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Current Question (ID: 18677)

Question:

$\text{The IUPAC name for complex ion, } [\text{Fe(CN)}_6]^{3-} \text{ is:}$

Options:

1. $\text{Hexacyanoiron(III) ion}$
2. $\text{Hexacyanitoferrate(III) ion}$
3. $\text{Tricyanoferrate(III) ion}$
4. $\text{Hexacyanidoferrate(III) ion}$

Solution:

$\text{HINT: For anion complex, ate is used in the name of the metal ion.}$ $\text{Explanation: The given complex is } [\text{Fe(CN)}_6]^{3-}$ $1. \text{ Since complex ion is an anion, the name of the metal ends with suffix } -\text{ate along with its oxidation number in the complex ion.}$ $2. \text{ Six } \text{CN}^- \text{ ligands are represented as cyanide, } \text{``hexa'' prefix will be used for this.}$ $3. \text{ Let oxidation number of Fe is } ``x''$ $x + 6(-1) = -3$ $x = +3$ $4. \text{ Thus, IUPAC name of } [\text{Fe(CN)}_6]^{3-} \text{ is hexacyanidoferrate(III) ion.}$

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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
}