Compare the chemistry of actinoids with that of the lanthanoids with special reference to: (iv) chemical reactivity.

Compare the chemistry of actinoids with that of the lanthanoids with special reference to: (iii) oxidation state

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.

What are the characteristics of the transition elements and why are they called transition elements? Which of the d-block elements may not be regarded as the transition elements?

In what way is the electronic configuration of the transition elements different from that of the non transition elements?

Which is the last element in the series of the actinoids? Write the electronic configuration of this element. Comment on the possible oxidation state of this element.

What may be the stable oxidation state of the transition element with the following d electron configurations in the ground state of their atoms : \(3d^{3}\), \(3d^{5}\), \(3d^{8}\) and \(3d^{4}\)?

Write the electronic configurations of the elements with the atomic numbers 61, 91, 101, and 109.

What are the different oxidation states exhibited by the lanthanoids?

Write down the electronic configuration of: (ii) \(Pm^{3+}\)

Calculate the number of unpaired electrons in the following gaseous ions: \(Mn^{3+}\), \(Cr^{3+}\), \(V^{3+}\) and \(Ti^{3+}\). Which one of these is the most stable in aqueous solution?

Explain giving reasons: (i) Transition metals and many of their compounds show paramagnetic behaviour.

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 points: (i) electronic configurations

Name the oxometal anions of the first series of the transition metals in which the metal exhibits the oxidation state equal to its group number.

Write down the electronic configuration of: (i) \(Cr^{3+}\)

Which metal in the first series of transition metals exhibits +1 oxidation state most frequently and why?

Write down the electronic configuration of: (iv) \(Ce^{4+}\)

For \(M^{2+}/M\) and \(M^{3+}/M^{2+}\) systems the \(E^{o}\) values for some metals are as follows: 

(i) the stability of \(Fe^{3+}\) in acid solution as compared to that of \(Cr^{3+}\) or \(Mn^{3+}\)

How would you account for the following: (iii) The \(d^{1}\) configuration is very unstable in ions.

For \(M^{2+}/M\) and \(M^{3+}/M^{2+}\) systems the \(E^{o}\) values for some metals are as follows:

Use this data to comment upon: (ii) the ease with which iron can be oxidised as compared to a similar process for either chromium or manganese metal.