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The colour of transition metal ion is a...

The colour of transition metal ion is attributed to:

A

small size metal ions

B

absorption of light in UV region

C

complete (ns) subshell

D

incomplete (n-1) d subshell

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The correct Answer is:
**Step-by-Step Solution:** 1. **Understanding the Color of Transition Metal Ions:** - Transition metal ions exhibit color due to the presence of unpaired electrons in their d-orbitals. 2. **Role of d-Orbitals:** - Transition metals have partially filled d-orbitals. The electrons in these d-orbitals can absorb specific wavelengths of light. 3. **Crystal Field Theory:** - When transition metal ions are placed in a ligand field (such as in a complex), the d-orbitals split into different energy levels. This splitting allows for electronic transitions between these levels. 4. **Absorption of Light:** - The energy difference between the split d-orbitals corresponds to the energy of visible light. When light is absorbed, an electron is promoted from a lower energy d-orbital to a higher energy d-orbital. 5. **Color Observation:** - The color observed is the complementary color of the light absorbed. For example, if a transition metal ion absorbs light in the red region, it will appear green. 6. **Conclusion:** - The color of transition metal ions is primarily attributed to the presence of unpaired electrons in the incomplete (n-1)d subshell. 7. **Identifying the Correct Option:** - Among the given options, the one that correctly describes the reason for the color of transition metal ions is "incomplete (n-1)d subshell." **Final Answer:** - The color of transition metal ions is attributed to the presence of unpaired electrons in the incomplete (n-1)d subshell. ---
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The colours of the transition metal are due to d-d excitation. The energy required for d-d electron axcitation is available in the visible range. Transition metal ions have the tendency to absorb certain rediations from the visible region and exhibit the complementary colour. The transition metal ions which have completely filled d-orbitals are colourless as the excitation of electron or electrons is not possible within d-orbitals. The transition metal ions which have completely empthy d-orbitals are also colourless. In KMnO_4 and K_2Cr_2O_7 , there are no unpaired electrons at the central atom but they are dep in colour. The colour of these compounds is due to charge transfer spectrum. for example in MnO_4 electron is momentrily transferred from O to the metal and thuys oxygen changes from O^(2-) and O^(ɵ) maganese from Mn^(7+) to Mn^(6+) . Q. Which of the following is paramagnetic as well as coloured ion?

The colours of the transition metal are due to d-d excitation. The energy required for d-d electron axcitation is available in the visible range. Transition metal ions have the tendency to absorb certain rediations from the visible region and exhibit the complementary colour. The transition metal ions which have completely filled d-orbitals are colourless as the excitation of electron or electrons is not possible within d-orbitals. The transition metal ions which have completely empthy d-orbitals are also colourless. In KMnO_4 and K_2Cr_2O_7 , there are no unpaired electrons at the central atom but they are dep in colour. The colour of these compounds is due to charge transfer spectrum. for example in MnO_4 electron is momentrily transferred from O to the metal and thuys oxygen changes from O^(2-) and O^(ɵ) maganese from Mn^(7+) to Mn^(6+) . Q. Which is a coloured ion?

The colours of the transition metal are due to d-d excitation. The energy required for d-d electron axcitation is available in the visible range. Transition metal ions have the tendency to absorb certain rediations from the visible region and exhibit the complementary colour. The transition metal ions which have completely filled d-orbitals are colourless as the excitation of electron or electrons is not possible within d-orbitals. The transition metal ions which have completely empthy d-orbitals are also colourless. In KMnO_4 and K_2Cr_2O_7 , there are no unpaired electrons at the central atom but they are dep in colour. The colour of these compounds is due to charge transfer spectrum. for example in MnO_4 electron is momentrily transferred from O to the metal and thuys oxygen changes from O^(2-) and O^(ɵ) maganese from Mn^(7+) to Mn^(6+) . Q. Select the correct statement:

The colours of the transition metal are due to d-d excitation. The energy required for d-d electron axcitation is available in the visible range. Transition metal ions have the tendency to absorb certain rediations from the visible region and exhibit the complementary colour. The transition metal ions which have completely filled d-orbitals are colourless as the excitation of electron or electrons is not possible within d-orbitals. The transition metal ions which have completely empthy d-orbitals are also colourless. In KMnO_4 and K_2Cr_2O_7 , there are no unpaired electrons at the central atom but they are dep in colour. The colour of these compounds is due to charge transfer spectrum. for example in MnO_4 electron is momentrily transferred from O to the metal and thuys oxygen changes from O^(2-) and O^(ɵ) maganese from Mn^(7+) to Mn^(6+) . Q. Which of the following compounds is (are) coloured due to charge transfer spectra and not due to d-d transition?

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