6.0791 x 102

b. 2.03 x 10-7

15. Perform the following calculations and round your answers to the appropriate number of significant figures or decimals places:

a. 5.02 x 103 + 6.17 x 104 _______________________

b. (8.205 x 10-5) x (1.16 x 10-3) _______________________

c. (7.214 x 108) / (3.6875 x 105) _______________________

16. Convert 5.7Km to miles

17. Mr. Gates wanted to buy his 82 students donuts. He figures each student will eat 2 donuts and when he picked up the donuts the drive through menu said that the cost is $13.58 for a box of a dozen (12) donuts. How much will it cost for Mr. Gates to feed his students donuts? If Mr. Gates has a coupon that will give him one additional free donut for every $20 spent on purchasing donuts, how many additional donuts will you get for free?

18. The smallest particle within an element that still retains its identity in a chemical reaction is what?

19. Who believed that an atom was a tiny indivisible and indestructible particle?

20. Who used experimental methods to observe patterns in which elements combined to form new products and as a result confirmed the presence of atoms?

21. What are the four principals of John Dalton’s atomic theory?

22. Discovered by J.J. Thompson, this negatively charged subatomic particle is called what?

23. What is the symbol for an electron?

24. Discovered by Earnest Rutherford, this positively charged subatomic particle is called what?

25. What is the symbol for a proton?

26. Discovered by James Chadwick, this neutrally charged subatomic particle is called what?

27. What is the symbol for a neutron?

28. What are the names of the three subatomic particles?

29. What did J.J. Thompson’s model look like?

30. What other name does the J.J. Thompson model go by?

31. The tiny central core of an atom that is composed of protons and neutrons is called what?

32. What is the net charge of a nucleus?

33. According to Rutherford, where were the electrons found?

34. Where in the atom is the majority of the mass found?

35. Where in the atom is the majority of the size found?

36. The atomic number of an element describes the number of what?

37. Can the atomic number of an element change and if so when?

38. Which number describes the mass of an atom in atomic mass units?

39. What equation is used to calculate the number of neutrons that exist in an atom?

40. What are the one or two letter combinations assigned to each element?

41. Is the following statement true or false? If a chemical symbol has two letters, both letters can be capitalized.

42. What is the difference between isotopes?

43. Do isotopes have different chemical properties?

44. What is the weighted average mass of the atoms in a naturally occurring sample of an element?

45. Fill in the blanks… The weighted average reflects both the ______ and the ______ of each isotope present.

46. What was the issue with Rutherford’s model of the atom?

47. What was the new idea that Bohr proposed in his model of the atom?

48. As you move farther away from the nucleus, Bohr said that:a) Energy levels would increase, but the energy required for electrons to jump between them would decrease.b) Energy levels would decrease, but the energy required for electrons to jump between them would increase.c) Both energy levels and the amount of energy required for electrons to jump between them would increase.d) Both energy levels and the amount of energy required for electrons to jump between them would decrease.

49. At most, how many electrons can the first orbit hold and how many could the second orbit hold at most?

50. What determined the allowed energies an electron can have and how likely it is to find an electron in various locations around the nucleus?

51. What is an atomic orbital?

52. The electron configuration of an atom is what?

53. Describe the Aufbau Principle.

54. Describe the Pauli Exclusion Principle.

55. Describe Hund’s Rule.

56. Define the frequency of a wave.

57. If Electron A falls farther than Electron B, will the same light be produced by the energy emitted from these electrons?

58. What does it mean for an electron to be in its ground state?

59. Do all elements produce the same light when electricity is passed through them?

60. How can we use an atomic emission spectrum to identify unknown elements?

61. What happens when electrons are de-excited?

62. What does it mean for energy to be emitted?

63. Explain the significance of the energy gap between suborbitals.

Element Symbol

Element

Name

Atomic Number

Mass Number

Electrons

Protons Neutrons

Te

17

55

247 151

64. Correctly fill in the following orbital diagram for the element Oxygen. Use arrows to represent electrons. (2pts)

Write out the correct unabbreviated electron configurations for the elements listed below.

65. Calcium (Ca) __________________________________________________

66. Sulfur (S) _______________________________________________________

67. Barium (Ba) _______________________________________________________

Write out the correct abbreviated (noble gas) configuration for the elements listed below.

68. Aluminum (Al) _______________________________________________________

69. Bromine (Br) _______________________________________________________

70. Sodium (Na) _______________________________________________________

71-74. Correctly fill in the boxes below, describing different parts of a wave:

1s 2s 2p 3s 3p 4s

If a light source has a frequency of 3.26 x 1014Hz…

75. What is the wavelength of the light source?

76. What is the energy of the light source?

77. Dimitri Mendeleev organized his periodic table around what increasing trend?a. Ionization Energyb. Atomic Numberc. Massd. Atomic Radius

78. Henry Mosely organized his periodic table around what increasing trend?a. Ionization Energyb. Atomic Numberc. Electronegativityd. Atomic Radius

79. The following is a definition of what: “When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.”

e. Periodic Truthf. Periodicity Theoryg. Law of Periodicityh. Periodic Law

80. A chart of the chemical elements that displays them in rows horizontally in order of increasing atomic number and vertically according to similarity of the chemical properties of their atoms is called what?

i. Periodic Tablej. Elemental Chartk. Property Diagraml. Periodicity Chart

81. Using group and period numbers, describe the location of Chromium.

82. Using group and period numbers, describe the location of Strontium.

83. Using group and period numbers, describe the location of Silver.

84. Using group and period numbers, describe the location of Lead.

85. What is the name of the group that sodium belongs to?

86. What is the name of the group that chlorine belongs to?

87. What is the name of the group that copper belongs to?

88. What is the name of the group that argon belongs to?

89. What is the name of the group that barium belongs to?

90. What is the name of the group that Uranium (U) belongs to?

91. Electronegativity increases as you move in which vertical and horizontal directions?

92. Atomic radius increases as you move in which vertical and horizontal directions?

93. Ionization energy decreases as you move in which vertical and horizontal directions?

94. Which group of elements has the lowest amount of electronegativity?

95. What is the difference between an atom and an ion?

96. What is the name of a positively charged ion?

97. What is the name of a negatively charged ion?

98. What is the name of the electrons in the outermost energy level of an atom?

99. Define the octet rule.

100. Draw the Lewis dot structure for an atom of sulfur.

101. Draw the Lewis dot structure for an atom of calcium.

102. What is formed by electrostatic attractions between positive and negative ions?

103. What is the name of a chemical formula of an ionic compound?

104. What does the Law of Definite Proportions tell us about ionic compounds?

105. What is the formula unit and the name for the ionic compound created from the combination of the following ions:

m. Na+ and O-2

n. K+ and CO3-2

o. Cu+ and Cl-

p. Cu+2 and Cl-

106. Explain what causes crystalline shapes of ionic compounds.

107. What are the coordination number of Na+ and Cl- ions in the following structure:

108. Explain what happens when you hit an ionic compound with a hammer and state the property responsible.

109. Why does salt conduct electricity when dissolved in water, but not as a solid?

110. What is responsible for metal ions bonding together?

111. Explain what happens when you hit a metal with a hammer and state the property responsible.

112. What does it mean for a metal to be ductile and how is this possible?

113. Explain why metals are good conductors of electricity.

114. Define the term “alloy” and provide an example of an alloy.

For the following molecular formulas, draw the corresponding Lewis dot structure and write the name of the compound and the geometric shape.

115. C2Br2

116. SH2

117. NI3

Write the names of the following covalent compounds:

118. S8H10 ________________________________________________

119. N3H9 ________________________________________________

120. P4S5 ________________________________________________

121. Determine if the following bonds are Polar Covalent, Nonpolar Covalent, or Ionic.

a. K and Cl

b. C and S

c. H and C