To determine the oxidation state of nitrogen ([tex]\(N\)[/tex]) in the ammonium ion ([tex]\(NH_4^+\)[/tex]), follow these steps:
1. Understand the overall charge: The ammonium ion ([tex]\(NH_4^+\)[/tex]) has an overall charge of [tex]\(+1\)[/tex].
2. Oxidation state of hydrogen: Each hydrogen atom typically has an oxidation state of [tex]\(+1\)[/tex].
3. Count the number of hydrogen atoms: In [tex]\(NH_4^+\)[/tex], there are 4 hydrogen atoms.
4. Calculate the total oxidation state contributed by hydrogen:
[tex]\[
4 \text{ (hydrogen atoms)} \times +1 \text{ (oxidation state per hydrogen)} = +4
\][/tex]
5. Set up the equation for the overall oxidation state: Let the oxidation state of nitrogen be [tex]\(N\)[/tex]. The sum of the oxidation states of all atoms in the ion must equal the overall charge of the ion. Therefore, we set up the equation:
[tex]\[
N + (+4) = +1
\][/tex]
6. Solve for the oxidation state of nitrogen:
[tex]\[
N + 4 = 1 \\
N = 1 - 4 \\
N = -3
\][/tex]
Thus, the oxidation state of nitrogen in [tex]\(NH_4^+\)[/tex] is [tex]\(-3\)[/tex].
The correct answer is:
D. [tex]\(-3\)[/tex]
