Why #"Mg"^(2+) +2"e"^(-) -> "MgO"# ?
From a web-tutorial on reduction potentials :
Why should adding 2 electrons to #"Mg"^(2+)# result in #"MgO"# ?
AFAIK, in #"MgO"# magnesium's oxidation state is also #(+2)# .
From a web-tutorial on reduction potentials :
Why should adding 2 electrons to
AFAIK, in
1 Answer
That's just a typo.
Explanation:
You are right, adding two electrons to a magnesium cation,
You can oxidize magnesium metal to magnesium cations and reduce magnesium cations back to magnesium metal.
The correct reduction half-reaction would be
#"Mg"^(2+) + 2"e"^(-) -> "Mg"# #" "E^0 = -"2.38 V"#
So that is just a mistake they made when writing out the half-reaction.
For example, the synthesis of magnesium oxide,
#2"Mg"_text((s]) + "O"_text(2(g]) -> 2"MgO"_text((s])#
Here you have the oxidation half-reaction
#2"Mg" -> 2"Mg"^(2+) + 4"e"^(-)#
Each magnesium atom loses two electrons, so two magnesium atoms will lose a total of four electrons.
The reduction half-reaction is
#"O"_2 + 4"e"^(-) -> 2"O"^(2-)#
Each oxygen atom gains two electrons, so two oxygen atoms will gain a total of four electrons.