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Questions
Account for the following:
Cr2+ is a strong reducing agent.
Give reasons for the following statement:
Cr2+ is a strong reducing agent.
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Solution
Cr2+ is strongly reducing in nature. It has a d4 configuration. While acting as a reducing agent, it gets oxidised to Cr3+ (with electronic configuration d3). This d3 configuration can be written as \[\ce{t^3_{2g}}\] configuration, which is a more stable configuration.
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RELATED QUESTIONS
Why do the transition elements have higher enthalpies of atomisation?
For M2+/M and M3+/M2+ systems, the E° 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 stability of Fe3+ in acid solution as compared to that of Cr3+ or Mn3+ and
- the ease with which iron can be oxidised as compared to a similar process for either chromium or manganese metal.
Compare the stability of +2 oxidation state for the elements of the first transition series.
Which among the following transition metal has the lowest melting point?
Generally transition elements form coloured salts due to the presence of unpaired electrons. Which of the following compounds will be coloured in solid-state?
Although fluorine is more electronegative than oxygen, but the ability of oxygen to stabilise higher oxidation states exceeds that of fluorine. Why?
Identify the metal and justify your answer.
Carbonyl \[\ce{M(CO)5}\]
Identify the metal and justify your answer.
\[\ce{MO3F}\]
Assertion (A): Transition metals show their highest oxidation state with oxygen.
Reason (R): The ability of oxygen to form multiple bonds to metals.
A pair of coloured ions is ______.
