Periodic Trends In Physical Properties|Screening Effect / Shielding Effect |Factors Which Influence I.E|Successive Ionisation Energies|Factors Affecting The Magnitude Of Electron Affinity|OMR

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

Application OF I.E || Inert Pair Effect || Electron Gain Elthalpy || Electron Affinity

d - Block Elements|Lanthanide Contraction|Ionic Radius|Comparion Of Ionic Radii With Atomic Radii|Variation Of Ionic Size Among Isoelectronic Ions|Ionization Enthalpy|Successive Ionization Enthalpies|Factors Affecting Ionization Enthalpy|Nuclear Charge|Atomic Size|Penetration Effect Of The Electrons|Questions|Shielding Or Screening Effect Of The Inner Shell Electrons|Electronic Configuration|Variation Of Ionization Enthalpy In Period|Explanation|Variation Along Group

Periodic Properties || Effective Nuclear Charge || Screening or Shielding Effect || Calculation OF Slater Constant || Variation OF Zeff along Group and Period

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

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. The electron affinities of halogens are: F =- 332, CI =- 349, Br =- 324,I =- 295 kJ mol^(-1) The higher value of CI as compared to that of F^(-) is due to:

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 species has the highest 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?