Respuesta :
Answer:
The difference between manganese (II) and manganese (IV) lies in the charge on the ion they form.
Explanation:
Manganese (II) refers to the +2 oxidation state of manganese, where the manganese atom loses two electrons to form a positively charged ion. This ion is represented as Mn2+. In this state, manganese has a charge of +2.
On the other hand, manganese (IV) refers to the +4 oxidation state of manganese, where the manganese atom loses four electrons to form a positively charged ion. This ion is represented as Mn4+. In this state, manganese has a charge of +4.
The difference between the two oxidation states is the number of electrons that manganese loses. Manganese (II) loses two electrons, while manganese (IV) loses four electrons. This difference in electron loss results in a difference in the charge on the ion formed.
The other options mentioned in the question are not correct:
A) The number of neutrons does not play a role in determining the oxidation state of an element. Neutrons are neutral particles found in the nucleus of an atom and do not affect the charge of an ion.
B) The location of manganese in a compound does not determine its oxidation state. The oxidation state is determined by the number of electrons gained or lost by the manganese atom.
C) The number of manganese nuclei does not determine the oxidation state. The oxidation state is solely based on the number of electrons gained or lost by the manganese atom.
Therefore, the correct answer is D) the charge on the ion it forms. The difference between manganese (II) and manganese (IV) is the charge on the ion they form, which is +2 and +4, respectively.
