Mg + Au+ -> Mg2+ + Au
what is the oxidation and reduction half reactions
Mg ==> Mg^2+ + 2e
Au^+ + e ==> Au
Do you know which is oxidation and which reduction?
Dr Bob 222 please stop
To determine the oxidation and reduction half-reactions, we need to identify the species being oxidized and reduced.
In this equation:
Mg + Au+ -> Mg2+ + Au
The magnesium (Mg) is being oxidized since it loses electrons and its oxidation state increases from 0 to +2.
The gold ion (Au+) is being reduced since it gains electrons, and its oxidation state decreases from +1 to 0.
Therefore, the oxidation half-reaction is:
Mg -> Mg2+ + 2e−
And the reduction half-reaction is:
Au+ + e− -> Au
In summarizing, the oxidation half-reaction is Mg -> Mg2+ + 2e−, and the reduction half-reaction is Au+ + e− -> Au.
To determine the oxidation and reduction half-reactions in the given chemical equation:
Mg + Au+ -> Mg2+ + Au
1. Identify the changes in oxidation states for each element in the equation.
- In this equation, Mg undergoes oxidation, as its oxidation state increases from 0 to +2.
- Au undergoes reduction, as its oxidation state decreases from +1 to 0.
2. Write the half-reactions for oxidation and reduction separately:
Oxidation Half-Reaction:
Mg -> Mg2+ + 2e-
In this reaction, Mg loses two electrons to form Mg2+.
Reduction Half-Reaction:
Au+ + e- -> Au
In this reaction, Au+ gains one electron to form Au.
Note: The coefficients in the balanced equation are not included in the half-reactions as they cancel out when balancing the overall equation.
Therefore, the oxidation half-reaction is Mg -> Mg2+ + 2e- and the reduction half-reaction is Au+ + e- -> Au.