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प्रश्न
To what extent do the electronic configurations decide the stability of oxidation states in the first series of the transition elements? Illustrate your answer with examples.
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उत्तर
- The ions in the oxidation state, in which the ions have fully filled or half-filled d shells, are more stable.
- For example, the +2 state of Mn is more stable than its other oxidation states.
- Because Mn2+ has a half-filled 3d5 shell. Similarly, the +2 state of Zn is its most stable state because it has a fully filled 3d10 shell.
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संबंधित प्रश्न
Which metal in the first transition series (3d series) exhibits + 1 oxidation state most frequently and why?
Account for the following:
E° value for the Mn3+/Mn2+ couple is much more positive than that for Cr3+/Cr2+.
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
How would you account for the following:
The d1 configuration is very unstable in ions.
The transition metals show _________ character because of the presence of unpaired· electrons and Cu+ is ____________ because of its electronic configuration is [Ar]3d10
Give reasons for the following:
The transition metals generally form coloured compounds.
Transition metals with lowest melting point is ______.
Highest oxidation state of manganese in fluoride is \[\ce{+4 (MnF4)}\] but highest oxidation state in oxides is \[\ce{+7 (Mn2O7)}\] because ______.
Why EΘ values for Mn, Ni and Zn are more negative than expected?
Answer the following question:
Which element of the first transition series has lowest enthalpy of atomisation?
Identify the metal and justify your answer.
Carbonyl \[\ce{M(CO)5}\]
On strong heating AgNO3, the gases evolved are:-
Which one of the following characters tie of the transition metal is associated with higher catalytic activity?
Account for the following:
Transition metals form alloys.
Consider the following standard electrode potential values:
\[\ce{Fe^{3+}_{ (aq)} + e^- -> Fe^{2+}_{ (aq)}}\], E0 = +0.77 V
\[\ce{MnO^{-4}_{ (aq)} + 8H^+ + 5e^- -> Mn^{2+}_{ (aq)} + 4H2O_{(l)}}\], E0 = +1.51 V
What is the cell potential for the redox reaction?
Consider the following standard electrode potential values:
\[\ce{Sn^{2+}_{ (aq)} + 2e^- -> Sn_{(s)}}\]; E0 = −0.14 V
\[\ce{Fe^{3+}_{ (aq)} + e^- -> Fe^{2+}_{ (aq)}}\]; E0 = +0.77 V
What is the cell reaction and potential for the spontaneous reaction that occurs?
Give two similarities in the properties of Sc and Zn.
‘Spin only’ magnetic moment is the same for which of the following ions?
- Ti3+
- Cr2+
- Mn2+
- Fe2+
- Sc3+
Choose the most appropriate answer from the options given below:
