what is the oxidation # of Nitrogen in NO2^-
The Correct Answer and Explanation is:
To determine the oxidation state of nitrogen (N) in NO2−\text{NO}_2^-NO2−, we follow these steps:
Step 1: Assign known oxidation states
- Oxygen (O) is typically assigned an oxidation state of −2-2−2 in compounds, except in peroxides or when bonded to fluorine.
- The overall charge on the NO2−\text{NO}_2^-NO2− ion is −1-1−1, meaning the sum of the oxidation states of the atoms in the ion must equal −1-1−1.
Step 2: Set up the equation
The ion NO2−\text{NO}_2^-NO2− consists of one nitrogen atom and two oxygen atoms. Let the oxidation state of nitrogen be xxx.
- The oxidation state of each oxygen is −2-2−2, so for two oxygen atoms, the total contribution is 2×(−2)=−42 \times (-2) = -42×(−2)=−4.
- The total charge on the ion is −1-1−1, so the equation for the sum of the oxidation states is:
x+(−4)=−1x + (-4) = -1x+(−4)=−1
Step 3: Solve for xxx
Now, solve the equation for xxx:x−4=−1x – 4 = -1x−4=−1x=−1+4=+3x = -1 + 4 = +3x=−1+4=+3
Conclusion
The oxidation state of nitrogen in NO2−\text{NO}_2^-NO2− is +3+3+3.
Explanation
The oxidation number of nitrogen in this ion is determined by the rule that the sum of the oxidation states in a compound or ion must equal the overall charge. Since each oxygen atom is assigned a typical oxidation state of −2-2−2, and the total charge on the ion is −1-1−1, nitrogen must have an oxidation state of +3+3+3 to balance the equation. Thus, nitrogen in NO2−\text{NO}_2^-NO2− is oxidized to an oxidation state of +3+3+3.
