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Current Question (ID: 7967)

Question:

In $\text{PO}_4^{3-}$ ion, the formal charge on the oxygen atom of the $\text{P-O}$ bond is:

Options:

1. $+1$
2. $-1$
3. $-0.75$ (Correct)
4. $+0.75$

Solution:

HINT: $\text{Formal charge} = \frac{\text{Total charge}}{\text{Number of O - atom}}$ Explanation: The formal charge over an atom of a polyatomic molecule or ion is the difference between the valence electron of that atom in the elemental state and the number of electrons assigned to that atom in Lewis structure. In $\text{PO}_4^{3-}$ ion, the formal charge on each $\text{O-atom}$ of $\text{P-O}$ bond is calculated as follows: $\text{Formal charge} = \frac{\text{Total charge}}{\text{Number of O - atom}} = \frac{-3}{4} = -0.75$ In the resonance structure, a total of $-3$ charge is distributed over four oxygen atoms.

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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
}