Import Question JSON

Current Question (ID: 8108)

Question:

$\text{The correct order of H-bond strength in the following compounds is:}$

Options:

1. $\text{H}_2\text{O} > \text{H}_2\text{O}_2 > \text{HF} > \text{H}_2\text{S}$
2. $\text{HF} > \text{H}_2\text{O}_2 > \text{H}_2\text{O} > \text{H}_2\text{S}$
3. $\text{HF} > \text{H}_2\text{O} > \text{H}_2\text{S} > \text{H}_2\text{O}_2$
4. $\text{HF} > \text{H}_2\text{O} > \text{H}_2\text{O}_2 > \text{H}_2\text{S}$

Solution:

$\text{HINT: Strength of H-Bonding } \propto \text{ Electronegativity } \propto \text{ Size of atom}$ $\text{Explanation:}$ $\text{STEP 1:}$ $\text{Two Requirements for Hydrogen Bonding:}$ $\text{1. Molecules has a hydrogen attached to a highly electronegative atom (N, O, F). (hydrogen bond donor)}$ $\text{2. Molecule has a lone pair of electrons on a small highly electronegative atom (N, O, F). (hydrogen bond acceptor)}$ $\text{STEP 2:}$ $\text{Sulphur doesn't form H-bonding. So, there is no H-bonding in } \text{H}_2\text{S}\text{.}$ $\text{Because of its high electronegativity and small size, HF has the strongest H-bonding.}$ $\text{As for the number of hydrogen bonds, if we look at the structure of ice, each hydrogen atom of water is involved in a hydrogen bond (each oxygen is involved in two). But peroxide has a larger number of hydrogen bonds.}$ $\text{STEP 3:}$ $\text{So, the correct order of strength of the H-bond is: } \text{HF} > \text{H}_2\text{O}_2 > \text{H}_2\text{O} > \text{H}_2\text{S}$

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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
}