Redox reactions- reactions in which one or more electrons is transferred.
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Transcript of Redox reactions- reactions in which one or more electrons is transferred.
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Redox reactions- reactions in which one or more electrons is transferred
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Oxidation and Reduction When a metal undergoes corrosion it
loses electrons to form cations:Ca(s) +2H+(aq) Ca2+(aq) + H2(g) Oxidized: atom, molecule, or ion
becomes more positively charged. Oxidation is the loss of electrons.
Reduced: atom, molecule, or ion becomes less positively charged. Reduction is the gain of electrons.
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Vanadium compounds having different oxidation numbers or oxidation states
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How do maximum and minimum values of the oxidation number correlate with the position in the periodic table?
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The oxidation number of an atom in an element is 0.Ex: Na (s), O2 (g), Hg (l)
The oxidation state of a monatomic ion is the same as its chargeEx. Na + = +1 Cl - = -1
Fluorine has an oxidation number of -1 in its compounds
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Oxygen usually has an oxidation number of -2 in its compounds. There are some exceptions:a. Oxygen has an oxidation number of -1 in peroxides, which contain the O2
2- ion.b. Oxygen has an oxidation number of -1/2 in
superoxides, which contain the O2- ion.
Hydrogen has an oxidation number of +1 unless it is combined with metals, in which case it has an oxidation number of -1. The sum of the oxidation numbers of all atoms in a substance must equal the total charge on the species: 0 for molecules; the ionic charge for ions.
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The position of the element in the periodic table may be useful:a. Group IA (1) elements have oxidation numbers
of +1 in their compounds.b. Group IIA (2) elements have oxidation numbers
of +2 in their compounds.c. Group VIIA (17) elements have oxidation
numbers of -1 unless combined with oxygen or a halogen closer to the top of the group.
d. In binary compounds, Group VIA (16) elements have oxidation numbers of -2, unless combined with oxygen or halogens.
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General Summary
Element: 0Fluorine: -1Oxygen: -2Hydrogen: +1
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H2SO4 H is +1 S is -2 unless combined with oxygen or a
halogen, so leave this for last O is -2 Use summation rule for S:
2(+1) + 1(S) + 4(-2) = 0 S = 0 - 2 + 8 = +6
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 H2O2
NO3- MnO4
- CO2 NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O O(-2) H(+1) SO2 CCl4 H2O2
NO3- MnO4
- CO2 NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 Cl (-1) C (+4) H2O2
NO3- MnO4
- CO2 NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 H2O2
NO3- O(-2) N(+5) MnO4
- CO2 NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 H2O2
NO3- MnO4
- CO2 O(-2) C(+4) NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 H2O2
NO3- MnO4
- CO2 NaNO3 KClO4 O (-2) K (+1) Cl (+7)
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 O(-2) S(+4)CCl4 H2O2
NO3- MnO4
- CO2 NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 H2O2 H(+1) O(-1)NO3
- MnO4-
CO2 NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 H2O2
NO3- MnO4
- O(-2) Mn(+7) CO2 NaNO3 KClO4
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Determine values of the oxidation number of each element in these compounds or ions:
H2O SO2 CCl4 H2O2
NO3- MnO4
- CO2 NaNO3 O(-2) Na(+1) N(+5)KClO4
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Oxidation- increase in oxidation state Loss of electrons
Reduction- decrease in oxidation state Gain of electrons
LEO goes GER
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2Na(s) + Cl2(g) 2NaCl(s)
What substances are being oxidized and reduced?