Ionisation Enthalpy

Ionisation enthalpies of Ce, Pr and Nd are higher than Th, Pa and U. Why?

The reducing nature of any metal in aqueous solution depends upon a.Enthalpy of atomisation b. Ionisation enthalpies c. Hydration energy

The reducing nature of any metal in aqueous solution depends upon a.Enthalpy of atomisation b. Ionisation enthalpies c. Hydration energy

Energy of an electron in the ground state of the hydrogen atom is -2.18xx10^(-18)J . Calculate the ionisation enthalpy of atomic hydrogen in terms of J mol^(-1) . Hint: Apply the idea of mole concept to derive the answer.

Why are the second ionisation enthalpies of group 1 elements much higher than their first ionisation enthalpies ?

The second ionisation enthalpies of elements are always higher than their first ionisation enthalpies because:

What is the order of successive ionisation enthalpies?

Match the correct ionisation enthalpies and electron gain enthalpies of the following elements.

Consider the following ionisation enthalpies of elements A and B: Which of the following statements is correct

The first ionisation enthalpies (in eV) of N & O are respectively given by: