Removal of electron becomes easier on moving down the group.
a) Comment the above statement based on ionization enthalpy.
b) How electronic configuration influences the ionization enthalpy value?

"Removal of electron becomes easier on moving down the group". Comment on the statement based on ionisation enthalpy.

"Removal of electron becomes easier on moving down the group". What is the relevance of half-filled and fully filled sub-levels in I.E determination?

Ionisation is the removal of electron from an.atom. What is ionisation enthalpy? How is it related to electronic configuration of atoms.

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.

a) On moving down a group what happens to electron gain enthalpy? b) Why chlorine shows more negative electron gain enthalpy than fluorine?

The energy released during the addition of an electron to an isolated neutral atom is called electron gain enthalpy. a) Explain how electron gain enthalpy differ from electronegativity. b) The second ionisation enthalpy of an element is always greater than the first ionisation enthalpy. Give reason.

What is the significance of the terms - isolated gaseous atom and ground state while defining the ionization enthalpy and electron gain enthalpy?

Assertion: Of all the elements, helium has the highest value of first ionization enthalpy. Reason: Helium has the most positive electron gain enthalpy of all the elements.

Atoms possessing stable configuration have less tendency to loss and consequently will have high value of ionization enthalpy. a) Justify this statement by taking the case of halffilled and completely filled configurations. b) The noble gases have highest ionization enthalpies in each respective periods. Why?