Oxidation state of nitrogen is incorrectly given for:

Options

A. `{:("Compound","Oxidation State"),([Co(NH_(3))_(5)Cl]Cl_(2),-3):}`
B. `{:("Compound","Oxidation State"),(NH_(2)OH,-1):}`
C. `{:("Compound","Oxidation State"),((N_(2)H_(5))_(2)SO_(4),+2):}`
D. `{:("Compound","Oxidation State"),(Mg_(3)N_(2),-3):}`

Answer

To determine the oxidation state of nitrogen in various compounds, we will analyze each option step by step.

### Step 1: Analyze the first compound, Co(NH3)5Cl2
1. **Identify the overall charge**: The complex has a counter ion of Cl2, which indicates that the overall charge of the complex is +2.
2. **Set up the equation**: Let the oxidation state of cobalt (Co) be \(X\). The ammonia (NH3) is a neutral ligand, contributing 0 to the charge. The chlorine (Cl) contributes -1 for each Cl atom.
\[ X + 5(0) + (-1) = +2 \]
Simplifying this gives:
\[ X - 1 = +2 \implies X = +3 \]
3. **Conclusion**: The oxidation state of cobalt is +3, which is correctly given.

### Step 2: Analyze the second compound, NH2OH (Hydroxylamine)
1. **Identify the overall charge**: NH2OH is a neutral molecule, so the overall oxidation state must be 0.
2. **Set up the equation**: Let the oxidation state of nitrogen be \(X\).
\[ X + 3(+1) + (-2) = 0 \]
Simplifying this gives:
\[ X + 3 - 2 = 0 \implies X + 1 = 0 \implies X = -1 \]
3. **Conclusion**: The oxidation state of nitrogen is -1, which is correctly given.

### Step 3: Analyze the third compound, N2H5SO4
1. **Identify the overall charge**: N2H5SO4 is a neutral molecule, so the overall oxidation state must be 0.
2. **Set up the equation**: Let the oxidation state of nitrogen be \(X\).
\[ 2X + 5(+1) + (-2) = 0 \]
Simplifying this gives:
\[ 2X + 5 - 2 = 0 \implies 2X + 3 = 0 \implies 2X = -3 \implies X = -\frac{3}{2} \]
However, since we have 2 nitrogen atoms, we can also express this as:
\[ 4X + 10 - 2 = 0 \implies 4X + 8 = 0 \implies 4X = -8 \implies X = -2 \]
3. **Conclusion**: The oxidation state of nitrogen is -2, but it is incorrectly given as +2.

### Step 4: Analyze the fourth compound, Mg3N2
1. **Identify the overall charge**: Mg3N2 is a neutral compound, so the overall oxidation state must be 0.
2. **Set up the equation**: Let the oxidation state of nitrogen be \(X\).
\[ 3(+2) + 2X = 0 \]
Simplifying this gives:
\[ 6 + 2X = 0 \implies 2X = -6 \implies X = -3 \]
3. **Conclusion**: The oxidation state of nitrogen is -3, which is correctly given.

### Final Conclusion:
The oxidation state of nitrogen is incorrectly given for the compound **N2H5SO4**, where it should be -2 but is incorrectly stated as +2.