Final answer:
The charge of manganese in Mn(NO₃)₂ is +2, as it must balance the charge from two nitrate ions, each with a -1 charge to make the overall compound neutral.
Step-by-step explanation:
The charge of manganese in Mn(NO₃)₂ is +2.
Mn(NO₃)₂ is a compound called manganese(II) nitrate. In this compound, the oxidation number of each nitrate ion (NO₃-) is -1. Since there are two nitrate ions, the total oxidation number contributed by the nitrate ions is -2. The overall charge of the compound is zero, meaning the sum of the oxidation numbers of all the elements must be zero. Therefore, the oxidation number of manganese (Mn) must be +2 to balance out the -2 from the nitrate ion's oxidation numbers.
To explain the charge of manganese in Mn(NO₃)₂, it's crucial to analyze the oxidation numbers of the components within the compound. The nitrate ion NO₃⁻ has an oxidation number of -1, and considering that there are two nitrate ions, we get a total of -2 for the charge contribution from the nitrate ions. Hence, to have a neutral compound, the charge of manganese must be +2 to counterbalance the overall negative charge from the nitrate ions.
This concept is seen in different compounds such as KMnO₄, where the manganese has an oxidation number of +7, as in the reduction half-reaction where Mn undergoes reduction from +7 to +2. Therefore, it's evident from the content loaded reactions that the charge of manganese varies depending on the compound it is part of. So in Mn(NO₃)₂, the manganese ion has a charge of +2, denoted as Mn²⁺.