Oxidation unit test Please help ASAP!!!

Which statement correctly describes the oxidation number of the manganese atom (Mn) in Mnl2 and MnO2?

O Manganese has an oxidation number of +4 in Mnl2 and +2 in MnO2.
o Manganese has an oxidation number of +2 in Mnl2 and +4 in MnO2.
o Manganese has an oxidation number of +4 in both Mnl2 and MnO2.
Manganese has an oxidation number of +2 in both Mnl2 and MnO2.

Manganese has an oxidation number of +2 in Mnl2 and +4 in MnO2.

Explanation:

Hey there!

In this case, according to the given information about the oxidation numbers, it turns out possible to figure out the oxidation number of manganese in both MnI2 and MnO2 by using the concept of charge balance, whereby we can define the oxidation state of iodine and oxygen as -1 and -2, respectively, since the former needs one electron to complete the octet and the latter, two of them.

Next, we can write the following x, since manganese has five oxidation states, and it is necessary to calculate the appropriate one:

Next, we multiply each anion's oxidation number by the subscript, to obtain the following:

Thus, the correct choice is Manganese has an oxidation number of +2 in Mnl2 and +4 in MnO2.

Regards!

it is stable as it is in group 0 which have full outer shells of electrons