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Current Question (ID: 18801)

Question:

$\text{The transition metals generally form coloured compounds due to:}$

Options:

1. $\text{Absorption of radiation to promote an electron.}$
2. $\text{Presence of ligands, the d-orbitals split up into two sets of orbitals.}$
3. $\text{Energy required to promote an electron in d subshell is low.}$
4. $\text{All of the above.}$

Solution:

$\text{HINT: Transition element show d-d transition.}$ $\text{Explanation:}$ $\text{We know that Transition elements have unfilled d subshells. When transition elements form cations they influence the electron cloud.}$ $\text{There are also elements with their d subshells incompletely filled and the energy of all the d orbitals does not remain the same.}$ $\text{Step 1:}$ $\text{The energy required to promote an electron in the s or p subshell is very high compared to that of promoting an electron in d or f subshell.}$ $\text{Step 2:}$ $\text{Most of the complexes of transition metals are coloured. This is because the absorption of radiation from the visible light region promotes an electron from one of the d-orbitals to another.}$ $\text{In the presence of ligands, the d-orbitals split up into two sets of orbitals having different energies.}$ $\text{Therefore, the transition of electrons can take place from one set to another. The energy required for these transitions is quite small and falls in the visible region of radiation.}$ $\text{The ions of transition metals absorb the radiation of a particular wavelength and the rest is reflected, imparting colour to the solution.}$

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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
}