Advertisements
Advertisements
प्रश्न
Explain briefly how +2 states become more and more stable in the first half of the first-row transition elements with increasing atomic numbers.
Advertisements
उत्तर
In the elements of the first half of the first row, with the removal of valance 4s electrons (+2 oxidation state) the 3d orbital gets gradually occupied. Since the number of empty d orbital decreases, the stability of the cations (M2+) increases from Sc2+ to Mn2+.
APPEARS IN
संबंधित प्रश्न
The magnetic moment of Mn2+ ion is ____________.
The correct order of increasing oxidizing power in the series
What are transition metals? Give four examples.
Complete the following.
\[\ce{MnO^2-_4 + H^+ ->?}\]
What are interstitial compounds?
Calculate the number of unpaired electrons in Ti3+, Mn2+ and calculate the spin only magnetic moment.
Explain the variation in `"E"_ ("M"^(3+)//"M"^(2+))^0` 3d series.
Compare the ionization enthalpies of the first series of the transition elements.
Why first ionization enthalpy of chromium is lower than that of zinc?
Transition metals show high melting points why?
