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Oxidation number of nitrogen is highest ...

Oxidation number of nitrogen is highest in :

A

`N_3H`

B

`N_2O_4`

C

`NH_4OH`

D

`NH_3`

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To determine the oxidation number of nitrogen in the given compounds, we will analyze each compound step by step. ### Step 1: Analyze the first compound, N3H 1. Let the oxidation number of nitrogen be \( X \). 2. The total oxidation state of the molecule must equal zero since it is neutral. 3. The equation can be set up as: \[ 3X + 1 = 0 \] 4. Solving for \( X \): \[ 3X = -1 \implies X = -\frac{1}{3} \] 5. Therefore, the oxidation number of nitrogen in N3H is \(-\frac{1}{3}\). ### Step 2: Analyze the second compound, N2O4 1. Let the oxidation number of nitrogen be \( X \). 2. The total oxidation state of the molecule must equal zero. 3. The equation can be set up as: \[ 2X + 4(-2) = 0 \] 4. Solving for \( X \): \[ 2X - 8 = 0 \implies 2X = 8 \implies X = 4 \] 5. Therefore, the oxidation number of nitrogen in N2O4 is \( +4 \). ### Step 3: Analyze the third compound, NH4OH 1. Let the oxidation number of nitrogen be \( X \). 2. The total oxidation state of the molecule must equal zero. 3. The equation can be set up as: \[ X + 4(+1) + 1 + 4(-2) = 0 \] 4. Simplifying gives: \[ X + 4 - 8 + 1 = 0 \implies X - 3 = 0 \implies X = -3 \] 5. Therefore, the oxidation number of nitrogen in NH4OH is \( -3 \). ### Step 4: Analyze the fourth compound, NH3 1. Let the oxidation number of nitrogen be \( X \). 2. The total oxidation state of the molecule must equal zero. 3. The equation can be set up as: \[ X + 3(+1) = 0 \] 4. Solving for \( X \): \[ X + 3 = 0 \implies X = -3 \] 5. Therefore, the oxidation number of nitrogen in NH3 is \( -3 \). ### Conclusion After analyzing all four compounds, we find: - N3H: Oxidation number of nitrogen = \(-\frac{1}{3}\) - N2O4: Oxidation number of nitrogen = \( +4\) - NH4OH: Oxidation number of nitrogen = \(-3\) - NH3: Oxidation number of nitrogen = \(-3\) The highest oxidation number of nitrogen is found in **N2O4**, which is \( +4 \). ### Final Answer The compound with the highest oxidation number of nitrogen is **N2O4**. ---

To determine the oxidation number of nitrogen in the given compounds, we will analyze each compound step by step. ### Step 1: Analyze the first compound, N3H 1. Let the oxidation number of nitrogen be \( X \). 2. The total oxidation state of the molecule must equal zero since it is neutral. 3. The equation can be set up as: \[ 3X + 1 = 0 ...
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Knowledge Check

  • The oxidation state of nitrogen is highest in

    A
    `N_(3)H`
    B
    `NH_(2)OH`
    C
    `N_(2)H_(2)`
    D
    `NH_(3)`
  • The oxidation state of nitrogen is highest in

    A
    `N_(3)H`
    B
    `NH_(3)`
    C
    `NH_(2)OH`
    D
    `N_(2)H_(4)`
  • The oxidation state of nitrogen is highest in

    A
    `NH_2OH`
    B
    `N_3H`
    C
    `N_2H_4`
    D
    `NH_3`
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