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Current Question (ID: 8077)

Question:

Paramagnetic species among the following is:

Options:

1. $ \text{CO} $
2. $ \text{O}_2^{-} $ (Correct)
3. $ \text{CN}^{-} $
4. $ \text{NO}^{+} $

Solution:

$\text{HINT: Paramagnetic species contains unpaired electrons in their molecular orbital electronic configuration.} \n\n \text{Explanation:} \n\n \text{Molecular orbital configuration of the given species is given as :} \n\n \text{CO} \: (6+8=14) = \sigma_{1s}^{2}, \sigma_{1s}^{\ast 2}, \sigma_{2s}^{2}, \sigma_{2s}^{\ast 2}, \pi_{2p_{x}}^{2} \approx \pi_{2p_{y}}^{2}, \sigma_{2p_{z}}^{2} \n\n (\text{All the electrons are paired so it is diamagnetic}) \n\n \text{Electronic configuration of } \text{O}_2^{-} \: (8+8+1=17) = \sigma_{1s}^{2}, \sigma_{1s}^{\ast 2}, \sigma_{2s}^{2}, \sigma_{2s}^{\ast 2}, \pi_{2p_{x}}^{2} \approx \pi_{2p_{y}}^{2}, \pi_{2p_{x}}^{\ast 2} \approx \pi_{2p_{y}}^{\ast 1} \n\n \text{This contains an unpaired electron. So, } \text{O}_2^{-} \text{ is paramagnetic in nature.}$

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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
}