Advertisements
Advertisements
प्रश्न
Give reasons:
Transition metals show variable oxidation states.
Account for the following:
Transition metals show variable oxidation states.
Explain giving reasons:
Transition elements exhibit variable oxidation states.
Why do transition elements exhibit variable oxidation states?
Advertisements
उत्तर १
- The variable oxidation states of transition elements are due to the participation of ns and (n − 1) d-electrons in bonding.
- A lower oxidation state is exhibited when the ns-electrons take part in bonding.
- Higher oxidation states are exhibited when the (n − 1) d-electrons take part in bonding.
- Since there is very little energy difference between these orbitals, both energy levels can be used for bond formation.
Thus, transition elements exhibit variable oxidation states.
उत्तर २
- In transition elements, the 3d and 4s electrons are close in energy and can be lost in different numbers during reactions.
- The involvement of both (n − 1) d and ns electrons in bonding allows multiple oxidation states.
- Stability of oxidation states is influenced by half-filled or fully filled d-subshells, leading to preferred oxidation numbers.
- For example, manganese shows oxidation states from +2 to +7, reflecting this variability.
Hence, transition elements show a wide range of oxidation states because they can lose different numbers of d and s electrons easily.
APPEARS IN
संबंधित प्रश्न
Why do the transition elements have higher enthalpies of atomisation?
Write the factors which are related to the colour of transition metal ions.
Give reasons:
E° value for the Mn3+/Mn2+ couple is much more positive than that for Fe3+/Fe2+.
Give reasons: Sc3+ is colourless in aqueous solution whereas Ti3+ is coloured.
Two metallic elements A and B have the following standard oxidation potentials: A = 0·40v B = - 0·80v. What would you expect if element A was added to an aqueous salt solution of element B? Give a reason for your answer.
Maximum oxidation state is shown by ____________.
Transition elements form binary compounds with halogens. Which of the following elements will form \[\ce{MF3}\] type compounds?
(i) \[\ce{Cr}\]
(ii) \[\ce{Co}\]
(iii) \[\ce{Cu}\]
(iv) \[\ce{Ni}\]
On the basis of the figure given below, answer the following questions:
- Why Manganese has lower melting point than Chromium?
- Why do transition metals of 3d series have lower melting points as compared to 4d series?
- In the third transition series, identify and name the metal with the highest melting point.
A pair of coloured ions is ______.
Decide which of the following atomic numbers are the atomic numbers of the inner transition elements:
29, 59, 74, 95, 102, 104
