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Electron gain enthalpy usually becomes ...

Electron gain enthalpy usually becomes less negative from top to bottom in a group. Is there any exception to this generalization ? Comment.

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### Step-by-Step Solution: 1. **Understanding Electron Gain Enthalpy**: - Electron gain enthalpy is defined as the amount of energy released when an electron is added to a neutral gaseous atom. It is usually expressed in kilojoules per mole (kJ/mol). A more negative value indicates that more energy is released when an electron is added. 2. **General Trend in Groups**: - As we move down a group in the periodic table, the size of the atoms increases due to the addition of electron shells. This generally leads to a decrease in the attraction between the nucleus and the added electron, resulting in less negative electron gain enthalpy. ...
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Electron gain enthalpies of halogens are largely negative. Explain.

" The electron gain enthalpy of "O" is less negative than that of "S" ."

Knowledge Check

  • In going down from top to bottom in Group 16.

    A
    Stability of +6 oxidation state decreases and that of +4 increases.
    B
    Stability of both +6 and +4 oxidation state increases.
    C
    Stability of both +6 and +4 oxidation state decreases.
    D
    Stability of +6 oxidation state increases and that of +4 decreases.

  • Assertion :- Electron gain enthalpy strictly becomes less negative on moving down the group. Reason :- Size increases and addition of extra electron is close to nucleas on moving down the group.

    A
    If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
    B
    If both Assertion & Reason are True but Reason is not a correct explanation of the Assertiion.
    C
    If Assertion is True but the Reason is False.
    D
    If both Assertion & Reason are False

  • There are certain properties of the elements which vary (increase or decrease) gradually in the same period or group with increase in atomic number. These properties of elements which show a regular gradation on moving from left to right in a period or from top to bottom in a group are called periodic properties. The recurrence of similar properties of elements after certain regular intervals when they are arranged in the increasing order of their atomic numbers is called periodicity valency, atomic/ Some of the properties such as ionic size, ionization enthalpies, electro-negativity, electron gain enthalpy, oxidizing/educing power, acid/base character etc. are directly related to the electronic configuration of the elements. On the other hand, there are some properties such as etc. which are indirectly related to the electronic configuration of the elements. The cause of repetition of similar electronic configuration of their atoms in valence shells after regular intervals melting points, density Down the group, the atomic/ionic radii, metallic character and valencing character increase whereas ionisation enthalpy and electronegativity decrease. Across a right, period from left to atomic/ionic radii and metallic character decrease whereas ionization enthalpy, electronegativity, non-metallic character and oxidizing power increase. In general, electron gain enthalpy decreases i.e., becomes less negative bottom in a group. Across a period from left to right there is an over all increase in the electron gain enthalpies (i.e., it becomes more negative). However most gases have positive electron gain enthalpies which do not show any regular trend. Which of the following has the highest electron gain enthalpy?

    A
    `Li^(+)`
    B
    `Na^(+)`
    C
    `F^(-)`
    D
    `Cl^(-)`

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    Electron gain enthalpy of fluorine (F) is less negative than that of chlorine (Cl). Why ?

    The tendency to gain electron _____ on going from top to bottom in a group of the periodic table.

    Electron gain enthalpy of fluorine is less than that of chlorine. Why?

    Assertion: Electron gain enthalpy always becomes less negative as we go down a group in Modern periodic table. Reason: The size of the atom increase on going down the group in Modern periodic table and the added electron would be farther from the nucleus.

    Assertion (A) : Electron gain enthapy becomes less negative as we go down a group. Reason ( R) : Size of the atom increases on goin down in the group in the added electron would be farther from the nucleus.

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