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Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
Both oxide and fluoride ions are highly electronegative and have a very small size. Due to these properties, they are able to oxidize the metal to its highest oxidation state.
Which is a stronger reducing agent Cr2+ or Fe2+ and why?
The following reactions are involved when Cr2+ and Fe2+ act as reducing agents.
Cr2+17-11-08_Sonali_12_Chemistry_8_10_html_m5602c98c.gif){kind=small}
Cr3+ Fe2+ Fe3+
The 17-11-08_Sonali_12_Chemistry_8_10_html_m2b4a9788.gif){kind=small}
value is −0.41 V and 17-11-08_Sonali_12_Chemistry_8_10_html_m5b1747e2.gif){kind=small}
is +0.77 V. This means that Cr2+ can be easily oxidized to Cr3+, but Fe2+ does not get oxidized to Fe3+ easily. Therefore, Cr2+ is a better reducing agent that Fe3+.
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
Both oxide and fluoride ions are highly electronegative and have a very small size. Due to these properties, they are able to oxidize the metal to its highest oxidation state.
Which is a stronger reducing agent Cr2+ or Fe2+ and why?
The following reactions are involved when Cr2+ and Fe2+ act as reducing agents.
Cr2+ Cr3+ Fe2+ Fe3+
The value is −0.41 V and is +0.77 V. This means that Cr2+ can be easily oxidized to Cr3+, but Fe2+ does not get oxidized to Fe3+ easily. Therefore, Cr2+ is a better reducing agent that Fe3+.
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