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Redox
- Ion Formation
- Metals: Are oxidised
and form positive ions.
- Non-Metals: Are reduced
and form negative ions.
- Metals: Are oxidised
and form positive ions.
- Oxidation Number Rules
- Ion: Charge on ion
- Uncombined Element: 0
- Combined Oxygen: -2
- Combined Hydrogen: +1
- Combined Fluorine: -1
- If there is a roman numeral after an element name,
that element has that oxidation number (e.g. In
Iron(II) Chloride, Iron has an oxidation number of 2+).
- Ion: Charge on ion
- Reactions
- Metals+Acids
- Metal is oxidised to form positive ion
- Hydrogen in acid reduced to form hydrogen gas
- Acid+Metal==Salt+H2
- Metal is oxidised to form positive ion
- Half Equations
- Show the oxidation or reduction of
certain elements during a reaction.
- e.g.
Mg+Cl2==MgCl2
- Mg==Mg(2+)+2[e(-)]
- Cl2+2[e(-)]==2[CL(-)]
- Mg==Mg(2+)+2[e(-)]
- Show the oxidation or reduction of
certain elements during a reaction.
- Metals+Acids
- Definitions
- Reduction
- Gain of electrons
- Decrease in oxidation number.
- Gain of electrons
- Oxidation
- Loss of electrons
- Increase in oxidation number.
- Loss of electrons
- Reduction
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