0 in the elemental form
+2 in its compounds
The oxidation number for Mg, or Magnesium is Mg+2. Magnesium is in the second family, which means is it will lose 2 electrons to be stable. Losing those two electrons will make it positive.
The magnesium is in the 2+ oxidation state and the oxygen is in the 2- oxidation state.
Oxidation number of O is -2. Oxidation number of Mg is +2.
Always -2 for oxides
2 apex
For Mg the oxidation no is +2 while it is -2 for oxygen.
Magnesium(II) so +2
+2 for Mg and -2 for O
This is an oxidation reaction; magnesium burn in oxygen.
+2
2 apex
For Mg the oxidation no is +2 while it is -2 for oxygen.
The O in oxides always has oxidation number -2 (except for in peroxides where it is -1). Since the overall species has oxidation number 0, Mg must also have oxidation number +2.
Magnesium(II) so +2
+2 for Mg -2 for O
Because in MgO magnesium is already in its highest oxidation state and cannot be oxidized further.
+2 for Mg and -2 for O
This is an oxidation reaction; magnesium burn in oxygen.
Oxidation state: +2
You cannot 'burn' MgO, it is refactory. I take it you mean burning Magnesium metal in oxygen - if so the answer is that the magnesium is oxidised to MgO and the oxygen is reduced - all reduction/oxidation ('redox') reactions are coupled - if something is oxidised the other is reduced.
oxidation number of I is -1. oxidation number of F is +1.