assigning oxidation numbers for ionic compounds, oxidation numbers can be assigned using the...
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![Page 1: Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table](https://reader034.vdocuments.mx/reader034/viewer/2022051401/56649e665503460f94b61e4b/html5/thumbnails/1.jpg)
Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
![Page 2: Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table](https://reader034.vdocuments.mx/reader034/viewer/2022051401/56649e665503460f94b61e4b/html5/thumbnails/2.jpg)
Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
Alkali Metals = +1
![Page 3: Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table](https://reader034.vdocuments.mx/reader034/viewer/2022051401/56649e665503460f94b61e4b/html5/thumbnails/3.jpg)
Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
Alkaline Earth Metals = +2
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Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
Group 13 Boron Group = +3
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Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
Group 15 Nonmetals = -3
![Page 6: Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table](https://reader034.vdocuments.mx/reader034/viewer/2022051401/56649e665503460f94b61e4b/html5/thumbnails/6.jpg)
Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
Group 16 Nonmetals = -2
![Page 7: Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table](https://reader034.vdocuments.mx/reader034/viewer/2022051401/56649e665503460f94b61e4b/html5/thumbnails/7.jpg)
Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
Halogens = -1
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Assigning Oxidation NumbersAssigning Oxidation Numbers
For ionic compounds, oxidation numbers can be assignedusing the expected charges from the periodic table.
Transition Metals depend on anion
![Page 9: Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table](https://reader034.vdocuments.mx/reader034/viewer/2022051401/56649e665503460f94b61e4b/html5/thumbnails/9.jpg)
Ionic CompoundsIonic CompoundsExample:
MgCl2+2 -1
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Ionic CompoundsIonic CompoundsExample:
Na2O+1 -2
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Ionic CompoundsIonic CompoundsExample:
Fe2O3
?? -2
We don’t know iron’s oxidation number from the periodic table since it is a transition metal.
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Ionic CompoundsIonic CompoundsExample:
Fe2O3
+3 -2
But since we know the compound is neutral, the oxidation numbers must add up to zero. Therefore, Fe has a +3 oxidation number in this compound.
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Ionic CompoundsIonic CompoundsExample:
Cr2O72-?? -2
We don’t know chromium’s oxidation number from the periodic table since it is a transition metal.
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Ionic CompoundsIonic CompoundsExample:
+6 -2
But since this ion has a charge of -2, the oxidation numbers must add up to negative two. Therefore the oxidation number of Cr is +6Cr2O72-
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Covalent CompoundsCovalent Compounds
Covalent compounds are made of two nonmetals, which from the periodic table are
always expected to be negative
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Covalent CompoundsCovalent Compounds
But since covalent compounds are neutral species, it is not possible for every element to
retain its negative oxidation number
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Covalent CompoundsCovalent Compounds
ONLY THE MORE ELECTRONEGATIVE ELEMENT keeps its negative oxidation number.
Other nonmetals must adapt to keep the compound neutral
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Electronegativity TrendElectronegativity Trend
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Covalent CompoundsCovalent CompoundsExample:
SO2
Since oxygen is the more electronegative element, it will
have its normal oxidation number.
-2
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Covalent CompoundsCovalent CompoundsExample:
SO2
The compound is neutral, so the oxidation number of sulfur will be sufficient to balance out the two
oxygen atoms.
-2+4
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Covalent CompoundsCovalent CompoundsExample:
OF2
Since fluorine is the more electronegative element, it will
have its normal oxidation number.
-1
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Covalent CompoundsCovalent CompoundsExample:
OF2
The compound is neutral, so the oxidation number of oxygen will be sufficient to balance out the
two fluorine atoms.
+2 -1
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Covalent CompoundsCovalent CompoundsExample:
PO43-
Since oxygen is the more electronegative element, it will
have its normal oxidation number.
-2
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Covalent CompoundsCovalent CompoundsExample:
PO43-
-2
The ion has a charge of negative three, so the oxidation numbers must add up to the total charge
of the ion.
+5
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
CaSO4
This is an ionic compound, so the charge of the metal cation is its
oxidation number
+2
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
CaSO4
The anion is a polyatomic ion, sulfate, and the charge of sulfate is negative two. So the oxidation
numbers of sulfur and oxygen must add to -2
+2
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
CaSO4
Oxygen is the more electronegative of the two, so it
keeps its normal oxidation number.
+2 -2
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
CaSO4
Sulfur and the four oxygen atoms must add to negative two (the charge of the sulfate anion).
+2 -2+6
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
Pb(OH)4This is an ionic compound, so the charge of the metal cation is its oxidation number. But this is a transition metal, so we cannot know it from its position on the
periodic table.
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
Pb(OH)4But the anion, the hydroxide ion, carries a charge of negative one. All four hydroxides are negative one, but since the compound is neutral, the oxidation number of
lead must balance it out.
+4
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
Pb(OH)4Within the anion, oxygen is the more electronegative of the two elements, and keeps its normal
oxidation number.
+4 -2
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Ionic Compounds with PolyatomicsIonic Compounds with PolyatomicsExample:
Pb(OH)4Within the hydroxide ion, the
oxygen and hydrogen must add to the charge of the ion, -1
+4 -2 +1