Question

How do ionisation energy and electron affinity determine whether atoms of elements will combine to form ionic compounds?

Answer 1

We know that the ionization energy is the minimum amount of energy required to remove the most slowly bound electro of any molecules and the amount of energy released when an electron is attracted to a neutral atom or molecule is known as electron affinity.

Complete answer:
Ionisation energy: It is generally an endothermic process. As we have general study that as for the electron from the Nucleus of the atom, tower the ionization energy. The unit of Ionisation energy is electron volts are period’s ionization energy increase from left to right. It can be expressed as follows: ${{Y}_{\left( g \right)}}+energy\to Y_{\left( g \right)}^{+}+{{e}^{-}}$
Electrons Negativity It is the toudinery of an atom to attract a shared put of electron or density. Electronegativity is determined by to can like, the nuclear charge, the opposite of electronegativity is electropositivity it is the ability of accept the electron it is depends upon the bond energy it is an transferable property it is expressed in electron votes As we go in periods form left to region the electronegativity increase Nitrogen, Oxygen and halogens all more electronegative than carbon Electronegativity of Hydrogen is similar to carbon.
We can define ionisation energy as the energy which is needed for the removal of one mole of electrons from one mole of isolated gaseous atom. Electron affinity is the energy liberated for that process. So the formation of ionic compounds depends on whether it loses electrons easily and forms a bond with the other atom.
Thus, a low first ionisation energy means that very little energy is required to remove that electron from the atom, and so means that the atom forms its $1+~$ cation quite readily. A high electron affinity, where "high" refers only to the magnitude of the number, and not its sign, means that the atom is more inclined to take in an electron to become a $1-~anion.$
Thus, it is now easy to see how ionisation energy and electron affinity affect the likelihood of ionic bonding taking place, by having an impact on the tendency of cation and anion formation.

Note:
Note that simply, the elements which have atomic number less have high ionization energy and which are at the bottom have decrease in ionization energy. When we increase in row then electron affinity also increases. More electronegative element bears a negative charge more easily, giving a more stable conjugate base and a stronger acid.