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

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.

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.

Account for the following: Atomic radius decreases from left to right in a period

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?

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

Give justification, The first lonisation enthalpy of carbon is greater than that of boron, whereas the reverse is correct for the second ionisation enthalpy.

Basicity of hydroxides of lanthanoids decreases along the period from left to right. Explain the reason.

Considering the elements from left to right in the third period of the periodic table, the atomic volume of the elements: