How does the ionisation enthalpy vary from left to right in the transition series ?

The periodicity is related to the electronic configuration that is all chemical and physical properties are a manifestation of the electronic configuration of the elements.the atomic and ionic radii genreally decrease in a period from left to right as a consequence the ionization enthalpies genrally increase and electron gain enthalpies become more negative across a period in other words the ionization enthalpy of the extreme left element element in a period is the least and the electron gain enthalpy of the element on the extreme right is the highest negative.this results into highly chemical reactivity at the two extremes and the lowest in the centre similarly down the group the increase in atomic and ionic radii result in gradual decrease in ionization enthalpies and a regular decrease (with exception in some third period elements)in electron gain enthalpies in the csea of main group elements. reducing and oxidizing behaviour of the elements metallic and non metallic character of elements acidic,basic,amphoteric and neutral charcter of the oxides of the elements The correct order of the metallic character is

Define Ionisation potential. How it changes form left,to right in 2nd period?

How is the variability in oxidation states of transition metals different from that of the non - transition metals ? Illustrate with examples.

What are transition elements? How many transition elements are present in the first transition series?

How much enerrgy is needed to ionise a H-atom if the electron occupies n=5 orbit? Compare your answer with the ionisation enthalpy of H-atom (energy required to remove the electron from n=1 orbit).

Why does Mn^(2+) exhibit the highest paramagnetism among the bivalent ions of the first transition series ?