321543
Electronic configuration of a transition element \(\mathrm{\mathrm{X}}\) in +3 oxidation state is \({\rm{[Ar]3}}{{\rm{d}}^{\rm{5}}}\). What is its atomic number?
321545
For the four successive transition elements \(\mathrm{(\mathrm{Cr}}\), \(\mathrm{\mathrm{Mn}, \mathrm{Fe}}\) and \(\mathrm{\mathrm{Co}}\) ), the stability of +2 oxidation state will be there in which of the following order?
\(\mathrm{\mathrm{Mn}^{2+}\left(d^{5}\right)}\) gets higest stabilisation due to halffilled configuration. In case of \(\mathrm{\mathrm{Fe}^{2+}\left(\mathrm{d}^{6}\right)}\), addition of one extra electron in the subshell destabilises it. Addition of two electrons in case of \(\mathrm{\mathrm{Co}^{2+}\left(d^{7}\right)}\) destabilises it more. \(\mathrm{\mathrm{Cr}^{2+}\left(d^{4}\right)}\) has one vacant subshell. \(\mathrm{\mathrm{Fe}^{2+}}\) gets more stabilisation as compared to \(\mathrm{\mathrm{Cr}}\) through exchange energy. So correct order is \(\mathrm{\mathrm{Mn}>\mathrm{Fe}>\mathrm{Cr}>\mathrm{Co}}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321546
Most common oxidation states are matched below with the elements. Which one is mismatched?
NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXII08:THE D- & F-BLOCK ELEMENTS
321543
Electronic configuration of a transition element \(\mathrm{\mathrm{X}}\) in +3 oxidation state is \({\rm{[Ar]3}}{{\rm{d}}^{\rm{5}}}\). What is its atomic number?
321545
For the four successive transition elements \(\mathrm{(\mathrm{Cr}}\), \(\mathrm{\mathrm{Mn}, \mathrm{Fe}}\) and \(\mathrm{\mathrm{Co}}\) ), the stability of +2 oxidation state will be there in which of the following order?
\(\mathrm{\mathrm{Mn}^{2+}\left(d^{5}\right)}\) gets higest stabilisation due to halffilled configuration. In case of \(\mathrm{\mathrm{Fe}^{2+}\left(\mathrm{d}^{6}\right)}\), addition of one extra electron in the subshell destabilises it. Addition of two electrons in case of \(\mathrm{\mathrm{Co}^{2+}\left(d^{7}\right)}\) destabilises it more. \(\mathrm{\mathrm{Cr}^{2+}\left(d^{4}\right)}\) has one vacant subshell. \(\mathrm{\mathrm{Fe}^{2+}}\) gets more stabilisation as compared to \(\mathrm{\mathrm{Cr}}\) through exchange energy. So correct order is \(\mathrm{\mathrm{Mn}>\mathrm{Fe}>\mathrm{Cr}>\mathrm{Co}}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321546
Most common oxidation states are matched below with the elements. Which one is mismatched?
321543
Electronic configuration of a transition element \(\mathrm{\mathrm{X}}\) in +3 oxidation state is \({\rm{[Ar]3}}{{\rm{d}}^{\rm{5}}}\). What is its atomic number?
321545
For the four successive transition elements \(\mathrm{(\mathrm{Cr}}\), \(\mathrm{\mathrm{Mn}, \mathrm{Fe}}\) and \(\mathrm{\mathrm{Co}}\) ), the stability of +2 oxidation state will be there in which of the following order?
\(\mathrm{\mathrm{Mn}^{2+}\left(d^{5}\right)}\) gets higest stabilisation due to halffilled configuration. In case of \(\mathrm{\mathrm{Fe}^{2+}\left(\mathrm{d}^{6}\right)}\), addition of one extra electron in the subshell destabilises it. Addition of two electrons in case of \(\mathrm{\mathrm{Co}^{2+}\left(d^{7}\right)}\) destabilises it more. \(\mathrm{\mathrm{Cr}^{2+}\left(d^{4}\right)}\) has one vacant subshell. \(\mathrm{\mathrm{Fe}^{2+}}\) gets more stabilisation as compared to \(\mathrm{\mathrm{Cr}}\) through exchange energy. So correct order is \(\mathrm{\mathrm{Mn}>\mathrm{Fe}>\mathrm{Cr}>\mathrm{Co}}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321546
Most common oxidation states are matched below with the elements. Which one is mismatched?
321543
Electronic configuration of a transition element \(\mathrm{\mathrm{X}}\) in +3 oxidation state is \({\rm{[Ar]3}}{{\rm{d}}^{\rm{5}}}\). What is its atomic number?
321545
For the four successive transition elements \(\mathrm{(\mathrm{Cr}}\), \(\mathrm{\mathrm{Mn}, \mathrm{Fe}}\) and \(\mathrm{\mathrm{Co}}\) ), the stability of +2 oxidation state will be there in which of the following order?
\(\mathrm{\mathrm{Mn}^{2+}\left(d^{5}\right)}\) gets higest stabilisation due to halffilled configuration. In case of \(\mathrm{\mathrm{Fe}^{2+}\left(\mathrm{d}^{6}\right)}\), addition of one extra electron in the subshell destabilises it. Addition of two electrons in case of \(\mathrm{\mathrm{Co}^{2+}\left(d^{7}\right)}\) destabilises it more. \(\mathrm{\mathrm{Cr}^{2+}\left(d^{4}\right)}\) has one vacant subshell. \(\mathrm{\mathrm{Fe}^{2+}}\) gets more stabilisation as compared to \(\mathrm{\mathrm{Cr}}\) through exchange energy. So correct order is \(\mathrm{\mathrm{Mn}>\mathrm{Fe}>\mathrm{Cr}>\mathrm{Co}}\).
CHXII08:THE D- & F-BLOCK ELEMENTS
321546
Most common oxidation states are matched below with the elements. Which one is mismatched?