🤓 Based on our data, we think this question is relevant for Professor Goodman's class at MONTANA.
We’re being asked to determine the oxidation state of the specified element in each given compound.
The rules for oxidation states are as follows:
A. General Rules:
1. For an atom in its elemental form (Zn, Cl2, C(graphite), etc.) O.S. = 0
2. For an ion (Li+, Al3+, etc.) O.S. = charge
B. Specific Rules:
1. Group 1A O.S. = +1
2. Group 2A O.S. = +2
3. Hydrogen O.S. = +1, with nonmetals
O.S. = –1 with metals and boron
4. Fluorine O.S. = –1
5. Oxygen O.S. = –1 in peroxides (X2O2, X = Group 1A)
O.S. = –1/2 in superoxides (XO2, X = Group 1A)
O.S. = –2 in other compounds
6. Group 7A O.S. = –1 (except when bonded to O)
a. What is the oxidation state of an individual bromine atom in NaBrO 3?
b. What is the oxidation state of an individual nitrogen atom in NH2OH?
c. What is the oxidation state of an individual sulfur atom in SO 42-?
d. What is the oxidation state of each individual carbon atom in C 2O42-?
Express the oxidation state numerically (e.g., +1).