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प्रश्न
How is the variability in oxidation states of transition metals different from that of p-block elements?
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उत्तर
In transition elements, the variability in the oxidation state is due to the participation of (n – 1)d orbitals and ns orbitals. Thus, oxidation states differ by unity. For example, Fe3+ to Fe2+, Cr3+ to Cr2+ etc.
On the other hand, the variable oxidation states shown by some p-block elements differ by two units. For example, Sn4+ to Sn2+, Pb4+ to Pb2+.
संबंधित प्रश्न
Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number?
Calculate the number of unpaired electrons in the following gaseous ions:
Mn3+, Cr3+, V3+ and Ti3+. Which one of these is the most stable in an aqueous solution?
Explain why transition metals and their compounds act as a catalyst.
Transition metals with lowest melting point is ______.
While filling up of electrons in the atomic orbitals, the 4s orbital is filled before the 3d orbital but reverse happens during the ionisation of the atom. Explain why?
Match the properties given in Column I with the metals given in Column II.
| Column I (Property) | Column II (Metal) | |
| (i) | Element with highest second ionisation enthalpy |
(a) \[\ce{Co}\] |
| (ii) | Element with highest third ionisation enthalpy |
(b) \[\ce{Cr}\] |
| (iii) | \[\ce{M}\] in \[\ce{M(CO)6}\] is | (c) \[\ce{Cu}\] |
| (iv) | Element with highest heat of atomisation |
(d) \[\ce{Zn}\] |
| (e) \[\ce{Ni}\] |
Give reasons for the following statement:
Transition metals and most of their compounds show paramagnetic behaviour.
The second ionization enthalpies of chromium and manganese are 1592 and 1509 kJ/mol respectively. Explain the lower value of Mn.
Give two similarities in the properties of Sc and Zn.
Compare the general characteristics of the first series of the transition metals with those of the second and third series metals in the respective vertical columns. Give special emphasis on the following point:
Atomic sizes
