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What is the oxidation state of an individual sulfur atom in SO42−?
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+ Inorganic chemistry
+ Oxidation
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Malcolm Campbell
What is the oxidation state of an individual sulfur atom in SO42−?
Sulfur is fully oxidized in sulfate ion, [math](O=)_{2}S(-O^{-})_{2}[/math], and assumes the Group oxidation number, i.e. [math]S(VI+)[/math]. As usual oxygen is the [math]O(-II)[/math] state. And so [math]+VI+4×(-II)=-2[/math]. As always, the weighted sum of the oxidation gives the charge of the ion. What are the oxidation numbers of the heteroatom in [math]PO_{4}^{3-}[/math], and [math]NO_{3}^{-}[/math]? What about in thiosulfate, [math]S_{2}O_{3}^{2-}[/math]?
Sulfur is fully oxidized in sulfate ion, [math](O=)_{2}S(-O^{-})_{2}[/math], and assumes the Group oxidation number, i.e. [math]S(VI+)[/math]. As usual oxygen is the [math]O(-II)[/math] state. And so [math]+VI+4×(-II)=-2[/math]. As always, the weighted sum of the oxidation gives the charge of the ion. What are the oxidation numbers of the heteroatom in [math]PO_{4}^{3-}[/math], and [math]NO_{3}^{-}[/math]? What about in thiosulfate, [math]S_{2}O_{3}^{2-}[/math]?
The oxidation states of the atoms in a molecule or ion must add up to the overall charge on the molecule or ion. So, in a neutral molecule the oxidation states of all the atoms will add to zero. In (SO4)2- then, the oxidation states of all atoms must add give -2.
The oxidation state of oxygen is almost always -2. So if we assign each oxygen atom in the sulfate ion a -2 charge, the total negative charge will add to 4(-2) = -8.
This means that the oxidation state of the sulfur atom must be a value that will reduce the -8 charge to -2.
The oxidation states of the atoms in a molecule or ion must add up to the overall charge on the molecule or ion. So, in a neutral molecule the oxidation states of all the atoms will add to zero. In (SO4)2- then, the oxidation states of all atoms must add give -2.
The oxidation state of oxygen is almost always -2. So if we assign each oxygen atom in the sulfate ion a -2 charge, the total negative charge will add to 4(-2) = -8.
This means that the oxidation state of the sulfur atom must be a value that will reduce the -8 charge to -2.
Sulfur is fully oxidized in sulfate ion, [math](O=)_{2}S(-O^{-})_{2}[/math], and assumes the Group oxidation number, i.e. [math]S(VI+)[/math]. As usual oxygen is the [math]O(-II)[/math] state. And so [math]+VI+4×(-II)=-2[/math]. As always, the weighted sum of the oxidation gives the charge of the ion. What are the oxidation numbers of the heteroatom in [math]PO_{4}^{3-}[/math], and [math]NO_{3}^{-}[/math]? What about in thiosulfate, [math]S_{2}O_{3}^{2-}[/math]?
Sulfur is fully oxidized in sulfate ion, [math](O=)_{2}S(-O^{-})_{2}[/math], and assumes the Group oxidation number, i.e. [math]S(VI+)[/math]. As usual oxygen is the [math]O(-II)[/math] state. And so [math]+VI+4×(-II)=-2[/math]. As always, the weighted sum of the oxidation gives the charge of the ion. What are the oxidation numbers of the heteroatom in [math]PO_{4}^{3-}[/math], and [math]NO_{3}^{-}[/math]? What about in thiosulfate, [math]S_{2}O_{3}^{2-}[/math]?
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The oxidation states of the atoms in a molecule or ion must add up to the overall charge on the molecule or ion. So, in a neutral molecule the oxidation states of all the atoms will add to zero. In (SO4)2- then, the oxidation states of all atoms must add give -2.
The oxidation state of oxygen is almost always -2. So if we assign each oxygen atom in the sulfate ion a -2 charge, the total negative charge will add to 4(-2) = -8.
This means that the oxidation state of the sulfur atom must be a value that will reduce the -8 charge to -2.
-8 + X = -2
X = -2 + 8 = +6
So, the oxidation state of sulfur is +6
The oxidation states of the atoms in a molecule or ion must add up to the overall charge on the molecule or ion. So, in a neutral molecule the oxidation states of all the atoms will add to zero. In (SO4)2- then, the oxidation states of all atoms must add give -2.
The oxidation state of oxygen is almost always -2. So if we assign each oxygen atom in the sulfate ion a -2 charge, the total negative charge will add to 4(-2) = -8.
This means that the oxidation state of the sulfur atom must be a value that will reduce the -8 charge to -2.
-8 + X = -2
X = -2 + 8 = +6
So, the oxidation state of sulfur is +6
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