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Current Question (ID: 7663)

Question:

The incorrect statement about ionization enthalpy is:

Options:

1. Ionization enthalpy increases for each successive electron.
2. Noble gases have the highest ionization enthalpy.
3. A big jump in ionization enthalpy indicates a stable configuration.
4. Ionization enthalpy of oxygen is higher than that of nitrogen. (Correct)

Solution:

HINT: Half filled orbital has high IE than partially filled orbital. Explanation: Ionization energy can be thought of as the energy required to remove an electron from the valence shell of an atom. Noble gases have highest ionisation enthalpy because of fully filled valence shell. Nitrogen is known to have a half-filled p-orbital and is quite stable. Therefore, the ionization enthalpy of nitrogen will be higher than that of oxygen.

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Expected JSON Format:

{
  "question": "The mass of carbon present in 0.5 mole of $\\mathrm{K}_4[\\mathrm{Fe(CN)}_6]$ is:",
  "options": [
    {
      "id": 1,
      "text": "1.8 g"
    },
    {
      "id": 2,
      "text": "18 g"
    },
    {
      "id": 3,
      "text": "3.6 g"
    },
    {
      "id": 4,
      "text": "36 g"
    }
  ],
  "solution": "\\begin{align}\n&\\text{Hint: Mole concept}\\\\\n&1 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\text{ moles of carbon atom}\\\\\n&0.5 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\times 0.5 \\text{ mol} = 3 \\text{ mol}\\\\\n&1 \\text{ mol of carbon} = 12 \\text{ g}\\\\\n&3 \\text{ mol carbon} = 12 \\times 3 = 36 \\text{ g}\\\\\n&\\text{Hence, 36 g mass of carbon present in 0.5 mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6].\n\\end{align}",
  "correct_answer": 4
}