Respuesta :

ali015
Your compound is [tex]K_{2}PtCl_{6}[/tex].

Remember that the oxidation numbers in a neutral compound must add up to zero. Cl has an oxidation number of -1 because it is a halogen K has an oxidation number of +1 because it is an alkali metal, which exhibits an oxidation state of +1 in compounds.

Since you have 6 atoms of Cl, you have -1(6) = -6 for the Cl. Since you 2 atoms of K, you have +1(2) = +2 for the K. The oxidation number of Pt must make all the oxidation numbers add up to zero:
+2 + (-6) + oxidation number of Pt = 0
-4 + oxidation number of Pt = 0
Oxidation number of Pt = 4

The oxidation number of platinum is +4 in [tex]K_2PtCl_6[/tex].

Given:

The coordination compound [tex]K_2PtCl_6[/tex]

To find :

The oxidation number of platinum in the given compound.

Solution

  • Number of potassium atoms = 2
  • Number of platinum atoms = 1
  • Number of chlorine atoms = 6

Let the oxidation number of platinum be x.

  • The oxidation number of potassium is = +1
  • The oxidation number of chlorine = -1

The overall charge on the compound's molecule = 0

[tex]2\times (+1)+x+6\times(-1)=0\\+2+x-6=0\\x=+6-2=+4[/tex]

The oxidation number of platinum is +4.

Learn more about an oxidation number here:

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