AP Chemistry Test (Chapter 4) (Green Bean Casserole) Please use the answer sheet!!

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1 AP Chemistry Test (Chapter 4) (Green Bean Casserole) Please use the answer sheet!! Multiple Choice/FIB (50%) Please use the following choices to answer questions 1-6. A) Sugar (C 11 H 22 O 12 ) B) NH 4 F C) OF D) PbSO 4 E) H 2 O H) Butter (C x H y O z ) I) Alcohol (C x H y O z ) K) N 2 1) Please choose all polar covalent substances. 2) Please choose all nonpolar covalent substances. 3) Please choose all soluble substances. 4) Please choose all substances containing both ionic and covalent bonds. 5) Please choose all ionic substances. 6) Please choose all substances that will dissociate in water. 7) Which one best describes the water molecule? A) δ- H B) δ+ O δ- H δ- δ+ δ- H O H C) δ+ H D) δ- O δ+ δ- δ+ H O H δ+ H 8) Please choose all false statements. A) All ionic substances dissociate in water. B) Water is polar covalent. C) All polar covalent substances dissociate in water. D) All nonpolar covalent substances are soluble in water. E) All polar covalent substances dissolve in water.

2 9) Please choose all true statements. A) Water dissociates in water. B) Soluble polar covalent substances dissociate in water. C) Soluble ionic substances dissociate in water. D) All nonpolar covalent substances are insoluble in water. E) Nonpolar covalent substances dissociate in water. 10) Please choose all true statements. A) Ionic formula units have extreme dipoles. B) Oil has slight dipoles. C) Water has no dipoles. D) N 2 has no dipoles. E) AlCl 3 has slight dipoles. 11) Please choose all true statements. A) Atoms in an ionic bond have extreme dipoles because the atoms transfer valence electrons completely. B) Atoms in a nonpolar covalent bond have no dipoles because the atoms share valence electrons equally. C) Atoms in a polar covalent bond have slight dipoles because the atoms share valence electrons unequally. D) Atoms in a polar covalent bond have slight dipoles because the atoms share valence electrons equally. E) Atoms in an ionic bond have no dipoles because the atoms share electrons unequally. Please use the following choices to answer questions A) Ca(OH) 2 B) H 2 SO 4 C) H 2 Cr 2 O 7 D) Al 2 (C 2 O 4 ) 3 E) Sugar (C 11 H 22 O 12 ) H) Zn(OH) 4 I) CuI 2 K) Mn(C 2 H 3 O 2 ) 5 12) Please choose all weak electrolytes. 13) Please choose all nonelectrolytes. 14) Please choose all strong electrolytes. 15) Which one best describes a nonelectrolyte? A) An ionic compound with a low lattice energy produces ions in the solution. B) An ionic compound with a high lattice energy produces ions in the solution. C) A polar covalent compound produces ions in the solution. D) A covalent compound produces no ions in the solution. E) A strong acid or base produces no ions in the solution.

3 16) Which one best describes a weak electrolyte? A) A strong acid or base yields a small percentage of ions in the solution. B) A weak acid or base yields a small percentage of ions in the solution. C) An ionic compound with a low lattice energy yields a small percentage of ions in the solution. D) A polar covalent compound yields a small percentage of ions in the solution. E) A polar covalent compound yields a large percentage of ions in the solution. 17) Which one best describes a strong electrolyte? A) An ionic compound with a small lattice energy yields a large percentage of ions in the solution. B) A polar covalent compound yields a small percentage of ions in the solution. C) A polar covalent compound yields a large percentage of ions in the solution. D) An ionic compound with a large lattice energy yields a large percentage of ions in the solution. E) A weak acid or base yields a small percentage of ions in the solution. 18) Which reaction will cause the light bulb on a conductivity tester to glow the brightest if neither reactant is limiting or excess? A) Al(OH) 3 (s) + 3 HClO 3 (aq) 3 HOH + Al(ClO 3 ) 3 B) 2 O 2 (g) + N 2 (g) 2 NO 2 (g) C) K 2 C 2 O 4 (aq) + 2 HClO 4 (aq) 2 KClO 4 + H 2 C 2 O 4 D) Pb(OH) 4 (aq) + 4 HI (aq) PbI HOH E) 2 Al(OH) 3 (s) + 3 CaCl 2 (aq) 2 AlCl Ca(OH) 2 19) Which one is the formula for the precipitate that forms when aqueous copper (II) sulfate is mixed with aqueous sodium phosphate? A) Na 3 PO 4 B) Cu 3 (PO 4 ) 2 C) Na 2 SO 4 D) CuPO 4 E) None of these 20) Which one would be most appropriate for making exactly 500 ml of a solution? A) Graduated cylinder and volumetric flask B) Beaker and graduated cylinder C) Buret and graduated cylinder D) Buret and volumetric flask E) Beaker and volumetric flask 21) What is the oxidation number of P in the P 3 O 8 4 ion? A) +12 B) -3 C) +4 D) +3 E) None of these

4 Please consider the following reaction to answer questions N 2 O (g) + ClO (aq) Cl (aq) + NO 2 (aq) 22) What species is reduced? 23) What element is oxidized? 24) What species loses electrons? 25) What element is the oxidizing agent? Free Response (66%) Please show all your work for any credit!! 1) A g sample of copper is dissolved in a small amount of HNO 3 to form Cu 3+ ions in solution. The resulting solution is diluted to a total volume of ml. Please calculate the molarity of the Cu 3+ ions. 2) How would you prepare ml of a M H 2 SO 4 solution from a stock solution of 16.0 M? 3) Please calculate the concentration of all ions in a M Fe 2 (SO 4 ) 5 solution. 4) You evaporate 50.0 ml of M Na 2 Cr 2 O 7 solution to dryness. What mass of Na 2 CrO 7 will be present? Please consider the following information to answer questions Cr(ClO 3 ) Na 2 C 2 O 4 10 NaClO 3 + Cr 2 (C 2 O 4 ) ml of M Cr(ClO 3 ) 5 is slowly added to ml of M Na 2 C 2 O 4. A chemistry student collects and dries the precipitate. The precipitate has a mass of g. 5) How many moles of limiting reagent are consumed? 6) Please calculate the % yield of the precipitate and give a likely source of error to explain the % yield. 7) Please calculate the concentration of the excess reagent after the reaction is complete. 8) An g impure sample of Al 2 (CO 3 ) 3 is titrated with 30.0 ml of M HCl until the reaction appears to be complete. What is the mass % Al 2 (CO 3 ) 3 in the impure sample? Al 2 (CO 3 ) HCl 2 AlCl H 2 O + 3 CO 2

5 9) A solution is 15.4 M H 2 C 2 O 4. The solution has a density of 1.12 g/ml. What is the mass % of H 2 C 2 O 4? 10) A ml sample of a M CaCl 2 solution is accidentally left on a hot plate overnight. The next morning, the solution is M. What volume of water evaporated from the original solution of CaCl 2? 11) What volume of M Al(NO 3 ) 3 solution is necessary to completely react with ml of M H 2 C 2 O 4 solution? 2 Al(NO 3 ) H 2 C 2 O 4 6 HNO 3 + Al 2 (C 2 O 4 ) 3

6 AP Chemistry Test (Chapter 4) (Turkey and Dressing) Please use the answer sheet!! Multiple Choice/FIB (50%) Please use the following choices to answer questions 1-6. A) PbSO 4 B) Alcohol (C x H y O z ) C) N 2 D) Sugar (C 11 H 22 O 12 ) E) Butter (C x H y O z ) H) H 2 O I) NH 4 F K) OF 1) Please choose all polar covalent substances. 2) Please choose all nonpolar covalent substances. 3) Please choose all soluble substances. 4) Please choose all substances containing both ionic and covalent bonds. 5) Please choose all ionic substances. 6) Please choose all substances that will dissociate in water. 7) Which one best describes the water molecule? A) δ+ H B) δ- O δ+ H δ- δ+ δ- H O H C) δ- H D) δ+ O δ+ δ- δ+ H O H δ- H 8) Please choose all false statements. A) All polar covalent substances dissolve in water. B) Water is polar covalent. C) All polar covalent substances dissociate in water. D) All nonpolar covalent substances are soluble in water. E) All ionic substances dissociate in water.

7 9) Please choose all true statements. A) Water dissociates in water. B) Soluble polar covalent substances dissociate in water. C) Nonpolar covalent substances dissociate in water. D) All nonpolar covalent substances are insoluble in water. E) Soluble ionic substances dissociate in water. 10) Please choose all true statements. A) Water has no dipoles. B) Oil has slight dipoles. C) Ionic formula units have extreme dipoles. D) N 2 has no dipoles. E) AlCl 3 has slight dipoles. 11) Please choose all true statements. A) Atoms in an ionic bond have no dipoles because the atoms share electrons unequally. B) Atoms in a nonpolar covalent bond have no dipoles because the atoms share valence electrons equally. C) Atoms in a polar covalent bond have slight dipoles because the atoms share valence electrons equally. D) Atoms in a polar covalent bond have slight dipoles because the atoms share valence electrons unequally. E) Atoms in an ionic bond have extreme dipoles because the atoms transfer valence electrons completely. Please use the following choices to answer questions A) Zn(OH) 4 B) H 2 SO 4 C) Al 2 (C 2 O 4 ) 3 D) H 2 Cr 2 O 7 E) Mn(C 2 H 3 O 2 ) 5 H) CuI 2 I) Ca(OH) 2 K) Sugar (C 11 H 22 O 12 ) 12) Please choose all weak electrolytes. 13) Please choose all nonelectrolytes. 14) Please choose all strong electrolytes. 15) Which one best describes a nonelectrolyte? A) An ionic compound with a low lattice energy produces ions in the solution. B) An ionic compound with a high lattice energy produces ions in the solution. C) A covalent compound produces no ions in the solution. D) A polar covalent compound produces ions in the solution. E) A strong acid or base produces no ions in the solution.

8 16) Which one best describes a weak electrolyte? A) A weak acid or base yields a small percentage of ions in the solution. B) A strong acid or base yields a small percentage of ions in the solution. C) An ionic compound with a low lattice energy yields a small percentage of ions in the solution. D) A polar covalent compound yields a small percentage of ions in the solution. E) A polar covalent compound yields a large percentage of ions in the solution. 17) Which one best describes a strong electrolyte? A) An ionic compound with a large lattice energy yields a large percentage of ions in the solution. B) A polar covalent compound yields a small percentage of ions in the solution. C) A polar covalent compound yields a large percentage of ions in the solution. D) An ionic compound with a small lattice energy yields a large percentage of ions in the solution. E) A weak acid or base yields a small percentage of ions in the solution. 18) Which reaction will cause the light bulb on a conductivity tester to glow the brightest if neither reactant is limiting or excess? A) Al(OH) 3 (s) + 3 HClO 3 (aq) 3 HOH + Al(ClO 3 ) 3 B) 2 Al(OH) 3 (s) + 3 CaCl 2 (aq) 2 AlCl Ca(OH) 2 C) K 2 C 2 O 4 (aq) + 2 HClO 4 (aq) 2 KClO 4 + H 2 C 2 O 4 D) Pb(OH) 4 (aq) + 4 HI (aq) PbI HOH E) 2 O 2 (g) + N 2 (g) 2 NO 2 (g) 19) Which one is the formula for the precipitate that forms when aqueous copper (II) sulfate is mixed with aqueous sodium phosphate? A) Na 3 PO 4 B) CuPO 4 C) Na 2 SO 4 D) Cu 3 (PO 4 ) 2 E) None of these 20) Which one would be most appropriate for making exactly 500 ml of a solution? A) Beaker and volumetric flask B) Beaker and graduated cylinder C) Buret and graduated cylinder D) Buret and volumetric flask E) Graduated cylinder and volumetric flask 21) What is the oxidation number of P in the P 3 O 8 4 ion? A) +3 B) +12 C) -3 D) +4 E) None of these

9 Please consider the following reaction to answer questions Cl (aq) + NO 2 (aq) N 2 O (g) + ClO (aq) 22) What species is reduced? 23) What element is oxidized? 24) What species loses electrons? 25) What element is the oxidizing agent? Free Response (66%) Please show all your work for any credit!! 1) A g sample of copper is dissolved in a small amount of HNO 3 to form Cu 3+ ions in solution. The resulting solution is diluted to a total volume of ml. Please calculate the molarity of the Cu 3+ ions. 2) How would you prepare ml of a M H 2 SO 4 solution from a stock solution of 18.0 M? 3) Please calculate the concentration of all ions in a M Fe 2 (SO 4 ) 5 solution. 4) You evaporate 70.0 ml of M Na 2 Cr 2 O 7 solution to dryness. What mass of Na 2 CrO 7 will be present? Please consider the following information to answer questions Cr(ClO 3 ) Na 2 C 2 O 4 10 NaClO 3 + Cr 2 (C 2 O 4 ) ml of M Cr(ClO 3 ) 5 is slowly added to ml of M Na 2 C 2 O 4. A chemistry student collects and dries the precipitate. The precipitate has a mass of g. 5) How many moles of limiting reagent are consumed? 6) Please calculate the % yield of the precipitate and give a likely source of error to explain the % yield. 7) Please calculate the concentration of the excess reagent after the reaction is complete. 8) An g impure sample of Al 2 (CO 3 ) 3 is titrated with 20.0 ml of M HCl until the reaction appears to be complete. What is the mass % Al 2 (CO 3 ) 3 in the impure sample? Al 2 (CO 3 ) HCl 2 AlCl H 2 O + 3 CO 2

10 9) A solution is 17.4 M H 2 C 2 O 4. The solution has a density of 1.12 g/ml. What is the mass % of H 2 C 2 O 4? 10) A ml sample of a M CaCl 2 solution is accidentally left on a hot plate overnight. The next morning, the solution is M. What volume of water evaporated from the original solution of CaCl 2? 11) What volume of M Al(NO 3 ) 3 solution is necessary to completely react with ml of M H 2 C 2 O 4 solution? 2 Al(NO 3 ) H 2 C 2 O 4 6 HNO 3 + Al 2 (C 2 O 4 ) 3

11 AP Chemistry Test (Chapter 4) Form Name Multiple Choice/FIB (50%) 1) 16) 2) 17) 3) 18) 4) 19) 5) 20) 6) 21) 7) 22) 8) 23) 9) 24) 10) 25) 11) 12) 13) 14) 15) Problems (66%) 1) Please use only the front side of each piece of paper. 2) Please number your problems clearly and consecutively. 3) Please staple your problems to the back of this page in numerical order. 4) Please write on the paper in the conventional manner. 5) Please do not make a separate list of answers. Record your answer at the end of the work supporting your answer. 6) Please circle/box your answer.

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