Download 163 ch23 Transition elements

Chem 163 Ready for class? Transition elements
1. The most abundant element in the earth’s atmosphere is ______________ and The most abundant
metal ion in seawater is _________.
2. What is the number of unpaired electrons in an octahedral, high-spin Mn(II) complex?
3. O3 and O2 are different form of oxygen. They are called __________________________.
4. In the diamond structure, the hybrid orbital set used by the carbon atoms to form σ-bonds is
________ and In the graphite structure, the hybrid orbital set used by the carbon atoms to form σbonds is ___________.
5. Determine the number of unpaired electrons in an octahedral, low-spin Cr(II) complex.
6. The ground state electron configuration of Zn2+ is ___________________________
7. List the following in order of decreasing stability.
8.
9.
O, O3, O2 . _____________________
The charge on the metal ion in the coordination complex ion, [Co(CO3)3]3-, is __________.
The oxidation numbers of cobalt in the compound [Co(NH3)5Cl]Cl2 is ______ and the coordination
number is _________.
10. The coordination number of platinum in the complex ion, [Pt(C2O4)2]2-, is _____.
11. Chelating ligands are __________________________________________ (definition) and the
example of a chelating legand is ____________.
12. The name for the transition metal complex [Fe(CN)6]3a. hexacyano ferrate(III)
b. hexacyanoiron(II)
c. iron(III) hexacyanide
d. ferrous cyanide
e. ferric cyanide
13. A coordination compound formed from cobalt(III) sulfate and ammonia contains six ammonia molecules as ligands. The formula of the compound is
a.
Co2(SO4)3∙6NH3
b.
[Co(NH3)6]2(SO4)3
c.
Co3SO4(NH3)6
d.
Co2(SO4)3(NH4)6
e.
Co2[(NH3)6](SO4)3
14. Consider the following data, taken at 25°C
Au2O3(s)
Au(s)
O2(g)
H of
-144.8 kJ mol-1
0.00 kJ mol-1
0.00 kJ mol-1
So
+0.1255 kJ mol-1K-
0.04741 kJ mol-1K-1 0.205 kJ mol-1K-
The decomposition reaction for Au2O3(s) is: 2 Au2O3(s) → 4 Au(s) + 3 O2(g). Using the data given
here, what is the equilibrium temperature for the reaction?
15. (a) Sketch the 5 d orbitals, and label them.
(b) Explain why d orbitals split (no longer all degenerate) in complex ions.
16.
(a) Is [Fe(H2O)6]+2 paramagnetic or diamagnetic?
(b) Is [Fe(CN)6]-4 paramagnetic or diamagnetic?
(c) List at least two things that are common in both of theses diagrams.
(d) One thing that is different is how 6 electrons fill the orbitals in different order. Give two reasons
why.