321530
Why is oxygen superior to fluorine in stabilizing higher oxidation states of transition metals?
1 Because oxygen is less electronegative than fluorine
2 Because of larger size of oxygen as compared to fluorine
3 Because of the ability of oxygen to form multiple bonds with metals
4 Both (1) and (3)
Explanation:
Oxygen can form \({\rm{p}}\,{\rm{\pi }} - {\rm{d}}\,{\rm{\pi }}\) multiple bonds with transition metals, so it can form compounds with higher oxidation states of metals. This property is not shown by fluorine as it has only one unpaired electron in its valence shell.
CHXII08:THE D- & F-BLOCK ELEMENTS
321531
The oxidation state of iron in potassium ferrocyanide is ____.
321532
In chromyl chloride, the number of d-electrons present on chromium is same as in (Given At. No. of Ti : 22, V :23, Cr : 24, Mn : 25, Fe : 26)
1 V (IV)
2 Mn (VII)
3 Fe (III)
4 Ti (III)
Explanation:
Chromyl chloride is \(\mathrm{CrO}_{2} \mathrm{Cl}_{2}\) Oxidation state of \(\mathrm{Cr}=+6\) \(\mathrm{Cr}^{+6}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\) Similarly \(\mathrm{Mn}^{+7}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\)
JEE - 2023
CHXII08:THE D- & F-BLOCK ELEMENTS
321533
Assertion : \(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\) Reason : \(\mathrm{Fe}^{2+}\) ions are easily oxidised to \(\mathrm{Fe}^{3+}\) ions.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
\(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\). The electronic configuration of \(\mathrm{Fe}^{3+}\) has half- filled 'd 'orbitals and thus becomes more stable. \({ }_{26} \mathrm{Fe}^{2+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{6}\) \({ }_{26} \mathrm{Fe}^{3+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{5}\). \(\mathrm{Fe}^{2+}\) ions are easily oxidised to more stable \(\mathrm{Fe}^{3+}\). So option (2) is correct.
321530
Why is oxygen superior to fluorine in stabilizing higher oxidation states of transition metals?
1 Because oxygen is less electronegative than fluorine
2 Because of larger size of oxygen as compared to fluorine
3 Because of the ability of oxygen to form multiple bonds with metals
4 Both (1) and (3)
Explanation:
Oxygen can form \({\rm{p}}\,{\rm{\pi }} - {\rm{d}}\,{\rm{\pi }}\) multiple bonds with transition metals, so it can form compounds with higher oxidation states of metals. This property is not shown by fluorine as it has only one unpaired electron in its valence shell.
CHXII08:THE D- & F-BLOCK ELEMENTS
321531
The oxidation state of iron in potassium ferrocyanide is ____.
321532
In chromyl chloride, the number of d-electrons present on chromium is same as in (Given At. No. of Ti : 22, V :23, Cr : 24, Mn : 25, Fe : 26)
1 V (IV)
2 Mn (VII)
3 Fe (III)
4 Ti (III)
Explanation:
Chromyl chloride is \(\mathrm{CrO}_{2} \mathrm{Cl}_{2}\) Oxidation state of \(\mathrm{Cr}=+6\) \(\mathrm{Cr}^{+6}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\) Similarly \(\mathrm{Mn}^{+7}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\)
JEE - 2023
CHXII08:THE D- & F-BLOCK ELEMENTS
321533
Assertion : \(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\) Reason : \(\mathrm{Fe}^{2+}\) ions are easily oxidised to \(\mathrm{Fe}^{3+}\) ions.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
\(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\). The electronic configuration of \(\mathrm{Fe}^{3+}\) has half- filled 'd 'orbitals and thus becomes more stable. \({ }_{26} \mathrm{Fe}^{2+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{6}\) \({ }_{26} \mathrm{Fe}^{3+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{5}\). \(\mathrm{Fe}^{2+}\) ions are easily oxidised to more stable \(\mathrm{Fe}^{3+}\). So option (2) is correct.
321530
Why is oxygen superior to fluorine in stabilizing higher oxidation states of transition metals?
1 Because oxygen is less electronegative than fluorine
2 Because of larger size of oxygen as compared to fluorine
3 Because of the ability of oxygen to form multiple bonds with metals
4 Both (1) and (3)
Explanation:
Oxygen can form \({\rm{p}}\,{\rm{\pi }} - {\rm{d}}\,{\rm{\pi }}\) multiple bonds with transition metals, so it can form compounds with higher oxidation states of metals. This property is not shown by fluorine as it has only one unpaired electron in its valence shell.
CHXII08:THE D- & F-BLOCK ELEMENTS
321531
The oxidation state of iron in potassium ferrocyanide is ____.
321532
In chromyl chloride, the number of d-electrons present on chromium is same as in (Given At. No. of Ti : 22, V :23, Cr : 24, Mn : 25, Fe : 26)
1 V (IV)
2 Mn (VII)
3 Fe (III)
4 Ti (III)
Explanation:
Chromyl chloride is \(\mathrm{CrO}_{2} \mathrm{Cl}_{2}\) Oxidation state of \(\mathrm{Cr}=+6\) \(\mathrm{Cr}^{+6}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\) Similarly \(\mathrm{Mn}^{+7}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\)
JEE - 2023
CHXII08:THE D- & F-BLOCK ELEMENTS
321533
Assertion : \(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\) Reason : \(\mathrm{Fe}^{2+}\) ions are easily oxidised to \(\mathrm{Fe}^{3+}\) ions.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
\(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\). The electronic configuration of \(\mathrm{Fe}^{3+}\) has half- filled 'd 'orbitals and thus becomes more stable. \({ }_{26} \mathrm{Fe}^{2+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{6}\) \({ }_{26} \mathrm{Fe}^{3+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{5}\). \(\mathrm{Fe}^{2+}\) ions are easily oxidised to more stable \(\mathrm{Fe}^{3+}\). So option (2) is correct.
321530
Why is oxygen superior to fluorine in stabilizing higher oxidation states of transition metals?
1 Because oxygen is less electronegative than fluorine
2 Because of larger size of oxygen as compared to fluorine
3 Because of the ability of oxygen to form multiple bonds with metals
4 Both (1) and (3)
Explanation:
Oxygen can form \({\rm{p}}\,{\rm{\pi }} - {\rm{d}}\,{\rm{\pi }}\) multiple bonds with transition metals, so it can form compounds with higher oxidation states of metals. This property is not shown by fluorine as it has only one unpaired electron in its valence shell.
CHXII08:THE D- & F-BLOCK ELEMENTS
321531
The oxidation state of iron in potassium ferrocyanide is ____.
321532
In chromyl chloride, the number of d-electrons present on chromium is same as in (Given At. No. of Ti : 22, V :23, Cr : 24, Mn : 25, Fe : 26)
1 V (IV)
2 Mn (VII)
3 Fe (III)
4 Ti (III)
Explanation:
Chromyl chloride is \(\mathrm{CrO}_{2} \mathrm{Cl}_{2}\) Oxidation state of \(\mathrm{Cr}=+6\) \(\mathrm{Cr}^{+6}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\) Similarly \(\mathrm{Mn}^{+7}=[\mathrm{Ar}] 3 \mathrm{~d}^{0}\)
JEE - 2023
CHXII08:THE D- & F-BLOCK ELEMENTS
321533
Assertion : \(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\) Reason : \(\mathrm{Fe}^{2+}\) ions are easily oxidised to \(\mathrm{Fe}^{3+}\) ions.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
\(\mathrm{Fe}^{3+}\) is more stable than \(\mathrm{Fe}^{2+}\). The electronic configuration of \(\mathrm{Fe}^{3+}\) has half- filled 'd 'orbitals and thus becomes more stable. \({ }_{26} \mathrm{Fe}^{2+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{6}\) \({ }_{26} \mathrm{Fe}^{3+}: 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 3 \mathrm{~d}^{5}\). \(\mathrm{Fe}^{2+}\) ions are easily oxidised to more stable \(\mathrm{Fe}^{3+}\). So option (2) is correct.
