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What is the oxidation state of [tex]N[/tex] in [tex]NH_4^+[/tex]?

A. -5
B. +1
C. +5
D. -3


Sagot :

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]