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Current Question (ID: 10682)

Question:

$\text{The correct order of the bond dissociation enthalpy of halogen molecules is:}$

Options:

1. $\text{Cl}_2 > \text{Br}_2 > \text{F}_2 > \text{I}_2$ (Correct)
2. $\text{Br}_2 > \text{I}_2 > \text{F}_2 > \text{Cl}_2$
3. $\text{F}_2 > \text{Cl}_2 > \text{Br}_2 > \text{I}_2$
4. $\text{I}_2 > \text{Br}_2 > \text{Cl}_2 > \text{F}_2$

Solution:

$\text{HINT: Bond dissociation enthalpy did not follow a regular trend (down the group bond dissociation energy decreases)}$ $\text{Explanation:}$ $\text{As the size increase, bond dissociation enthalpy decreases. Also as the size of atoms get smaller, electron pairs on the two atoms get close enough to experience repulsion.}$ $\text{In the case of F}_2\text{, repulsion is large due to its small size and the bond becomes weaker.}$ $\text{Thus, the order of bond dissociation energy is : Cl}_2 > \text{Br}_2 > \text{F}_2 > \text{I}_2$

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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
}