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Current Question (ID: 18849)

Question:

$\text{Which of the following statements is false?}$

Options:

1. $\text{Cr}^{2+} \text{ is strongly oxidizing while manganese(III) is strongly reducing.}$
2. $\text{Cobalt(II) is stable in an aqueous solution but in the presence of complexing reagents, it is easily oxidized.}$
3. $\text{The d}^1 \text{ configuration is very unstable in ions.}$
4. $\text{None of the above.}$

Solution:

$\text{HINT: Cr}^{2+} \text{ is strongly reducing in nature.}$ $\text{Explanation:}$ $\text{(i) Cr}^{2+} \text{ is strongly reducing in nature. It has a d}^4 \text{ configuration. While acting as a reducing agent, it gets oxidized to Cr}^{3+} \text{ (electronic configuration, d}^3) \text{ which is a more stable configuration.}$ $\text{In the case of Mn}^{3+} \text{ (d}^4), \text{ it acts as an oxidizing agent and gets reduced to Mn}^{2+} \text{ (d}^5). \text{ This has an exactly half-filled d-orbital and is highly stable.}$ $\text{(ii) Co(II) is stable in aqueous solutions. However, in the presence of strong field complexing reagents, it is oxidized to Co (III).}$ $\text{Although the 3rd ionization energy for Co is high, but the higher amount of crystal field stabilization energy (CFSE) released in the presence of strong field ligands overcomes this ionization energy.}$ $\text{(iii) The ions in d}^1 \text{ configuration tend to lose one more electron to get into stable d}^0 \text{ configuration.}$ $\text{Also, the hydration or lattice energy is more than sufficient to remove the only electron present in the d-orbital of these ions.}$ $\text{Therefore, they act as reducing agents.}$

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Upload a JSON file containing LaTeX/MathJax formatted question, options, and solution.

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
}