Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals a

Transcription

1 Chemistry Final Exam Review and Practice Chapters Covered ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 13, 14, 15, 16, 19, 20

2 Topics to Expect: Periodic Table: s, p, d, f blocks Metal, Metalloid, Non metal, etc. Periodic Trends, Family names Electron Configuration: Orbitals and SubLevels Bonding: covalent, ionic, Lewis dot diagrams Electron Configuration: Atomic #, mass, core notation Bonding: nonpolar covalent, polar covalent, 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. Shape and number of s and p orbitals. Number of electrons each orbital each sublevel and each level can hold. Location of s, p, d, f blocks on periodic table. Lewis dot diagrams. Formation of complete octets by transfer of / sharing of electrons.

4 Electron Configuration & Periodic Table Atomic Number Electrons, Protons and Neutrons Core notation using chemical symbol of preceding noble gas Trends for physical and chemical properties Atomic radii, ionization energy, electronegativity

5 Bonding Ionic versuscovalent Valence electrons and dot diagrams Lewis structures: shared pairs and lone pairs

6 Molecular Shapes and Polarity Recognize drawings of ball and stick models 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 Dispersion, dipole-dipole, hydrogen bonding: types of intermolecular forces in covalent compounds

7 Solutions Solubility Curves and Vocabulary

8 Acids, Bases and ph Self Ionization of Water and ph

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

10 What is the maximum number of electrons that can by held in an s sublevel? B. 2

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

12 What is the maximum # of e - that can by held in a p sublevel? C. 6

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

14 What is the total number of sublevel for n=2? B. 2

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

16 For an element whose electron configuration is [Ne]3s 2 3p 3, how many dots would the Lewis dot diagram have? B. 5

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

18 How many dots does the Lewis dot diagram for chlorine have? C. 7

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

20 A positive lithium ion is formed when a neutral lithium atom: D. loses one electron

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

22 When a potassium atom becomes an ion, it: D. loses one electron

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

24 When a calcium atom becomes an ion, it: D. loses two electrons

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

26 Use the periodic table to locate K; what block is it in? a. s-block

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

28 What does [Ar]4s 1 represent? b. the abbreviated electron configuration for K

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

30 What does Ar represent in [Ar]4s 1? c. the chemical symbol of the preceding noble gas

31 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 b. polar covalent c. ionic d. intermolecular

32 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

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

34 A bond is nonpolar covalent if the difference in electronegativities between the two atoms is: C. less than 0.4

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

36 Which of the following bonds would be considered completely nonpolar? B. O-O

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

38 For the diatomic molecule Cl 2, how many electron(s) does each chlorine share with the other A. 1 chlorine?

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

40 How many pairs of shared and unshared electrons does the Lewis dot structure for water have? C. 2, 2

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

42 In a double bond between two atoms, the number of shared electrons is: B. 4

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

44 In the compound ammonia, NH 3 : D. The Lewis structure will have one unshared pair of electrons

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

46 What kind of compound would form between nonmetallic atoms and non metallic atoms? D. Covalent

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

48 What kind of compound would form between polyatomic ions and metallic ions? C. Ionic

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

50 What kind of compound would form between metallic ions and nonmetallic ions? C. Ionic

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

52 What kind of compound would form between potassium and bromine?: C. Ionic

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

54 Predict the physical state of the compound formed between magnesium and oxygen: C. Probably a solid

55 The physical state of nearly all ionic compounds at the temperature of boiling water is: A. Solid B. liquid C. Gas D. Different for each ionic compound

56 The physical state of nearly all ionic compounds at the temperature of boiling water is: A. Solid

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

58 Ionic Compounds are generally: C. Formed when a metal transfers its valence electron to a nonmetal

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

60 How does a covalent bond differ from an ionic bond? A. Ionic: transfer of e - ; covalent: sharing of e -

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

62 Which theory is used to account for the shape of molecules? D. VSEPR theory

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

64 Which of the following does a ball and stick model reveal about chemical bonds? C. both A and B

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

66 What shape does an ammonia, NH 3, molecule have? A. pyramidal

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

68 What shape does a water molecule have? D. bent

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

70 In a molecule of carbon dioxide, what kind of bonds connect the carbon atom to the 2 oxygen atoms? D. two double bonds

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

72 What shape is a carbon dioxide molecule? A. linear

73 What shape is a methane molecule? A. tetrahedral B. bent C. trigonal planar D. pyramidal

74 What shape is a methane molecule? A. tetrahedral

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

76 What is the bond angle of a molecule of ammonia, NH 3? A. 107 o (<109.5 o )

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

78 What is the bond angle of a molecule of carbon dioxide? D. 180 o

79 What is the bond angle of a molecule of methane? A. 107 o B o C. 120 o D. 180 o

80 What is the bond angle of a molecule of methane? B o

81 What is the bond angle of a molecule of water? A. 90 o B. 105 o C. 107 o D o

82 What is the bond angle of a molecule of water? B. 105 o

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

84 Which of the following properties would you expect to find in a small nonpolar molecule? A. Gas at room temperature

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

86 In a pyramidal molecule, how many unshared pairs of valence electrons does the central atom have? B. One

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

88 In a tetrahedral molecule, how many unshared pairs of valence electrons does the central atom have? A. None

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

90 In polar bonds electrons are: A. Shared unequally

91 Dipoles are: A. Nonpolar bonds B. Polar bonds C. Nonpolar molecules D. Polar molecules

92 B. Polar bonds Dipoles are:

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

94 What determines the polarity of a bond? A. Electronegativity difference only

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

96 What determines the polarity of a molecule? C. Both A and B

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

98 How are the electrons shared in a bond between carbon & oxygen? C. Oxygen attracts them more

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

100 All solutions have the following properties except that the: D. Final physical state of a solution is a liquid

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

102 Which of the following statements applies to the dissolved solute particles in a solution? B. They will be in the same phase as the solvent

103 Which two substances are miscible in all proportions? A. Water and sugar B. Water and mineral oil C. Water and gasoline D. Water and ethanol

104 Which two substances are miscible in all proportions? D. Water and ethanol

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

106 An alloy is an example of a: C. Solid solution

107 All of the following are solutions except: A. Ocean water B. 14K gold bracelet C. antifreeze D. A concrete building block

108 All of the following are solutions except: D. A concrete building block

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

110 Solutions with water as the solvent are called: C. Aqueous solutions

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

112 Molarity is expressed as: C. Moles of solute / Liters of solution

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

114 A solution that contains as much solute as can possibly be dissolved under existing A. saturated conditions is said to be:

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

116 Which of the following is NOT an important factor influencing solubility? D. Volume of solution

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

118 Common nonpolar solvents include all of the following except: A. Salt water

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

120 Ionic solids best dissolve in liquid solvents that are: A. polar

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

122 Which of the following s solubility is most affected by pressure? C. Gases

123 Why can water dissolve NaCl, whereas hexane cannot? 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 C. Both water and salt are inorganic, while hexane is organic D. Water can form hydrogen bonds with NaCl

124 Why can water dissolve NaCl, whereas hexane cannot? B. As a polar solvent, water is attracted to both anions and cations

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

126 The rate at which a solid can be dissolved in a liquid solvent can be increased by: B. Grinding the solute into smaller pieces

127 To identify the strongest acid, compare the K a and: A. The highest 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 D. The K a closest to ph 0 is the strongest acid

128 To identify the strongest acid, compare the K a and: A. The highest K a value is the strongest acid

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

130 Substances that change color when added to acids or bases are called: A. indicators

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

132 The ionic compound formed in acid-base neutralization reactions is: B. a salt

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

134 A substance that can act as either an acid or a base is described as: D. amphoteric

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

136 Which of the following is least able to donate a proton? D. F -

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

138 Which of the following could be a conjugate acid-base pair? C. strong acid weak base

139 The K a for HCN is 6.2x What is the conjugate base for HCN in the following equation? HCN + H 2 O H 3 O + + CN - A. H 2 O, weak B. H 2 O, strong C. CN -, weak D. CN -, strong

140 The K a for HCN is 6.2x What is the conjugate base for HCN in the following equation? HCN + H 2 O H 3 O + + CN - D. CN -, strong

141 The acid dissociation constant measures an acid s: A. concentration B. strength C. number of protons D. degree of sourness

142 The acid dissociation constant measures an acid s: B. strength

143 Which 1M solution, hydrofluoric acid or formic acid, would have the greater H 3 O + concentration? A. the acid with more hydrogen atoms B. the acid with the higher K a C. the acid with the higher molar mass D. neither

144 Which 1M solution, hydrofluoric acid or formic acid, would have the greater H 3 O + concentration? B. the acid with the higher K a

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

146 HNO 3 reacts with magnesium metal to give off the gas: C. hydrogen

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

148 B. red HNO 3 turns litmus paper:

149 What is the ph of M HCl? A. 3 B. 2 C. 1.3 D. 4

150 What is the ph of M HCl? A. 3

151 What affect does increasing the ph have on the hydronium ion concentration? A. Doubles it B. Halves it C. Increases by power of 2 (10 times more) D. Decreases by power of 2 (10 times less)

152 What affect does increasing the ph have on the hydronium ion concentration? D. Decreases by power of 2 (10 times less)

153 What is the ph of an acid if the hydronium ion concentration is 2 x 10-4 M? A. 2 B. 3.7 C. 4.3 D. 4.7

154 What is the ph of an acid if the hydronium ion concentration is 2 x 10-4 M? B. 3.7

155 Determine the ph of a M NaOH solution. A. 3 B. 4 C. 11 D. 14

156 Determine the ph of a M NaOH solution. C. 11

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

158 Pure water contains which of the following species? D. all of these

159 Determine the hydroxide ion concentration of a solution with a ph of 13. A. 1.0 x B. 13 C. 1 D. 1.0 x 10-1

160 Determine the hydroxide ion concentration of a solution with a ph of 13. D. 1.0 x 10-1

161 The definition of ph is: A. log[h 3 O + ] B. the percent of hydronium ions C. the parts per million of hydronium ions D. log[oh - ]

162 The definition of ph is: A. log[h 3 O + ]

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

164 Two common ways to measure ph are: B. with indicators and a ph meter

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

166 The equivalence point of a strong acid-strong base titration curve is: D. all of the above

167 If phenolphtalein is used as an indicator in a titration of a strong acid with a strong base, at what point will the solution turn pink? A. before the equivalent point B. at the equivalence point C. after the equivalence point D. need more information

168 If phenolphtalein is used as an indicator in a titration of an acid with a base, at what point will the solution turn pink? C. after the equivalence point

169 Chemistry Final Exam Good Luck! ESSENTIALLY CUMMULATIVE List of Chapters: Ch: 6, 7, 8, 9, 10, 11, 13, 14, 15, 16, 19, 20 Read CHAPTER SUMMARIES Complete the review package.