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प्रश्न
Write down the number of 3d electrons in the following ion:
Cu2+
Indicate how would you expect the five 3d orbitals to be occupied for this hydrated ions (octahedral).
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उत्तर १
| Metal ion | Number of d-electrons | Filling of d-orbitals |
| Cu2+ | 9 | \[\ce{t^6_{2g}e^3_g}\] |
उत्तर २
Cu2+: 3d9
Filling of orbitals in an octahedral hydrated ion:
Cu2+: \[\ce{t^6_{2g}e^3_g}\]
| ↑↓ | ↑ | eg | |
| ↑↓ | ↑↓ | ↑↓ | t2g |
(1 unpaired electron)
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संबंधित प्रश्न
ln which pair highest oxidation states of transition metals are found:
The elements of 3d transition series are given as: Sc Ti V Cr Mn Fe Co
Answer the following: Which element is a strong oxidising agent in +3 oxidation state and why?
Why do the transition elements have higher enthalpies of atomisation?
In 3d series (Sc to Zn), which element has the lowest enthalpy of atomisation and why?
How would you account for the following: Transition metals form complex compounds.
|
`E_((M^(2+)/M)` |
Cr | Mn | Fe | Co | Ni | Cu |
| -0.91 | -1.18 | -0.44 | -0.28 | -0.25 | -0.34 |
From the given data of E0 values, answer the following questions :
(1) Why is `E_(((Cu^(2+))/(Cu)))` value exceptionally positive
(2) Why is `E_(((Mn^(2+))/(Mn)))` value is highly negative as compared to other elements
(3) Which is the stronger reducing agents Cr2+ or Fe2+ ? Give Reason.
Explain why Cu+ ion is not stable in aqueous solutions?
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The d1 configuration is very unstable in ions.
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| Example | Magnetic Moment (BM) |
| K2[MnCl4] | 5.9 |
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