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Solutions

Exercise 1: Determine the oxidation number for each of the transition metal atoms or ions

7.

[V(OH2)6](NO3)3

x + 6(0) + 3(-1) = 0      x = +3

8.

(NH4)2[CoCl4]

2(+1) + x + 4(-1) = 0   x = +2

9.

[Co(py)4]Br2

x + 4(0) + 2(-1) = 0   x = +2

10.

K4[Mn(CN)6]

4(+1) + x + 6(-1) = 0x = +2

11.

[Co(P(CH3)3)4]2(SO4)3

2(x + 4(0)) +3(-2) = 0x = +3

12.

Ni(NH3)4Cl2

x + 4(0) + 2(-1) = 0x = +2

Exercise 2: Put the following compounds together to give the formula of the compound.

Remember to use [ ] to identify the complex ion in ionic complexes.

Where you need a counterion to produce a neutral compound, use either K+ or SO4-2.

Remember to list the cation first, followed by anion for ionic compounds.

Metal/charge Ligands Formula

2.

Co+2 Four Br

determine if complex is anionic or cationic

1(Co+2) + 4(Br-) = 1(+2) + 4(-1) = -2    complex is anionic

determine necessary counter ion for neutral compound must be positive so select potassium (K+)

formula is  Kx[Co(Br)4]

solve for number of potassium needed          x(K+)+1(Co+2)+4(Br-)=x(+1)+1(+2)+4(-1)=0 x=2

substitute for x                                    K2[Co(Br)4]

3.

Ru+3 Three oxalates

1(Ru+3) + 3(ox-2) = 1(+3) + 3(-2) = -3complex is anionic choose K+

Kx[Ru(ox)3]

x(K+) + 1(Ru+3) + 3(ox-2) = x(+1) + 1(+3) + 3(-2) = 0 x=3

K3[Ru(ox)3]

4.

Os+3 Three dppe

1(Os+3) + 3(dppe) = 1(+3) + 3(0) = +3complex is cationic choose SO4-2

[Os(dppe)3](SO4)x

1(Os+3) + 3(dppe) + x(SO4-2) = 1(+3) + 3(0) + x(-2) = 0 x=3/2  

[Os(dppe)3](SO4)3/2 * 2 = [Os(dppe)3]2(SO4)3

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