To what extent do the electronic configuration decide the stability of oxidation states first series of the transition elements? justify your answer with examples."

Compare the stability of +2 oxidation state for the elements of the first transition series.

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

In the first transition series, the highest oxidation state is exhibited by:

Transition elements show variable oxidation state. a) Do you agree with, this statement? b) Illustrate with an example

In the first row transition metals, the element that exhibits only +3 oxidation state is

Would you expect the second electron gain enthalpy O as positive, more negative or less negative than the first ? Justify your answer.

The atomic number of an element is 19. a. Write the subshell electronic configuration. b. Find the group, period and oxidation state of this element. c. Write any pecularity of the block in which this element belongs to?

Transition metals show variable oxidation states due to tendency of ‘d’ as well as ‘s’ electrons to take part In bond formation:- Which element in the first series of transition elements does not exhibit variable oxidation states and why?

Two compounds of iron are given. FeSo_4, Fe_2(SO_4)_3 (The oxidation state of SO_4 -2 ) a. Identify the compound in which iron shows +2 oxidation state. b. Which of these compound posses Fe^3+ ions. c. write the subshell electronic configuration of Fe^3+ ions d. Give reason for the various oxidation states of transition elements.