Question

define ionization enthalpy .how does the successive ionization enthalpies change for an atom explain?​

Answer 1

Explanation:

In physics and chemistry, ionization energy or ionisation energy is the minimum amount of energy required to remove the most loosely bound electron of an isolated neutral gaseous atom or molecule.

The amounts of enthalpies required to remove first, second and subsequent electrons from the gaseous atom one after the other are collectively called successive ionisation enthalpies. IE3 > IE2 > IE1. Second ionisation enthalpy is always greater than the first ionisation enthalpy.

Answer 2

Explanation:

Ionisation energy is the energy required to remove an electron from the outermost shell of an isolated gaseous atom. When the first electron or the most loosely bound electron is removed, the amount of energy required is less than the energy required to remove the electron in the next successive shell. This ionisation energy goes on increasing with the number of electrons removed.

So the number of electrons removed from the successive no of shells and the energy involved is called successive ionization energy.

The amounts of energies required to remove 2nd, 3rd ,4th… electron from cations after removal of 1st electron are successive ionization energies.

The ionization energy order is

I.E1<I.E2<I.E3<I.E4…

In general successive ioniZation energies always increase as the electrons to be removed get closer to the nucleus, there is a strong attraction between nucleus and electron, therefore more energy is required to remove the next electron.