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Current Question (ID: 7971)

Question:

The number of sigma ($\sigma$) and pi ($\pi$) bonds in pent-2-en-4-yne is:

Options:

1. $13\ \sigma$ bonds and no $\pi$ bond.
2. $10\ \sigma$ bonds and $3\ \pi$ bonds. (Correct)
3. $8\ \sigma$ bonds and $5\ \pi$ bonds.
4. $11\ \sigma$ bonds and $2\ \pi$ bonds.

Solution:

HINT: Molecule contains one double bond and one triple bond. Explanation: Single bond represents sigma bond, double bond represents one sigma and one $\pi$ bond. Triple bond represents one sigma and two $\pi$ bonds. The structure of pent-2-en-4-yne is as follows: $\text{CH}_3 - \text{CH} = \text{CH} - \text{C} \equiv \text{C} - \text{H}$ The number of sigma bonds is $3 \text{ (in CH}_3) + 1 \text{ (C-C single)} + 1 \text{ (C=C double)} + 1 \text{ (C-H in CH)} + 1 \text{ (C-C single)} + 1 \text{ (C\equiv C triple)} + 1 \text{ (C-H in CH)} = 10 \ \sigma \text{ bonds}$. The number of pi bonds is $1 \text{ (in C=C double bond)} + 2 \text{ (in C}\equiv \text{C triple bond)} = 3 \ \pi \text{ bonds}$. Thus, the molecule contains a total of $10$ sigma bonds and $3$ pi bonds.

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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
}