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Current Question (ID: 8010)

Question:

Which of the following is a pair of polar molecules?

Options:

1. $\text{CO}_2 \text{ and } \text{H}_2\text{O}$
2. $\text{BF}_3 \text{ and } \text{PCl}_3$
3. $\text{SO}_2 \text{ and } \text{SCl}_2$ (Correct)
4. $\text{CS}_2 \text{ and } \text{SO}_3$

Solution:

To determine which pair consists of polar molecules, we need to analyze the geometry and bond polarity of each molecule. 1. **$\text{CO}_2$ (Carbon Dioxide):** * Structure: Linear (O=C=O) * Bond polarity: C-O bonds are polar due to electronegativity difference. * Overall polarity: The two equal and opposite bond dipoles cancel each other out, making $\text{CO}_2$ a non-polar molecule. * **$\text{H}_2\text{O}$ (Water):** * Structure: Bent (due to two lone pairs on oxygen) * Bond polarity: O-H bonds are polar. * Overall polarity: The bent shape prevents the bond dipoles from canceling, making $\text{H}_2\text{O}$ a polar molecule. * Conclusion for Pair 1: Not both are polar. 2. **$\text{BF}_3$ (Boron Trifluoride):** * Structure: Trigonal planar * Bond polarity: B-F bonds are polar. * Overall polarity: The symmetrical trigonal planar geometry causes the three equal bond dipoles to cancel, making $\text{BF}_3$ a non-polar molecule. * **$\text{PCl}_3$ (Phosphorus Trichloride):** * Structure: Trigonal pyramidal (due to one lone pair on phosphorus) * Bond polarity: P-Cl bonds are polar. * Overall polarity: The trigonal pyramidal shape and the presence of a lone pair lead to a net dipole moment, making $\text{PCl}_3$ a polar molecule. * Conclusion for Pair 2: Not both are polar. 3. **$\text{SO}_2$ (Sulfur Dioxide):** * Structure: Bent (due to one lone pair on sulfur) * Bond polarity: S-O bonds are polar. * Overall polarity: The bent shape results in a net dipole moment, making $\text{SO}_2$ a polar molecule. * **$\text{SCl}_2$ (Sulfur Dichloride):** * Structure: Bent (due to two lone pairs on sulfur) * Bond polarity: S-Cl bonds are polar. * Overall polarity: The bent shape results in a net dipole moment, making $\text{SCl}_2$ a polar molecule. * Conclusion for Pair 3: Both $\text{SO}_2$ and $\text{SCl}_2$ are polar. 4. **$\text{CS}_2$ (Carbon Disulfide):** * Structure: Linear (S=C=S) * Bond polarity: C-S bonds are polar. * Overall polarity: The two equal and opposite bond dipoles cancel, making $\text{CS}_2$ a non-polar molecule. * **$\text{SO}_3$ (Sulfur Trioxide):** * Structure: Trigonal planar * Bond polarity: S-O bonds are polar. * Overall polarity: The symmetrical trigonal planar geometry causes the three equal bond dipoles to cancel, making $\text{SO}_3$ a non-polar molecule. * Conclusion for Pair 4: Not both are polar. Therefore, the pair of polar molecules is $\text{SO}_2$ and $\text{SCl}_2$.

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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
}