Electron Affinity or Electron Gain Enthalpy || Factors Affecting( ΔeqH) || Trends in ΔeqH || Exception OF ΔeqH || Prediction OF sign OF ΔeqH and Ionisation Energy

Electron Gain Enthalph/Electron affinity - Definition/unit/Factors affecting EA || Trends and Exceptions || Applications

Revision|Electron Gain Enthalpy|Periodic Trend|OMR

The amount of energy released when an electron is added to an isolated gaseous atom to produce a monovalent anion is called electron affinity of first electron affinity or electron gain enthalpy. The first electron affinity is given a negative sign as the addition of an electron to a neutral atom is an exoergic process. The addition of electron to A^(-) requires energy to overcome the force of repulsion. Thus, the second electron affinity is an endoergic process. The magnitude of electron affinity depends on a number of factors such as (i) atomic size (ii) effective nuclear charge (iii) screening effects (iv) half and fully filled orbitals and (v) shape of orbital. In general, electron affinity increase as the atomic radii decrease in a period. However, there are exceptions when the atoms have stable configuration. In a group, electron affinity decreases as the size increases. However, the members of 3rd period have somewhat higher values than the members in the 2nd period of the same subgroups. Which of the following has least electron affinity?

The amount of energy released when an electron is added to an isolated gaseous atom to produce a monovalent anion is called electron affinity of first electron affinity or electron gain enthalpy. The first electron affinity is given a negative sign as the addition of an electron to a neutral atom is an exoergic process. The addition of electron to A^(-) requires energy to overcome the force of repulsion. Thus, the second electron affinity is an endoergic process. The magnitude of electron affinity depends on a number of factors such as (i) atomic size (ii) effective nuclear charge (iii) screening effects (iv) half and fully filled orbitals and (v) shape of orbital. In general, electron affinity increase as the atomic radii decrease in a period. However, there are exceptions when the atoms have stable configuration. In a group, electron affinity decreases as the size increases. However, the members of 3rd period have somewhat higher values than the members in the 2nd period of the same subgroups. Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative spin) of the given atomic species?

Ionisation Energy || Successive Ionisation Energy || Factors Affecting Ionisation Energy || Trends in Ionisation Energy

Exception OF Ionisation Energy - G-13/G-14 || d-block || Ionisation Energy OF Iso-electronic Species || Prediction OF Sign OF Ionisation Energy || Application OF Ionisation Energy (Important)

Variation Of Ionization Enthalpy In Period|Explanation|Variation Along Group|Variation Of I. E. Along Group 13|Electron Gain Enthalpy|Successive Electron Gain Enthalpy|Factors On Which The Electron Gain Enthalpy Depends|Variation Within A Group|Variation Along A Period |Difference Between Electron Gain Enthalpy & Electron Affinity|Significance Of Electron Gain Enthalpy|Electronegativity|Factors On Which Electronegativity Depends|Variation In Group And Period|Summary

Why is the second electron gain enthalpy negative (i.e. energy is absorbed)?

Discuss the factors affecting electron gain enthalpy and the trend in its variation in the periodic table.