For the following complex ions indicate the charge on the metal by fdh56iuoui

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									Chemistry 106, Chapter 15 Exercises
1. For the following coordination compounds give the formula and charge for the counter ion and the
   complex ion.
   a. [Pd(NH3)3Cl]NO3 b. [Co(NH3)5Cl]CO3 c. Ca[Ni(CN)4] d. Na2[CdCl4]

2. For the following complex ions indicate the charge on the metal ion, ligand formula and charge,
   coordination number, and predicted geometry.
   a. [Ag(NH3)2]+1                      e. [Cr(OH)6]3-                        i. [Zn(C2O4)2]2-
   b. [NiCl4]2-                         f. [Fe(CN)6]3-                        j. [Zn(en)(C2O4)]
                 2+
   c. [Zn(NH3)4]                        g. [Co(en)2(SCN)Cl]+
   d. [Al(H2O)6]3+                      h. [Ni(H2O)2Cl2(OH)2]2-

3. What is the formula of the sodium salt of the ion below? The magnesium salt?
   [Ni(H2O)2Cl2(OH2]2-

4. What is the formula of the sulfide salt of the ion below? The fluoride salt?
   [Co(en)2(SCN)Cl]+

5. Give the formula and charge of each of the following complexes:
   a. Cr3+, two oxalate (C2O4)2- ions, two H2O molecules
   b. Cr3+, five NH3 molecules, one SO42- ion
   c. Cr3+, one ethylenediamine molecule, two ammonia molecules, two I- ions
   d. Pt2+, two ammonia molecules, one oxalate ion
   e. Pt2+, two NH3 molecules, one thiocyante ion (SCN-), one Br- ion
   f. Pt2+, one ethylenediamine molecule, two NO3- ions

6. Predict the formula of the complex formed by
   a. Zn2+ with C2O42-               d. Ag+ with H2O                        g. Fe3+ with C2O42-
   b. Ag+ with CN-                   e. Pd2+ with Br-
        2+         -
   c. Cd with CN                     f. Pt2+ with H2O

7. Give the electronic configuration for the following ions and indicate the number of unpaired electrons
   in each.
   a. V2+    b. Zn2+    c. Cu+    d. Mn4+     e. Ti3+ f. Cr3+     g. Ru4+

8. Identify the Lewis acid and the Lewis base in each of the following reactions.
   a. B(OH)3 + H2O → B(OH)4- + H+
   b. Ag+ + 2NH3 → Ag(NH3)2+
   c. BF3 + F- → BF4-
   d. 6H2O + Fe3+ → Fe(H2O)63+
   e. CN- + H2O → HCN + OH-
   f. HgI2 + 2I- → HgI42-
Answers to Complex Ion Exercises

1. a. NO3-, [Pd(NH3)3Cl]+    b. CO32-, [Co(NH3)5Cl]2+      c. Ca2+, [Ni(CN)4]2-    d. Na+, [CdCl4]2-

2. a. Ag1+, NH3, 2, linear                                   g. Co3+, H2NCH2CH2NH2, SCN1-, Cl-, 6
   b. Ni2+, Cl-, 4, tetrahedral or square planar                 octahedral
   c. Zn2+, NH3, 4, tetrahedral or square planar             h. Ni2+, H2O, Cl1-, OH1-, 6, octahedral
   d. Al3+, H2O, 6, octahedral                               i. Zn2+, (C2O4)2]2-, 4, tetrahedral or square
   e. Cr3+, OH-, 6, octahedral                                   planar
   f. Fe3+, CN-, 6, octahedral                               j. Zn2+, H2NCH2CH2NH2, C2O42-, 4,
                                                                 tetrahedral or square planar

3. Na2[Ni(H2O)2Cl2(OH2]
   Mg[Ni(H2O)2Cl2(OH2]

4. [Co(en)2(SCN)Cl]2S
   [Co(en)2(SCN)Cl]F

5. a. [Cr(C2O4)2(H2O)2]1-                                    d. [Pt(NH3)2(ox)]
   b. [Cr(NH3)5(SO4)]1+                                      e. [Pt(NH3)2(SCN)Br]
   c. [Cr(en)(NH3)2I2]1+                                     f. [Pt(en)(NO3)2]

6. a. [Zn(C2O4)2]2-                                          e. [PdBr4]2-
   b. [Ag(CN)2]1-                                            f. [Pt(H2O)4]2+
   c. [Cd(CN)4]2-                                            g. [Fe(C2O4)3]3-
   d. [Ag(H2O)2]1+

7. a. V2+      1s22s22p63s23p64s03d3
   b. Zn2+     1s22s22p63s23p64s03d10
   c. Cu+      1s22s22p63s23p64s03d10
   d. Mn4+     1s22s22p63s23p64s03d3
   e. Ti3+     1s22s22p63s23p64s03d1
   f. Cr3+     1s22s22p63s23p64s03d3
   g. Ru4+     1s22s22p63s23p64s23d104p65s04d4

8. For the following, the Lewis acid is in italics. The other reactant is the Lewis base.
   a. B(OH)3 + H2O → B(OH)4- + H+
   b. Ag+ + 2NH3 → Ag(NH3)2+
   c. BF3 + F- → BF4-
   d. 6H2O + Fe3+ → Fe(H2O)63+
   e. CN- + H2O → HCN + OH-
   f. HgI2 + 2I- → HgI42-

								
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