Question

If the ionization potential is IP, the electron affinity is EA and electro-negativity is x then which of the following relations is correct?
A.${\text{2X - IP - EA = 0}}$
B.${\text{2EA - X - IP = 0}}$
C.${\text{2IP - X - EA = 0}}$
D.All of the above

Answer 1

The magnitude of electro-negativity depends upon its ionization potential and electron affinity. Higher ionization potential and high electron affinity of an element indicates higher electronegative value of that element.

Complete step by step answer:
Electron Affinity-Electron affinity is the amount of energy emitted when, in its lower energy level, an electron is attached to the outermost shell of one mole of an isolated gaseous atom. When an electron is added to the element's outermost shell, negative ions are produced.
Ionization Potential- Ionization potential is the minimum energy needed from an isolated gaseous atom the loosely retained outermost shell electron in the ground state.
Electro-negativity- The atoms' attraction towards their own electrons and other electrons is electro-negativity. According to Mulliken, electro-negativity can be expressed as the average of ionization energy and electron affinity of an atom. If the ionization potential is IP, the electron affinity is EA and electro-negativity is x then we can write the relation between them as-
$\Rightarrow X = \dfrac{{IP + EA}}{2}$
On simplifying we get-
$\Rightarrow 2X = IP + EA$
On transferring the terms IP and EA on the left side, we get-
$\Rightarrow$ ${\text{2X - IP - EA = 0}}$

The correct answer is option A.

Note:
-Electron affinity is also called electron gain enthalpy as it is the measure of the ease with which an atom accepts an electron to form an anion.
-It can be endothermic or exothermic.
- If an atom is added and energy is released then the electron gain enthalpy is negative.
- If energy is needed to add an electron then it is positive.