16-exam4

16-exam4 - CHEMISTRY 16 EXAM IV Dr M Richards-Babb(Version...

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Unformatted text preview: CHEMISTRY 16 EXAM IV Dr. M. Richards-Babb July 31, 1998 (Version I) An optical scoring machine will grade this examination. The machine is not programmed to accept the correct one of two sensed answers and will not sense answers which are lightly marked. Mark your answer sheet carefully with a No. 2 soft lead pencil and erase any undesired marks COMPLETELY. Avoid making any extraneous marks on the answer sheet other than the information requested below. A On the answer sheet: 1. Print your name in the space for NAME (last name first, circle your last name). ‘ 2. In the space marked SUBJEC'I: print your student number. 3. In the space marked HOUR print Summer II ‘98. Check to see that you have 20 examination questions, periodic table and scratch paper when the exam begins. HAND IN ONLY THE ANSWER SHEET. Useful Equations and Constants: KW=1.O><10"4 at 25°C CHEM l6 EXAM IV CHOOSE THE ONE BEST ANSWER 1. A solution is saturated with AlPO4. Addition of which of the following will cause a decrease in the solubility of AlPO4? I—INO3 AlCl3 Na3PO4 NaCl A. All will cause an increase. B. HNO, ' C. NaaPO4 and NaCl D. HN03, AlCl3, and Na3PO4 E. AlCl3 and Na3PO4 2. The pH of a saturated solution of Mn(OH)2 is: Ksp(Mn(OH)2)=1 .9 x 10"3 A. 9.86 B. 7.61 C. Not enough information need concentration of Mn(OH)2. D. 13.32 ' E. 4.44 3. The molar solubility of Bil; in 0.067M K1 is: Ksp(BiI3)=8.0><10‘19 A. 6.7><10'2 M B. 2.7x10‘-'5M C. 5.4><10'2° M -D. 1.2X10"7M E. 3.1><10'7 M _ 4. Lanthanum iodate La(103)3 has Ksp=6.2X10“2. When the following solutibns are mixed, which will NOT cause precipitation of La(103)3? 100. mL of 0.125 M LaCN03)3 with 100. mL of 0.050 M NaIO, 50. mL of 0.125 M La(NO,)3 with 50. mL of 0.050 M NaIO, 10. mL of 0.0050 M LaCNO3)3 with 10. mL of 0.0050 M NaIO; 50. mL of 0.00050 M La(NO3)3 with 50. mL of 0.0050 M NaIO, All will cause precipitation of La(IO3)3. WPCF’?’ A solution is 0.050 M in each of the cations Ag+ and Mg”. Solid NaZCO3 is added to the solution to precipitate the ions as carbonates and to separate Ag" from Mg”. What 0 concentration of CO;2 should be maintained to precipitate as much of the Ag+ as possible without precipitating the Mg”? (K..(Mgc0.>=1x10-5; K..(Ag2c03>=8.1><10"2) A. 3X10'9M B. 1X10'3M C. 2X10’4M D. 3X10'3M E. l><lO"°M Which of the following reagents can be used to distinguish between ng” and Hg”? (HINT: Use solubility rules) A. Addition of HZS/in 0.3 M HCl B. Addition of (NH4)2CO3/in NH3/NH4C1 C. Addition of HCl D. Addition of HZS/in NH3/NH4C1 E. Addition of HNO3 A solution is originally 4.2><10‘s M in each of the metal ions Co”, Fe” and Ag*. Solid NaZS is added such that the 8'2 concentration becomes 1.4><10"9M. Which of the metal ions will precipitate as the metal sulfide? Ksp(CoS)=4.0>< 10-21 sz(FeS)=6.0><10"8 Ksp(AgZS)=6X 104° A. Ag+ B. Co” and Fe*2 C. Co”2 and Ag+ D. Fe” E. Co”, Fe” and Ag” In the metal complex salt K4[Ru(CN)4(SCN)2], the oxidation state (charge) on the ruthenium is while the coordination number is . A. -4; ten B. +4; six C. .t +2; six D. +3; four E. None of the above are correct. 10. '11. 12. 13. mcowa For the metal complex ion given in question #8, what type(s) of isomerism is(are) possible? linkage and ionization ionization and geometric geometric linkage and geometric linkage Optical isomers (enantiomers) are possible for which of the following metal complex ions? A. fac-[Pt(NH3);rBr3]+ B. mer-[Pt(NH3)3Br3]* C. [Pt(NH3)sBr]+3 D. cis-[Pt(en)2BrCl]+2 E. trans-[Pt(en)2BrCl]+2 Use crystal field theory to decide which of the complexes below will have five unpaired electrons. A. [Fe(CN)6]‘3 B. [Fe16]‘3 C. [Mn(H20)5]+2 D. [CoF.3]‘4 E. Both B and C. The metal complex [Ni(NH3)2Br2] is diamagnetic while the metal complex [Til-“J3 is paramagnetic with one unpaired electron. Valence bond theory predicts that the Ni will use hybrid orbitals during bonding while the Ti will use hybrid orbitals. Sps; Spsdz sp; d2er3 dspz; sp’d2 dspz; dzsp3 dzsp3; sp3 mpow> An octahedral “d6” metal complex with weak field ligands will have unpaired electrons while an octahedral “d7” metal complex with strong field ligands will have unpaired electrons. A. . four; one B. zero; three C. six; seven D. zero; one B. four; three 14. 15. 16. 17.‘ In an octahedral complex the metal greater extent than the other d orbitals because orbital(s) is(are) raised in energy to a dxy, (1x2 and dyz; the negatively charged ligands point in between the lobes. d,a_y2 and dzz; the negatively charged ligands point directly at their lobes. dzz; it has a different shape and energy than the rest. . d,(2_y2 and dzz; they are filled with electrons while the other d-orbitals are empty. None of the above are true. All of the metal d-orbitals have the same energy. mpow> An aqueous solution of an ionic compound was colored. Which of the following salts could NOT be the ionic compound? (HINT: Consider the electronic configuration of the metal cation.) A; Mchosh B. Zn(ClO4)2 C. ScCl3 D. Cr(CzH302)2 E. Answers A, B, and C. Cadium cations Cd+2 form a soluble metal-complex ion [Cd(NH3)4]“2 upon the addition of ammonia. The molar solubility of CdS in 2.0 M NH3 is: Ksp(CdS)=3 .6>< 10‘”; K,{Cd(NH3)4]+2=4.OX 10° A. 6.0><10"5 M B. 0.50 M C. 2.5><10'12 M D. 1.4X10'2° M E. 4.8><10'll M Chromium (III) cations are amphoteric but do not form ammonia complexes. Which of the following statements is TRUE? Solid Cr(OH)3 will dissolve in an excess of ammonia. ' Solid Cr(OH)3 will not dissolve in an excess of sodium hydroxide. Cr(OH)3 will not dissolve in acidic solutions (pH<4). Solid Cr(OI-I)3 will not form on addition of a limited amount of ammonia to Cr"3(aq). Solid Cr(OH)3 will dissolve in an excess of sodium hydroxide. WPOP’? 18. 19. 20. The equilibrium concentration of Ag+ is 3.3><10'8 M in a 0.15 M solution of the metal . complex [Ag(CN)2]'. The numerical value of K for [Ag(CN)2]f is: A. 2.7><10l7 B. l.0><1021 C. 4.2><10l9 D. 3.0X10'9 E. 1.4X10” Which of the following statements pertaining to spontaneity is TRUE? A. All endothermic reactions are spontaneous. B A decrease in entropy on going from reactants to products favors a spontaneous . reaction. C All exothermic reactions are spontaneous. D. A reaction spontaneously moves toward equilibrium. E All reactions accompanied by an increase in entropy are spontaneous. Which of the following processes is accompanied by a decrease in entropy? CuCl(s) -' Cu*(aq) + Cl'(aq) 2 H3PO4(5) "’ P205(5) + 3 H20(g) 4 Fe(s) + 3 02(g) -* 2 Fe203(s) 3 5(5) + 2 1120(8) —’ 2 H23(g) + 302(g) Both A and, C. mpowa ...
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16-exam4 - CHEMISTRY 16 EXAM IV Dr M Richards-Babb(Version...

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