3. Determine the oxidation state of the metal in each of the following a. Al2(SO4)3.18H2O b.(Al(H2°)6)3+ c.(Ag(NH3)2)+

Question

3. Determine the oxidation state of the metal in each of the following
a. Al_²(SO₄)₃.18H₂O
b.(Al(H2°)₆)³⁺
c.(Ag(NH₃)₂)⁺

 

Answer 1

A) Al₂(SO₄)₃ x 18H₂O

 

To determine this, you only need to pay attention to the charge of the common ion (SO₄).

 

Since SO₄ is typically -2, we can assume that there are six negative charges in this complex. Since there are two Al atoms, each has an oxidation state of +3.

 

In this particular complex, we can ignore the water molecules since they are not included in brackets, thus not coordinated to the metal atom.

 

B) (Al(H₂O)₆)³⁺)

 

In this complex, the six water molecules represent 3 negative charges (half the number of water molecules). So, if the overall complex is +3 (indicated by the superscript after the complex), then the Al atom must be in the +6 oxidation state.

 

C) (Ag(NH₃)₂)⁺

 

For this complex, we treat ammine (NH₃) ligands as neutral ligands. So, if the overall charge of the complex is +1, then the Ag atom must be in the +1 oxidation state.

 

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