Question

Define Ionisation energy, electron affinity, electronegativity?

Answer 1

Hint: 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 step by step 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 is periods ionization energy increase from left to right.
It can be expressed as follows:
$Y(g)+\text{energy}\to {{Y}^{+}}(g)+{{e}^{-}}$
Where, $Y$ is any Atom or molecule ${{Y}^{+}}$ is the ion with removal of one electron ${{e}^{-}}$ is an removed electron.
Electron affinity:
Nonmetals have more positive value of electron affinity $({{\text{E}}_{\text{ea}}})$ than metals.
Atoms whose anions are more stable. Then neutral atoms have greater the value of ${{\text{E}}_{\text{ea}}}$.
it is expressed by ${{\text{E}}_{g}}$]
$P(g)+{{e}^{-}}\to {{P}^{-}}(g)+\text{energy}$
Where, $P(o)=$ Atomic or molecule
$P(g)$ atom after gaining of an electron
The electron affinity is the property used only I gaseous state only
By above expression it is an exothermic reaction.
As we increase in row (Periods) then ${{\text{E}}_{\text{ea}}}$ increases it measured in kilo joule/mole.
${{\text{E}}_{\text{ea}}}=-\text{ }\!\!\Delta\!\!\text{ E(attach)}=\text{ }\!\!\Delta\!\!\text{ Edetach}$
Attachment (release)
Detachment (required)
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.

Note: 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:
$C < N < O < F$
Electronegativity increases in a period.