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Current Question (ID: 18745)

Question:

$\text{The complex ion among the following that cannot absorb visible light is:}$

Options:

1. $[\text{Ni(CN)}_4]^{2-}$
2. $[\text{Cr(NH}_3)_6]^{3+}$
3. $[\text{Fe(H}_2\text{O})_6]^{2+}$
4. $[\text{Ni(H}_2\text{O})_6]^{2+}$

Solution:

$\text{STEP 1: In } [\text{Ni(CN)}_4]^{2-}, \text{ Ni is present as } \text{Ni}^{2+}$ $\text{Ni}^{2+} = [\text{Ar}] \ 3d^8 \ 4s^0$ $\text{As cyanide is a strong field ligand, it is seen that the pairing will take place and due to fully filled orbital, it will not absorb visible light.}$ $\text{STEP 2: For the other complexes, the configuration is:}$ $[\text{Cr(NH}_3)_6]^{3+}, \text{ Cr}^{3+} = [\text{Ar}] \ 3d^3 \ 4s^0$ $[\text{Fe(H}_2\text{O})_6]^{2+}, \text{ Fe}^{2+} = [\text{Ar}] \ 3d^6 4s^0$ $[\text{Ni(H}_2\text{O})_6]^{2+}, \text{ Ni}^{2+} = [\text{Ar}] \ 3d^8 \ 4s^0$ $\text{The other complex contains unpaired electron hence, it can show transition at visible region.}$

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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
}