Question

NI2O3 using rules to find oxidation numbers of atoms​

Answer 1

Answer:

Oxidation number is -1: balanced equation by entering the number of -2 2 + 2 OH- Ni2O3!

Explanation

Rules for Assigning Oxidation Numbers.

1. The convention is that the cation is written first in a formula, followed by the anion. For example, in NaH, the H is H-; in HCl, the H is H+.
2. The oxidation number of a free element is always 0. The atoms in He and N2, for example, have oxidation numbers of 0.
3. The oxidation number of a monatomic ion equals the charge of the ion. For example, the oxidation number of Na+ is +1; the oxidation number of N3- is -3.
4. The usual oxidation number of hydrogen is +1. The oxidation number of hydrogen is -1 in compounds containing elements that are less electronegative than hydrogen, as in CaH2.
5. The oxidation number of oxygen in compounds is usually -2. Exceptions include OF2 because F is more electronegative than O, and BaO2, due to the structure of the peroxide ion, which is [O-O]2-.
6. The oxidation number of a Group IA element in a compound is +1.
7. The oxidation number of a Group IIA element in a compound is +2.
8. The oxidation number of a Group VIIA element in a compound is -1, except when that element is combined with one having a higher electronegativity. The oxidation number of Cl is -1 in HCl, but the oxidation number of Cl is +1 in HOCl
9. The sum of the oxidation numbers of all of the atoms in a neutral compound is 0.
10. The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion. For example, the sum of the oxidation numbers for SO42- is -2.

Answer 2

Answer:

NI will lose electron but O will gain electron

hope it is clear

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