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प्रश्न
Comment on the statement that elements of the first transition series possess many properties different from those of heavier transition elements.
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उत्तर १
- In the first transition series, lower oxidation states are more stable, while heavier transition elements have higher oxidation states.
- The 5d transition series exhibits higher ionization enthalpy compared to the 3d and 4d transition series.
- M-M bonding is prevalent in heavier transition metals, but less so in the first series.
- The elements in the first transition series do not form complexes with coordination numbers of 7 or 8.
- Elements in the first series can form high or low-spin complexes based on ligand strength, while those in the other series form low-spin complexes regardless of ligand strength.
उत्तर २
This statement is true. According to the heavier transition elements (elements of the second and third transition series), the elements of the first transition series have different atomic radii, melting and boiling temperatures, ionization enthalpies, atomization enthalpies, and other characteristics. Their mentioned characteristics have significantly lower values.
संबंधित प्रश्न
What are interstitial compounds?
Which metal in the first transition series (3d series) exhibits + 1 oxidation state most frequently and why?
Why is the highest oxidation state of a metal exhibited in its oxide or fluoride only?
To what extent do the electronic configurations decide the stability of oxidation states in the first series of the transition elements? Illustrate your answer with examples.
How would you account for the following:
The d1 configuration is very unstable in ions.
Give reasons: Sc3+ is colourless in aqueous solution whereas Ti3+ is coloured.
The transition metals show _________ character because of the presence of unpaired· electrons and Cu+ is ____________ because of its electronic configuration is [Ar]3d10
Account for the following :
Ti4+ is colourless whereas V4+ is coloured in an aqueous solutions.
Transition elements show high melting points. Why?
The halides of transition elements become more covalent with increasing oxidation state of the metal. Why?
Identify the metal and justify your answer.
Carbonyl \[\ce{M(CO)5}\]
Account for the following:
In case of transition elements, ions of the same charge in a given series show progressive decrease in radius with increasing atomic number.
A metallic ion 'M' reacts with chloride ion to form white precipitate which is readily soluble in aqueous ammonia. Identify 'M'?
Mercury is the only metal liquid at room temperature due to its:-
Passing H2S gas into a mixture of Mn2+ and Ni2+, Cu2+, ions in an acidified aqueous solution precipitates.
How is the variability in oxidation states of transition metals different from that of p-block elements?
The disproportionation of \[\ce{MnO^{2-}_4}\] in acidic medium resulted in the formation of two manganese compounds A and B. If the oxidation state of Mn in B is smaller than that of A, then the spin-only magnetic moment (µ) value of B in BM is ______. (Nearest integer)
Which of the following ions has the electronic configuration 3d6?
(Atomic number: Mn = 25, Co = 27, Ni = 28)
Describe the oxidising action of potassium dichromate and write the ionic equation for its reaction with iron (II) solution.
Describe the oxidising action of potassium dichromate and write the ionic equation for its reaction with H2S.
