Write the rules to assign oxidation number.
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Rules for Assigning Oxidation Numbers
Oxidation numbers are real or hypothetical charges on atoms, assigned by the following rules:
1. Atoms in elements are assigned 0.
2. All simple monatomic ions have oxidation numbers
equal to their charges. (e.g., all Group IA ions are +1;
all group IIA ions are +2; all the following ions have
oxidation numbers given by their charges - Fe2+, Al3+,s2-, N3-)
3. Fluorine is always -1 in its compounds.
4. Halogens are usually -1, except when a central atom or
when combined with a more electronegative element
(e.g., assign I as -1 in NI3, but +3 in ICl3).
5. Oxygen is -2 in most of its compounds, except in cases
like peroxides (H2O2, Na2O2) where it is -1.
6. Hydrogen is usually +1, except in hydrides with
electropositive elements, particularly with metal
cations, where it is -1 (e.g., NaH,CaH2,BH4).
7. The sum of all oxidation numbers for a neutral
compound is zero; the sum is the charge on the species
for a complex ion.
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Answer:
The convention is that the cation is written first in a formula, followed by the anion. ...
The oxidation number of a free element is always 0. ...
The oxidation number of a monatomic ion equals the charge of the ion. ...
The usual oxidation number of hydrogen is +1. ...
The oxidation number of oxygen in compounds is usually -2.
Explanation:
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