Advertisements
Advertisements
Question
How is the variability in oxidation states of transition metals different from that of p-block elements?
Solution
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+.
RELATED QUESTIONS
Which metal in the first transition series (3d series) exhibits + 1 oxidation state most frequently and why?
Following are the transition metal ions of 3d series:
Ti4+, V2+, Mn3+, Cr3+
(Atomic numbers: Ti = 22, V = 23, Mn = 25, Cr = 24)
Answer the following:
1) Which ion is most stable in an aqueous solution and why?
2) Which ion is a strong oxidising agent and why?
3) Which ion is colourless and why?
Why is \[\ce{HCl}\] not used to make the medium acidic in oxidation reactions of \[\ce{KMnO4}\] in acidic medium?
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?
Mention the type of compounds formed when small atoms like H, C and N get trapped inside the crystal lattice of transition metals. Also give physical and chemical characteristics of these compounds.
A complex in which dsp2 hybridisation takes place is
Assertion (A): Transition metals have high enthalpy of atomisation.
Reason (R): Greater number of unpaired electrons in transition metals results in weak metallic bonding.
Write the ionic equation for reaction of KI with acidified KMnO4.
Describe the oxidising action of potassium dichromate and write the ionic equation for its reaction with iron (II) solution.
Decide which of the following atomic numbers are the atomic numbers of the inner transition elements:
29, 59, 74, 95, 102, 104
