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The colour of the transition metal ions ...

The colour of the transition metal ions is due to

A

d-d transition

B

Charger transfer

C

Change in the geometry

D

None

Text Solution

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The correct Answer is:
To answer the question about the color of transition metal ions, we need to analyze the factors that contribute to their coloration. Here’s a step-by-step breakdown of the solution: ### Step 1: Understanding the Electronic Configuration Transition metals have partially filled d-orbitals. The electronic configuration of these metals allows for the possibility of d-d transitions, where an electron can be promoted from a lower energy d-orbital to a higher energy d-orbital. **Hint:** Recall that the d-orbitals can hold a maximum of 10 electrons, and their filling can lead to various oxidation states and colors. ### Step 2: D-D Transitions When light (electromagnetic radiation) hits a transition metal ion, it can provide enough energy to promote an electron from a lower energy d-orbital to a higher energy d-orbital. This process is known as a d-d transition. The specific wavelengths of light absorbed during this transition correspond to the energy difference between the two d-orbitals involved. **Hint:** Think about how the absorption of specific wavelengths of light results in the complementary color being observed. ### Step 3: Role of Electromagnetic Radiation The energy of the absorbed light falls within the visible spectrum. The wavelengths of light that are absorbed determine the color that is observed. For example, if a transition metal ion absorbs light in the red region, it may appear green, which is the complementary color. **Hint:** Remember that the color observed is always the color that is not absorbed by the ion. ### Step 4: Charge Transfer Transitions In addition to d-d transitions, transition metal ions can also exhibit charge transfer transitions. This occurs when an electron moves from a ligand to the metal ion or from the metal ion to a ligand. These transitions can also contribute to the color of the complex. **Hint:** Consider the impact of ligands and their ability to influence the color through charge transfer. ### Step 5: Conclusion The color of transition metal ions is primarily due to: 1. **D-D transitions**: The promotion of electrons within the d-orbitals. 2. **Charge transfer transitions**: The movement of electrons between the metal and ligands. Thus, both d-d transitions and charge transfer are responsible for the coloration observed in transition metal ions. **Final Answer:** The color of transition metal ions is due to d-d transitions and charge transfer transitions.
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The colour of transition metal ions is due to ............... in d-subshell and .............. transition.

The colour of the transition metal ions is//are due to:

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?

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. K_2Cr_2O_7 gives coloured solution in water. The colour is due to

The colour of transition metal ion is attributed to:

The colour of transition metal ion is attributed to:

Transition metals:

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