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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)
संबंधित प्रश्न
Why +2 oxidation state of manganese is more stable?
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?
Account for the following:
Cu+ ion is unstable in aqueous solution.
How is the variability in oxidation states of transition metals different from that of the non-transition metals? Illustrate with examples.
Calculate the number of unpaired electrons in the following gaseous ions:
Mn3+, Cr3+, V3+ and Ti3+. Which one of these is the most stable in an aqueous solution?
Give reasons: Sc3+ is colourless in aqueous solution whereas Ti3+ is coloured.
Why do transition metal ions possess a great tendency to form complexes?
In lake test for Al3+ ions, there is the formation of coloured ‘floating lake’. It is due to ______.
Interstitial compounds are formed when small atoms are trapped inside the crystal lattice of metals. Which of the following is not the characteristic property of interstitial compounds?
When acidified \[\ce{K2Cr2O7}\] solution is added to \[\ce{Sn^{2+}}\] salts then \[\ce{Sn^{2+}}\] changes to ______.
While filling up of electrons in the atomic orbitals, the 4s orbital is filled before the 3d orbital but reverse happens during the ionisation of the atom. Explain why?
Mercury is the only metal liquid at room temperature due to its:-
The number of terminal oxygen atoms present in the product B obtained from the following reactions is:
\[\ce{FeCr2O4 + Na2CO3 + O2 -> A + Fe2O3 + CO2}\]
\[\ce{A + H^+ -> B + H2O + Na^+}\]
The second ionization enthalpies of chromium and manganese are 1592 and 1509 kJ/mol respectively. Explain the lower value of Mn.
A pair of coloured ions is ______.
Explain the use of different transition metals as catalysts.
Give a reason for the following:
Zinc, cadmium and mercury are considered as d-block elements but not regarded as transition elements.
For M2+/M and M3+/M2+systems, the EΘ values for some metals are as follows:
| Cr2+/Cr | −0.9 V |
| Mn2+/Mn | −1.2 V |
| Fe2+/Fe | −0.4 V |
| Cr3/Cr2+ | −0.4 V |
| Mn3+/Mn2+ | +1.5 V |
| Fe3+/Fe2+ | +0.8 V |
Use this data to comment upon:
The ease with which iron can be oxidised as compared to a similar process for either chromium or manganese metal.
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Atomic sizes
