AP Chemistry Summer Assignment

AP Chemistry Summer Assignment 1) Name this compound: Cr 3 (PO 4 ) 2 a) Chromium Diphosphate b) Trichromium Phosphate c) Chromium (II) Phosphate d) Chromium (II) Diphosphate 2) How many significant figures are there: 0.00340 a) 6 b) 3 c) 5 d) 2 3) The nucleus of an atom contains a) Electrons and neutrons b) Electrons and protons c) Protons and neutrons d) All three 4) What is the correct name for LiCl? a) lithium chloride b) Monolithium monochloride c) Dilithium Chloride d) Lithium dichloride 5. How many significant figures would there be for the answer to the calculation? 2.25 x (9.135 x 3.5) + 3.456 x (2 x 4.5) a) 1 b) 2 c) 3 d) 4 6. How much 10.0M of NaCl would you need to create a 50mL solution of 0.10M NaCl a) 5mL b) 10mL c) 2 ml d) 6mL 7. Convert 12 grams of oxygen gas (O 2 ) into moles using stoichiometry. A. 0.421 moles B. 0.375 moles C. 0. 579 moles D. 0.118 moles 8. Find the answer using the right number of significant 8.2087 ml + 2.430 ml + 0.09 ml A. 11.7287 B. 11.728 C. 11.73 D. 11.72 9. Round the following number to three significant 0.9976 grams A. 0.997 grams B. 0.99 grams C. 0.998 grams D. 0.989grams 10. Density is expressed in a. Decantation b. Grams/mL c. Moles/Kilogram d. Cal/g*c 11. The general formula for a double replacement reaction is a. A + B à AB b. AB à A + B c. AB + C à CB + A d. AB + CD à AD + CB 12. The number 0.032040 has significant figures. a. 4 b. 6 c. 3 d. 7 e. 5 13. Equation: 4!"# $ 4!"# ' + 2# ' How many grams of # ' are produced from 138 g of!"# $? a) 105.9 grams b) 40.3 grams c) 21.8 grams d) 4.8 grams

14. Write a chemical equation for the following circumstance: When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. a) 3,./ + 3"0, + 3"0./ b),./ ' + 2"0, + 2 "0./ c),./ + "0, + "0./ d),./ ', +./ 15. Which equation below is correctly balanced? e) # $ # ' f) "1 2 "# $ " ' # + 1 ' # g) 2.# + # ' 2.# ' h).3(#1) $ + 1./# 2.3(./# 2 ) $ + 1 ' # 16. What is the electron configuration for Iron? A: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 1 B: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5 C: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 D: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 17. Draw the Lewis structure of O 2. A: B: C: D: 18. What is the final volume from the dilution of 538.0mL of 2.573M H 2 SO 4 to 1.437M H 2 SO 4? A. 962mL B. 963mL C..964L D. 9.63L 19. Which ionic molecule is nonsoluble? A. NaO B. Ca(OH) 2 C. MgF 2 D. AgCl 20. What is the final volume of a gas if it is in a 5.6L sealed container with 1.48 atm at 25 o C and the pressure increased to 2.56 atm while the temperature also increases to 90 o C? A. 3.94L B. 11.655L C..394L D. 1165mL 21. Which compound fully dissociates? A. HSO 4 B. HClO 2 C. HCl D. HNO 2 22. Which compound has the smallest bond angle? A. CH 4 B. PCl 5 C. H 2 O D. PF 3 23. What volume of 0.50 M HCl solution is needed to create 20 ml of 0.05 M HCl solution? a. 10 ml b. 5 ml c. 2 ml d. 1 ml 24. How many ml s of water are needed to satisfy the proposed situation above? a. 18 ml b. 13 ml c. 5 ml d. 2 ml 25. The following reaction is an example of what type of reaction? KBr (aq) + AgNO 3 (aq) à AgBr (s) + KNO 3 a. Single displacement b. Double displacement c. Synthesis d. Decomposition e. Combustion 26. How many moles of KNO 3 exist in 5 L of 0.2 M KNO 3 solution? a. 0.04 b. 1 c. 2.5 d. 10

27. How many moles of carbon are in 50.0g of carbon? (C s molar mass = 12.01 g/mole) a. 0.240 b. 2.65 c. 4.16 d. 605 28. How many significant figures does 300 have? a. 0 b. 1 c. 2 d. 3 29. What is 25 C in Kelvin? a. 248 K b. 100 K c. 298 K d. 325 K 30. True or False: It is possible to have negative Kelvin. a. True b. False 31. What is the ph of a solution with a [H 3 O + ] = 5.61x10 8 M? a. 4.39 b. 5.82 c. 7.25 d. 11.3 32. What is the percentage of carbon in glucose? (C 6 H 12 O 6 ) a. 25% b. 40% c. 50% d. 72% 33. What is the electron configuration of nitrogen? a. 1s 2 2s 2 2p 3 b. 1s 1 2s 1 2p 3 3p 2 c. 1p 2 2p 2 2s 3 d. 1s 2 2s 2 2p 6 34. What is the electron configuration of N 3? a. 1s 2 2s 2 2p 3 b. 1s 2 2s 2 2p 6 c. 1p 2 2p 2 2s 6 d. 1s 1 2s 1 2p 3 3p 2 35. The number of valence electrons that an element has is based on its: A. Group number (vertical columns) B. Period (horizontal row) C. Mass 36. There are orbital types when writing electron configurations: A. 5 (S, P, D, F, G) B. 4 (S, P, D, F) C. 3 (S, P, D) 37. form when atoms gain or lose electrons: A. Ions B. Ionic compounds C. Covalent compounds 38. A 20 gram sample has a halflife of 15 years. How long does it take for half of the sample to remain? How long does it take for 5 grams to remain? A. 15 years, 25 years B. 25 years, 30 years C. 15 years, 30 years 39. An ionic compound: A. Consists of a metal + a nonmetal or a metal + a poly atomic ion B. Consists of two metals C. Consists of two nonmetals or a nonmetal + a poly atomic ion 40. A covalent compound: A. Consists of a metal + a nonmetal B. Consists of a poly atomic ion + a metal C. Consists of two nonmetals 41. Solubility refers to and the symbol for a soluble substance is : A. The ability of a substance to dissolve in water, aq B. The percentage of salt in a substance, s C. How acidic a substance is, a 42. bonds are primarily responsible for holding water molecules together in the liquid state: A. Hydrogen B. Oxygen C. Carbon 43. bonds are the strongest and closest together: A. Single B. Double C. Triple

44. A diatomic molecule is: A. A molecule with two atoms of the same element (N 2, O 2, F 2, Cl 2, Br 2, I 2, H 2 ) B. A molecule with two different elements of the same numerical charge (H +1 +F 1, Ca +2 +O +2, Al +3 +N 3 ) C. Not real 45. Which reaction is correctly balanced: A. 2Al +3 + 3Cl 2 1 à2alcl 3 B. 2Ca +2 + 2HBRà2CaBr 2 + 1H 2 C. 3CO + O 2 2 à2co 2 46. Which of the following is an oxidation reaction? A. Ca +2 + 2e à Ca B. Ca à Ca +2 + 2e C. Ca +2 + 2e + Ca à 0 47. Which of the following is a reduction reaction? A. Cl 2 + 2e à 2Cl B. 2Cl à Cl 2 + 2e C. 2Cl + 2e + Cl à 0 48. What is the electron configuration of Al? a) 1s 2 2s 2 2p 6 3s 2 3p 6 b) 1s 2 2s 2 2p 6 3s 2 3p 1 c) 1s 2 2s 2 2p 6 3s 2 d) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 49. What is the molecular weight of CO 2? a. 44.01 g b. 22.01g c. 42.01g d. 43.01g 50. What is the molecular weight of NaCl? a. 58.44 g b. 59.44g c. 49.44g d. 48.44g 51. Which of the following is NOT Acetate? A: C 2 H 3 O 2 B: C 2 H 3 O 2 2 C: CH 3 COO D: all of the above 53. Which of the following bond angles are incorrect? a. linear 180 trigonal planar 120 tetrahedral 100 trigonal pyramidal 90 octahedral 90 b. linear 120 trigonal planar 180 tetrahedral 109.5 trigonal pyramidal 120/90 octahedral 90 c. linear 180 trigonal planar 120 tetrahedral 109.5 trigonal pyramidal 90/120 octahedral 90 D: linear 180 trigonal planar 120 tetrahedral 109 trigonal pyramidal 90/120 octahedral 90 54. Equation: 4!"# $ 4!"# ' + 2# ' How many grams of # ' are produced from 138 g of!"# $? a. 105.9 grams b. 40.3 grams c. 21.8 grams d. 4.8 grams 55. Write a chemical equation for the following circumstance: When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. a. 3,./ + 3"0, + 3"0./ b.,./ ' + 2"0, + 2 "0./ c.,./ + "0, + "0./ d.,./ ', +./ 56. Which equation below is correctly balanced? a) # $ # ' b) "1 2 "# $ " ' # + 1 ' # c) 2.# + # ' 2.# ' d).3(#1) $ + 1./# 2.3(./# 2 ) $ + 1 ' # 57. What is the electron configuration for Titanium? a. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 38 ' b. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 4: ' c. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 3: ;< d. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 3: ' 52. What type of bond is the longest? A: single bonds B: double bonds C: triple bonds D: all the same length

58. Find the molarity: 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution. a. 1 M b. 10 M c. 5 M d. 8 M 59. Calculate the percent composition of silver in AgCl. a. 75.3% b. 97.3% c. 24.7% d. 45.8% 60. Which states of matter are significantly compressible? a. Solids only b. Solids & Liquids c. Liquids & Gases d. Gases only 61. Homogeneous mixtures are also known as a. Solids b. Solutions c. Compounds d. Substances 62. Gases and Liquids share the property of a. Definite shape b. Compressibility c. Indefinite shape d. Incompressibility 63. Which element is a metal? a) Carbon b) Phosphorus c) Krypton d) Yttrium 64. Which group consists of the alkali earth metals? a. 16 b. 18 c. 2 d. 7 65. Which element would have atoms with the same number of outer electrons as carbon atoms? a. Silicon b. Boron c. Nitrogen d. Neon 66. Name this compound: Cr 3 (PO 4 ) 2 a. Chromium Diphosphate b. Trichromium Phosphate c. Chromium (II) Phosphate d. Chromium (II) Diphosphate 67. How many significant figures are there: 0.00340 a. 6 b. 3 c. 5 d. 2 68. The nucleus of an atom contains a. Electrons and neutrons b. Electrons and protons c. Protons and neutrons 69. What and where are the families on the periodic table? A: Alkali Metals col. 2, Alkaline Earth Metals col.1, Halogens col. 17, Noble Gases col. 18, Transition metals col. 316 B: Alkali Metals col. 2, Alkaline Earth Metals col.1, Halogens col. 17, Noble Gases col. 18, Transition metals col. 216 C: Alkali Metals col. 1, Alkaline Earth Metals col. 2, Halogens col. 17, Noble Gases col. 18, Transition metals col. 316 D: Alkali Metals col. 1, Alkaline Earth Metals col. 2, Halogens col. 17, Noble Gases col. 18, 70. Which Periodic table trend increases to the right and up? a. Electronegativity, Ionic Radii, Ionization Energy b. Metallic Ionic Radii, Ionization Energy c. Electronegativity, Ionization Energy, Nonmetallic d. Metallic, Atomic Radii, Electronegativity 71. What are the alkane prefixes for 15? a. Meth, Eth, Prop, But, Pentb. Meth, Prop, Pent, Hex, Heptc. Hex, Hept, Oct, Non, Decd. Pent, Hex, Hep, Oct, Non 72. What is the General Format of a Synthesis reaction? a. AB + CD à AD + CB b. element + element à compound c. compound à element + element d. A + BC à AC + B 73. WHAT IS THE OXIDATION STATE OF C IN CO 2? a. 4+ b. 2+ c. 2 d. 4

74. WHAT IS THE MOLE TO LITER RATIO? a. 1 mole = 22.2 liters b. 1 mole = 22.4 liters c. 1 mole = 24.2 liters d. 1 mole = 24.4 liters 75. What is the electron configuration of F? a) 1s 2 2s 2 2p 6 b) 1s 2 2s 2 2p 5 c) 1s 2 2s 2 2p 4 d) 1s 2 2s 2 2p 3 75. What is the molecular weight of H 2 O? a. 18.02 g b. 20.02g c. 22.02g d. 24.02g 77. How many Significant figures would there be for the answer to the calculation? 4.908*5.76 + 7.2345*2 a) 3 b) 2 c) 1 d) 4 78. Equation: 4!"# $ 4!"# ' + 2# ' How many grams of # ' are produced from 138 g of!"# $? a. 105.9 grams b. 40.3 grams c. 21.8 grams d. 4.8 grams 79. Write a chemical equation for the following circumstance: When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. a. 3,./ + 3"0, + 3"0./ b.,./ ' + 2"0, + 2 "0./ c.,./ + "0, + "0./ d.,./ ', +./ 80. Which equation below is correctly balanced? a. # $ # ' b. "1 2 "# $ " ' # + 1 ' # c. 2.# + # ' 2.# ' d..3(#1) $ + 1./# 2.3(./# 2 ) $ + 1 ' # 81. What is the electron configuration for Titanium? a. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 38 ' b. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 4: ' c. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 3: ;< d. 17 ' 27 ' 28 9 37 ' 38 9 47 ' 3: ' 82. Find the molarity: 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution. a. 1 M b. 10 M c. 5 M d. 8 M 83. Calculate the percent composition of silver in AgCl. a. 75.3% b. 97.3% c. 24.7% d. 45.8% 84. Which of the elements below has the highest electronegativity? a. Potassium b. Lithium c. Hydrogen d. Nitrogen 85. As you move up and to the right on the periodic table: a. Atomic radius increases and electronegativity decreases b. Atomic radius decreases and electronegativity increases c. Atomic radius increases and electronegativity increases d. Atomic radius decreases and electronegativity decreases 86. Choose ALL intermolecular forces that are in 1 ' #? a. Hydrogen bonding b. Hydrogen bonding, dipoledipole bonding c. Dispersion forces d. Hydrogen bonding, dipoledipole bonding, dispersion forces 87. What is the final volume from the dilution of 538.0mL of 2.573M H 2 SO 4 to 1.437M H 2 SO 4? A. 962mL B. 963mL C..964L D. 9.63L 88. Which ionic molecule is nonsoluble? A. NaO B. Ca(OH) 2 C. MgF 2 D. AgCl

89. What is the final volume of a gas if it is in a 5.6L sealed container with 1.48 atm at 25C and the pressure increased to 2.56 atm while the temperature also increases to 90C? A. 3.94L B. 11.655L C..394L D. 1165mL 90. Which compound fully dissociates? A. HSO 4 B. HClO 2 C. HCl D. HNO 2 91. Which compound has the smallest bond angle? A. CH 4 B. PCl 5 C. H 2 O D. PF 3 92. In the ionic compound magnesium fluoride, what is the ratio of the two elements necessary so that each element obtains its octet from the transfer of electrons? a. 1 magnesium : 2 fluorine b. 3 magnesium : 1 fluorine c. 2 magnesium : 1 fluorine d. 1 magnesium : 1 fluorine 93. which is the Bronsted Base in the following equilibrium reaction? 96. What is the VESPR Electron based bond shape of this molecule? a. Trigonal Pyramidal b. Linear c. TShaped d. Square Planar 97. What is the VESPR Electron based bond angle of this molecule? a. 180 b. 120 c. 109.5 d. 90 98. What are the bond pairs in the shape above? A. CH 3 COOH CH 3 COOH + H 2 O ß> H 3 O + + CH 3 COO B. H 2 O C. H 3 O + D. CH 3 COO 94. What is the Bronsted acid in the following equilibrium reaction? HCO 3 + H 2 O ß> OH + H 2 CO 3 A. H 2 O B. H 2 CO 3 C. HCO 3 D. OH 95. What is the oxidation number of Al in Al + I 2 à AlI 3? A. 0 B. 3 C. 3 D. 2 a. 5 bonds, 1 lone pair b. 6 bonds, 0 lone pairs c. 2 bonds, 3 lone pairs d. 4 bonds, 1 lone pair 99. How much 5.0 M of KF would you need to create a 50 ml solution of 0.20 M of KF? a. 0.50 ml b. 20mL c..10ml d..20ml 100. What is the molecular weight of CO? a. 28.01 g b. 30.0g c. 16.0g d. 12.01g

101. What is the electron configuration of an O 2 ion? a) 1s 2 2s 2 2p 4 b) 1s 2 2s 2 2p 5 c) 1s 2 2s 2 2p 3 d) 1s 2 2s 2 2p 6 102. A tshaped molecule has how many bonding pairs and lone pairs of electrons, respectively? a) 4 1 b) 3 2 c) 2 2 d) 4 0 103. What is the electron configuration of a Cl ion? a) 1s 2 2s 2 2p 6 3s 2 3p 5 b) 1s 2 2s 2 2p 6 3s 2 3p 4 c) 1s 2 2s 2 2p 6 3s 2 3p 6 d) 1s 2 2s 2 2p 6 3s 2 104. What is the molarity of 100 ml of a 0.10 M NaOH solution after being diluted with 50 ml of water? a) 0.66 M b) 0.015 M c) 0.15 M d) 0.067 M 105. What is the empirical for a Chromium Oxide that was found to contain 52 grams of Chromium and 32 grams of Oxygen? a) CrO 2 b) Cr 2 O c) CrO 3 d) Cr 2 O 3 106. What is the oxidation number of Sulfur in the compound H 2 SO 4? a) 6+ b) 6 c) 2+ d) 1+ 107. If the concentration of H + ions is greater than the concentration of OH ions the solution is: a) Basic b) Acidic c) Neutral d) It is impossible to tell from this given information. 109. Find the answer using the right number of significant 8.2087 ml + 2.430 ml + 0.09 ml a. 10.7287 b. 10.728 c. 10.73 d. 10.72 110. Round the following number to three significant 0.9976 grams a. 0.997 grams b. 0.99 grams c. 0.998 grams d. 0.989grams 111. Convert 10.65 grams of sulfur into moles. a. 0.322 moles b. 0.324 moles c. 0.456 moles d. 0.566 moles 112. Find the answer using the right number of significant 9.40 g + 3.520 g + 1.8 g a. 14.00g b. 14g c. 14.3 g d. 14.72g 113. Round the following number to three significant a. 9.00 g b. 8.77g c. 8.87g d. 9.11g 8.76532grams 108. Convert 12 grams of Oxygen gas (O 2 ) into moles. a. 0.421 moles b. 0.375 moles c. 0. 579 moles d. 0.118 moles

114. What VSPER shape is the following image representing? a. Bent b. Tetrahedral c. Trigonal Planar d. Linear 115. What VSPER shape is the following image representing? a. Tetrahedral b. Trigonal Pyramidal c. Trigonal Planar d. Bent 116. Which of the following elements could be represented in the following image? 119. What is the final volume of a gas if it is in a 5.6L sealed container with 1.48 atm at 25 o C and the pressure increased to 2.56 atm while the temperature also increases to 90 o C? A. 3.94 L B. 11.655 L C..394 L D. 1165 ml 120. Which compound fully dissociates? A. HSO 4 B. HClO 2 C. HCl D. HNO 2 121. Which compound has the smallest bond angle? A. CH 4 B. PCl 5 C. H 2 O D. PF3 122. In the ionic compound magnesium fluoride, what is the ratio of the two elements necessary so that each element obtains its octet from the transfer of electrons? a. 1 magnesium : 2 fluorine b. 3 magnesium : 1 fluorine c. 2 magnesium : 1 fluorine d. 1 magnesium : 1 fluorine 123. what is the oxidation number of Al in Al + I 2 > AlI 3? A. 0 B. 3 C. 3 D. 2 a. H 2 O b. NH 3 c. BCl 3 d. BeCl 2 117. What is the final volume from the dilution of 538.0mL of 2.573M H 2 SO 4 to 1.437M H 2 SO 4? A. 962 ml B. 963 ml C..964 L D. 9.63 L 118. Which ionic molecule is nonsoluble? A. NaO B. Ca(OH) 2 C. MgF 2 D. AgCl 124. Of the following, the smallest and lightest subatomic particle is the. A. neutron B. proton C. alpha particle D. electron 125. All atoms of a given element have the same. A. number of protons B. density C. mass D. number of electrons and neutrons 126. Which atom has the largest number of neutrons? A. phosphorus30 B. calcium40 C. potassium39 D. argon40

127. Which atom is being oxidized in the reaction? Mg + 2HCl à MgCl 2 + H 2 a) Mg b) HCl c) MgCl 2 d) H 2 128. What is the correct formula for this chemical compound? Iron (II) hydroxide a. 2FeH 2 b. Fe(OH) 2 c. Fe 2 OH 2 d. Fe 2 H 2 129. What is the strongest form of radiation? a. Alpha b. Beta c. Gamma d. Delta 130. The law of constant composition applies to. a. Solids b. compounds c. heterogeneous mixtures d. solutions 131. An element cannot. a. be a pure substance b. be part of a homogeneous mixture c. be part of a heterogeneous mixture d. be separated into other substances by chemical means 132. Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gases 4. compression of oxygen gas a. 1, 3 b. 2, 3, 4 c. 1, 4 d. 1, 3, 4