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During a group discussion a student argu...

During a group discussion a student argued that ionization enthalpy depends only upon electronic configuration.
a) Do you agree? Comment.
b) Define shielding effect/screening effect.
c) Is there any relation between ionization enthalpy and shielding effect/screening effect? Explain

Answer

Step by step text solution for During a group discussion a student argued that ionization enthalpy depends only upon electronic configuration. a) Do you agree? Comment. b) Define shielding effect/screening effect. c) Is there any relation between ionization enthalpy and shielding effect/screening effect? Explain by CHEMISTRY experts to help you in doubts & scoring excellent marks in Class 11 exams.

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During a group discussion a student argues that both oxidation state and valence are the same. a) Do you agree? b) Justify taking the case of [AICI(H_2O)_5]^2+

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Knowledge Check

  • The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. Which one of the following statements is incorrect in relation to ionisation enthalpy?

    A
    Ionization enthalpy increases for removal of successive electrons.
    B
    The greatest increase in ionization enthalpy is experienced on removal of electron from core of noble gas configuration.
    C
    End of valence electrons is marked by a big jump in ionization enthalpy.
    D
    Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value.

  • The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. The first ionization energy of Na, Mg, Al and Si are in the order of:

    A
    `Na lt Al lt Mg lt Si`
    B
    `Na gt Mg gt Al gt Si`
    C
    `Na lt Mg lt Al gt Si`
    D
    `Na gt Mg gt Al lt Si`

  • The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. Considering the elements F, Cl, O and S, the correct order of their electron affinity values is:

    A
    `F gt Cl gt O gt S`
    B
    `F gt O gt Cl gt S`
    C
    `Cl gt F gt S gt O`
    D
    `O gt F gt S gt Cl`

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    The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. Identify the least stable ion amongst the following:

    Paragraph Carboxylic acids are distinctly acidic because they ionize in water to give hydronium ions: RCOOH+H_(2)O hArr RCOO^(-) +H_(3)O^(+) The acidic strength depends upon the extent of ionizations of the acid and the stability of the anion formed. The acidic strength can also be expressed in terms of dissociation constant K_(a) or pK_(a) which are related as pK_(a)= -log K_(a) . Most unsubstituted carboxylic acids have K_(a) values in the range of 10^(-4) to 10^(-5) (pK_(a) =4-5) . The substitutents have marked effect on the acidic strength of carboxylic acids. Any group that stabilizes the carboxylate ion more than the carboxylic acid group will increase the acidic strength, and the group which destabilizes the carboxylate group more than the carboxylic acid group will decrease the acidic strength. In a similar manner, the electron-releasing groups makes benzoic acid weaker, while the electron-withdrawing groups make benzoic acid stronger. The ortho isomer of every substituted benzoic acid (whether electron releasing or electron withdrawing) is the strongest among the three isomers due to ortho effect. Which of the following is the weakest acid?

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