1. Chemistry Final Exam Review and Practice Chapters Covered –ESSENTIALLY CUMMULATIVE –List of Chapters: CP: 4, 5, 7, 8,. 14, 15, 18, 19 H: 5, 6, 7, 8, 12, 14, 18

2. Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non –metal, etc. Electron Configuration: Orbitals and SubLevels Valence Electrons Electron Configuration: Atomic #, mass, core notation Periodic Trends: Chemical and Physical Properties Atomic Radii, Electronegativity, Ionic Radii, Ions /Compounds Family names Bonding: Covalent and Ionic Lewis dot diagrams Bonding:Electronegativity to determine if nonpolar covalent or polar covalent, both bond and molecules. Bonding : molecular shapes, intermolecular forces Solutions: solubility curves Acid and Bases and pH

3. Atomic Sturcture and Electron Configuration Location of electrons in s, p, d, f orbitals. Location of electrons in s, p, d, f orbitals. Shape and number of s and p orbitals. Shape and number of s and p orbitals. Number of electrons each orbital each sublevel and each level can hold. Number of electrons each orbital each sublevel and each level can hold. Location of s, p, d, f blocks on periodic table. Location of s, p, d, f blocks on periodic table. Lewis dot diagrams. Lewis dot diagrams. Formation of complete octets by transfer of / sharing of electrons. Formation of complete octets by transfer of / sharing of electrons.

4. Electron Configuration & Periodic Table Filling orbital diagrams Filling orbital diagrams Writing electron configurations Writing electron configurations Core notation using chemical symbol of preceding noble gas Core notation using chemical symbol of preceding noble gas Trends for physical and chemical properties Trends for physical and chemical properties Atomic radii, ionization energy, electronegativity Atomic radii, ionization energy, electronegativity

5. Bonding Ionic versus covalent Ionic versus covalent Valence electrons and dot diagrams Valence electrons and dot diagrams Lewis structures: shared pairs and lone pairs Lewis structures: shared pairs and lone pairs Stability of “octet” electron arrangement of noble gases

6. Molecular Shapes and Polarity Recognize drawings of ball and stick models Recognize drawings of ball and stick models Use VSEPR Use VSEPR Recognize dipole as electrons being pulled towards the higher electronegative element, causing a partial negative charge on that atom and a partial positive charge on the lower electronegative atom Recognize dipole as electrons being pulled towards the higher electronegative element, causing a partial negative charge on that atom and a partial positive charge on the lower electronegative atom Dispersion, dipole-dipole, hydrogen bonding: types of intermolecular forces in covalent compounds

7. Solutions Solubility Curves Solubility Curves Vocabulary Vocabulary –Saturated, Unsaturated, Supersaturated –Solute, Solvent, Solution, etc. Molarity definition and calculation Molarity definition and calculation

8. Acids, Bases and pH Acid and base characteristic Acid and base characteristic Vocabulary: Vocabulary: –K a, –K a, dissociation, electrolyte,amphoteric neutralization reaction and products Self Ionization of Water and pH Self Ionization of Water and pH –Defintion / math formula –Calculation from molarity

9. What is the maximum number of electrons that can by held in an “s” sublevel? A.1 A.1 B.2 B.2 C.6 C.6 D.8 D.8 #1

10. What is the maximum # of e - that can by held in a “p” sublevel? A.1 A.1 B.2 B.2 C.6 C.6 D.8 D.8 #2

11. What is the total number of sublevel for n=2? A.1 A.1 B.2 B.2 C.6 C.6 D.8 D.8 #3

12. For an element whose electron configuration is [Ne]3s 2 3p 3, how many dots would the Lewis dot diagram have? A.3 A.3 B.5 B.5 C.8 C.8 D.13 D.13 #4

13. How many dots does the Lewis dot diagram for chlorine have? A.3 A.3 B.5 B.5 C.7 C.7 D.8 D.8 #5

14. A positive lithium ion is formed when a neutral lithium atom: A.gains one proton A.gains one proton B.gains one electron B.gains one electron C.loses one proton C.loses one proton D.loses one electron D.loses one electron #6

15. When a potassium atom becomes an ion, it: A.gains one proton A.gains one proton B.gains one electron B.gains one electron C.loses one proton C.loses one proton D.loses one electron D.loses one electron #7

16. When a calcium atom becomes an ion, it: A.gains two protons A.gains two protons B.gains two electrons B.gains two electrons C.loses two protons C.loses two protons D.loses two electrons D.loses two electrons #8

17. Use the periodic table to locate K; what block is it in? a. s-block a. s-block b. p-block b. p-block c. d-block c. d-block d. f-block d. f-block #9

18. What does [Ar]4s 1 represent? a. the full electron configuration of K a. the full electron configuration of K b. the abbreviated electron configuration for K b. the abbreviated electron configuration for K c. the full mass designation for K c. the full mass designation for K d. the block designation for K d. the block designation for K #10

19. What does Ar represent in [Ar]4s 1 ? a. the block of the periodic table a. the block of the periodic table b. the highest orbital filled b. the highest orbital filled c. the chemical symbol of the preceding noble gas c. the chemical symbol of the preceding noble gas d. the chemical symbol of the element d. the chemical symbol of the element #11

20. What kind of bond is predicted to form between B and H if their electronegativities are 2.0 and 2.2 respectively? a. nonpolar covalent a. nonpolar covalent b. polar covalent b. polar covalent c. ionic c. ionic d. intermolecular d. intermolecular #12

21. A bond is nonpolar covalent if the difference in electronegativities between the two atoms is: A. 2.1 or more A. 2.1 or more B. between 0.5 and 2.1 B. between 0.5 and 2.1 C. less than 0.4 C. less than 0.4 D. less than zero D. less than zero #13

22. Which of the following bonds would be considered completely nonpolar? A. H-N A. H-N B. O-O B. O-O C. O-C C. O-C D. F-Cl D. F-Cl #14

23. For the diatomic molecule Cl 2, how many electron(s) does each chlorine share with the other chlorine? A. 1 A. 1 B. 2 B. 2 C. 7 C. 7 D. 8 D. 8 #15

24. How many pairs of shared and unshared electrons does the Lewis dot structure for water have? A. 4, 0 A. 4, 0 B. 3, 1 B. 3, 1 C. 2, 2 C. 2, 2 D. 4, 4 D. 4, 4 #16

25. In a double bond between two atoms, the number of shared electrons is: A. 2 A. 2 B. 4 B. 4 C. 6 C. 6 D. 8 D. 8 #17

26. In the compound ammonia, NH 3 : A. Each hydrogen has a partial negative charge A. Each hydrogen has a partial negative charge B. The nitrogen has a full positive charge B. The nitrogen has a full positive charge C. The N-H bond is ionic C. The N-H bond is ionic D. The Lewis structure will have one unshared pair of electrons D. The Lewis structure will have one unshared pair of electrons #18

27. What kind of compound would form between nonmetallic atoms and non metallic atoms? A. Nonpolar covalent A. Nonpolar covalent B. Polar covalent B. Polar covalent C. Ionic C. Ionic D. Covalent D. Covalent #19

28. What kind of compound would form between polyatomic ions and metallic ions? A. Nonpolar covalent A. Nonpolar covalent B. Polar covalent B. Polar covalent C. Ionic C. Ionic D. Covalent D. Covalent #20

29. What kind of compound would form between metallic ions and nonmetallic ions? A. Nonpolar covalent A. Nonpolar covalent B. Polar covalent B. Polar covalent C. Ionic C. Ionic D. Covalent D. Covalent #21

30. What kind of compound would form between potassium and bromine?: A. Nonpolar covalent A. Nonpolar covalent B. Polar covalent B. Polar covalent C. Ionic C. Ionic D. Macromolecular covalent D. Macromolecular covalent #22

31. Predict the physical state of the compound formed between magnesium and oxygen: A. Probably a gas A. Probably a gas B. Probably a liquid B. Probably a liquid C. Probably a solid C. Probably a solid D. Impossible to determine from the given data D. Impossible to determine from the given data #23

32. The physical state of nearly all ionic compounds at room temperature is: A. Solid A. Solid B. liquid B. liquid C. Gas C. Gas D. Different for each ionic compound D. Different for each ionic compound #24

33. Ionic Compounds are generally: A. Conductors of electricity in the solid state A. Conductors of electricity in the solid state B. Gases at room temperature B. Gases at room temperature C. Formed when a metal transfers its valence electron to a nonmetal C. Formed when a metal transfers its valence electron to a nonmetal D. Electrically charged D. Electrically charged #25

34. How does a covalent bond differ from an ionic bond? A. Ionic: transfer of e - ; covalent: sharing of e - A. Ionic: transfer of e - ; covalent: sharing of e - B. Ionic: involves 2 e - ; covalent: involves 4 e - B. Ionic: involves 2 e - ; covalent: involves 4 e - C. Ionic: btw metals; covalent btw nonmetals C. Ionic: btw metals; covalent btw nonmetals D: Ionic: usually acids; covalent: usually bases D: Ionic: usually acids; covalent: usually bases #26

35. Which theory is used to account for the shape of molecules? A. theory of relativity A. theory of relativity B. thermodynamic theory B. thermodynamic theory C. kinetic theory C. kinetic theory D. VSEPR theory D. VSEPR theory #27

36. Which of the following does a ball and stick model reveal about chemical bonds? A. their arrangement in space A. their arrangement in space B. their presence and type B. their presence and type C. both A and B C. both A and B D. neither A or B D. neither A or B #28

37. What shape does an ammonia, NH 3, molecule have? A. pyramidal A. pyramidal B. trigonal planar B. trigonal planar C. tetrahedral C. tetrahedral D. bent D. bent #29

38. What shape does a water molecule have? A. pyramidal A. pyramidal B. trigonal planar B. trigonal planar C. tetrahedral C. tetrahedral D. bent D. bent #30

39. In a molecule of carbon dioxide, what kind of bonds connect the carbon atom to the 2 oxygen atoms? A. two single bonds A. two single bonds B. one single and one double bond B. one single and one double bond C. one double and one triple bond C. one double and one triple bond D. two double bonds D. two double bonds #31

40. What shape is a carbon dioxide molecule? A. linear A. linear B. bent B. bent C. trigonal planar C. trigonal planar D. pyramidal D. pyramidal #32

41. What shape is a methane, CH 4 molecule? A. tetrahedral A. tetrahedral B. bent B. bent C. trigonal planar C. trigonal planar D. pyramidal D. pyramidal #33

42. What is the bond angle of a molecule of ammonia, NH 3 ? A. 107 o A. 107 o B. 109.5 o B. 109.5 o C. 120 o C. 120 o D. 180 o D. 180 o #34

43. What is the bond angle of a molecule of carbon dioxide? A. 107 o A. 107 o B. 109.5 o B. 109.5 o C. 120 o C. 120 o D. 180 o D. 180 o #35

44. What is the bond angle of a molecule of methane? A. 107 o A. 107 o B. 109.5 o B. 109.5 o C. 120 o C. 120 o D. 180 o D. 180 o #36

45. What is the bond angle of a molecule of water? A. 90 o A. 90 o B. 105 o B. 105 o C. 107 o C. 107 o D 109.5 o D 109.5 o #37

46. Which of the following properties would you expect to find in a small nonpolar molecule? A. Gas at room temperature A. Gas at room temperature B. Solid at room temperature B. Solid at room temperature C. Very high melting point C. Very high melting point D Very high boiling point D Very high boiling point #38

47. In a pyramidal molecule, how many unshared pairs of valence electrons does the central atom have? A. None A. None B. One B. One C. Two C. Two D. Three D. Three #39

48. In a tetrahedral molecule, how many unshared pairs of valence electrons does the central atom have? A. None A. None B. One B. One C. Two C. Two D. Three D. Three #40

49. In polar bonds electrons are: A. Shared unequally A. Shared unequally B. Shared equally B. Shared equally C. Completely transfered C. Completely transfered D. Not shared at all D. Not shared at all #41

50. Dipoles are: A. Nonpolar bonds A. Nonpolar bonds B. Polar bonds B. Polar bonds C. Nonpolar molecules C. Nonpolar molecules D. Polar molecules D. Polar molecules #42

51. What determines the polarity of a bond? A. Electronegativity difference only A. Electronegativity difference only B. Molecular shape only B. Molecular shape only C. Both A and B C. Both A and B D. Neither A and B D. Neither A and B #43

52. What determines the polarity of a molecule? A. Electronegativity difference only A. Electronegativity difference only B. Molecular shape only B. Molecular shape only C. Both A and B C. Both A and B D. Neither A and B D. Neither A and B #44

53. How are the electrons shared in a bond between carbon & oxygen? A. They are shared equally A. They are shared equally B. Carbon attracts them more B. Carbon attracts them more C. Oxygen attracts them more C. Oxygen attracts them more D. Electrons are completely transferred D. Electrons are completely transferred #45

54. All solutions have the following properties except that the: A. Dissolved particles are very small A. Dissolved particles are very small B. Particles in a solution are evenly distributed B. Particles in a solution are evenly distributed C. Solution particles do not settle out C. Solution particles do not settle out D. Final physical state of a solution is a liquid D. Final physical state of a solution is a liquid #46

55. Which of the following statements applies to the dissolved solute particles in a solution? A. They can be seen with the unaided eye A. They can be seen with the unaided eye B. They will be in the same phase as the solvent B. They will be in the same phase as the solvent C. They will settle out when left standing C. They will settle out when left standing D. There is always less solute than solvent D. There is always less solute than solvent #47

56. An alloy is an example of a: A. Gaseous mixture A. Gaseous mixture B. Liquid solution B. Liquid solution C. Solid solution C. Solid solution D. Solid mixture D. Solid mixture #48

57. Solutions with water as the solvent are called: A. Liquids A. Liquids B. Miscible solutions B. Miscible solutions C. Aqueous solutions C. Aqueous solutions D. Electrolytes D. Electrolytes #49

58. Molarity is expressed as: A. Moles of solvent / Liters of solute A. Moles of solvent / Liters of solute B. Moles of solute / Liters of solvent B. Moles of solute / Liters of solvent C. Moles of solute / Liters of solution C. Moles of solute / Liters of solution D. Moles of solute / moles of solution D. Moles of solute / moles of solution #50

59. A solution that contains as much solute as can possibly be dissolved under existing conditions is said to be: A. saturated A. saturated B. supersaturated B. supersaturated C. soluble C. soluble D. concentrated D. concentrated #51

60. Which of the following is NOT an important factor influencing solubility? A. Chemical nature of solute A. Chemical nature of solute B. Temperature B. Temperature C. Chemical nature of solvent C. Chemical nature of solvent D. Volume of solution D. Volume of solution #52

61. Common nonpolar solvents include all of the following except: A. Salt water A. Salt water B. Carbon tetrachloride B. Carbon tetrachloride C. Hexane C. Hexane D. Vegetable oil D. Vegetable oil #53

62. Ionic solids best dissolve in liquid solvents that are: A. polar A. polar B. nonpolar B. nonpolar C. viscous C. viscous D. transparent D. transparent #54

63. Which of the following’s solubility is most affected by pressure? A. Ionic solids A. Ionic solids B. Supersaturated solutions B. Supersaturated solutions C. Gases C. Gases D. Alloys D. Alloys #55

64. Why can water dissolve NaCl, whereas hexane cannot? A. Hexane is attracted to the sodium, but not to the chlorine A. Hexane is attracted to the sodium, but not to the chlorine B. As a polar solvent, water is attracted to both anions and cations B. As a polar solvent, water is attracted to both anions and cations C. Both water and salt are inorganic, while hexane is organic C. Both water and salt are inorganic, while hexane is organic D. Water can form hydrogen bonds with NaCl D. Water can form hydrogen bonds with NaCl #56

65. The rate at which a solid can be dissolved in a liquid solvent can be increased by: A. Lowering the temperature of the solvent A. Lowering the temperature of the solvent B. Grinding the solute into smaller pieces B. Grinding the solute into smaller pieces C. Increasing the air pressure on the liquid C. Increasing the air pressure on the liquid D. Lowering the temperature of the solute D. Lowering the temperature of the solute #57

66. To identify the strongest acid, compare the K a and: A. The highest K a value is the strongest acid A. The highest K a value is the strongest acid B. The lowest K a value is the strongest acid B. The lowest K a value is the strongest acid C. The K a closest to pH 7 is the strongest acid C. The K a closest to pH 7 is the strongest acid D. The K a closest to pH 0 is the strongest acid D. The K a closest to pH 0 is the strongest acid #58

67. Substances that change color when added to acids or bases are called: A. indicators A. indicators B. electrolytes B. electrolytes C. insulaotrs C. insulaotrs D. capacitators D. capacitators #59

68. The ionic compound formed in acid-base neutralization reactions is: A. water A. water B. a salt B. a salt C. hydride C. hydride D. hydroxide D. hydroxide #60

69. A substance that can act as either an acid or a base is described as: A. neutral A. neutral B. ambidextrous B. ambidextrous C. conjugate C. conjugate D. amphoteric D. amphoteric #61

70. Which of the following is least able to donate a proton? A. HF A. HF B. H 2 O B. H 2 O C. HCO 3 - C. HCO 3 - D. F - D. F - #62

71. Which of the following could be a conjugate acid-base pair? A. strong acid –strong base A. strong acid –strong base B. weak acid - weak base B. weak acid - weak base C. strong acid – weak base C. strong acid – weak base D. need more information D. need more information #63

72. The acid dissociation constant, K a, measures an acid’s: A. concentration A. concentration B. strength B. strength C. number of protons C. number of protons D. degree of sourness D. degree of sourness #64

73. HNO 3 reacts with magnesium metal to give off the gas: A. oxygen A. oxygen B. nitrogen B. nitrogen C. hydrogen C. hydrogen D. no gas is given off D. no gas is given off #65

74. HNO 3 turns litmus paper: A. blue A. blue B. red B. red C. no color change C. no color change D. green D. green #66

75. What is the pH of 0.00100M HCl? A. 3 A. 3 B. 2 B. 2 C. 1.3 C. 1.3 D. 4 D. 4 #67

76. What affect does increasing the pH by 2 have on the hydronium ion concentration? A. Doubles it A. Doubles it B. Halves it B. Halves it C. Increases by power of 2 (100 times more) C. Increases by power of 2 (100 times more) D. Decreases by power of 2 (100 times less) D. Decreases by power of 2 (100 times less) #68

77. What is the pH of an acid if the hydronium ion concentration is 1 x 10 -4 M? A. 1 A. 1 B. 4 B. 4 C. 10 C. 10 D. 10000 D. 10000 #69

78. Determine the pH of a 0.00100M NaOH solution. A. 3 A. 3 B. 4 B. 4 C. 11 C. 11 D. 14 D. 14 #70

79. Pure water contains which of the following species? A. H 2 O molecules A. H 2 O molecules B. H 3 O + ions B. H 3 O + ions C. OH - ions C. OH - ions D. all of these D. all of these #71

80. Determine the hydroxide ion concentration of a solution with a pH of 13. A. 1.0 x 10 -13 A. 1.0 x 10 -13 B. 13 B. 13 C. 1 C. 1 D. 1.0 x 10 -1 D. 1.0 x 10 -1 #72

81. The definition of pH is: A. –log[H 3 O + ] A. –log[H 3 O + ] B. the percent of hydronium ions B. the percent of hydronium ions C. the parts per million of hydronium ions C. the parts per million of hydronium ions D. log[OH - ] D. log[OH - ] #73

82. Two common ways to measure pH are: A. with indicators and thermometers A. with indicators and thermometers B. with indicators and a pH meter B. with indicators and a pH meter C. by taste and color C. by taste and color D. by electric conductivity and by temperature D. by electric conductivity and by temperature #74

83. The equivalence point of a strong acid-strong base titration curve is: A. at a pH of 7 A. at a pH of 7 B. at the steepest part of the curve B. at the steepest part of the curve C. when the solution is neutral C. when the solution is neutral D. all of the above D. all of the above #75

84. Chemistry Final Exam Good Luck! Read CHAPTER SUMMARIES Complete the review package.