The reactivity of an element is very much related to its ionization enthalpy.
In general, ionization enthalpy increases from left to right across a period. Give the reason.

The reactivity of an element is very much related to its ionization enthalpy. Observe the following graph in which the first ionization enthalpies (DeltaH_1) of elements of the second period are plotted against their atomic numbers (Z): Identify the anomalour values and justify.

The reactivity of an element is very much related to its inoization enthalpy. Observe the following graph in wich the first ionozation enthalpies (delta_1H) of elements of the sercond period are ploptted agiains their atomic number (Z):

The first ionisation enthalpies of second period elements generally increase from left to right along the period. Give reason for this general trend.

Why does the first ionization enthalpy increase as we go from to across a given period of the Periodic Table?

Name of elements with atomic numbers greater than 100 are given by IUPAC the first inoisation enthalpies of second period element generally increase from lewft to right along the period. Give reason for this general trend.

A quantitative measure of the tendency of an element to lose electron is given by its ionisation enthalpy (I.E.). I.E. increases from left to right in a period of the periodic table. However, in second period, the I.E of oxygen is less than that of nitrogen. Why?

Which one of the following statements is incorrect in relation to ionization enthalpy? (1)Ionization enthalpy increases for each successive electron.(2)The greatest increase in ionization enthalpy is experienced on removal of electron from core noble gas configuration (3)End of valence electrons is marked by a big jump in ionization enthalpy (4)Removal of electron from orbitals bearing lower n value is higher than from orbital having higher 'n' value.

The electronegativity of elements from left to right in a period of periodic table.