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Classification of Elements and Periodicity in Properties Test - 35

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Classification of Elements and Periodicity in Properties Test - 35
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  • Question 1
    1 / -0
    Which of the following element is expected to have highest electron gain enthalpy :
    Solution
    The element with electron configuration 1s22s22p63s23p51s^22s^22p^63s^23p^5 is expected to have highest electron gain enthalpy. On moving down the group, the electron gain enthalpy decreases. However in general, the electron gain enthalpies of some third period elements are more negative than the corresponding second period elements. Also when on addition of an electron, stable inert gas configuration is obtained, the electron gain enthalpy has high value.
  • Question 2
    1 / -0
    Which one the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of given atomic species ?
    Solution
    The correct order of electron gain enthalpy (with negative sign) of given atomic species is O<S<F<Cl\displaystyle O<S<F<Cl

    In a period, on moving from left to right, electron affinity increases due to increase in the effective nuclear charge and decrease in size.

    In a group on moving from top to bottom, the electron affinity decreases due to decrease in the effective nuclear charge and increase in size. But there is an exception for FF and OO due to its small size.
  • Question 3
    1 / -0
    Which statement is correct?
    Solution
    The electron affinity of bromine (324.2kJ/mol)(-324.2 \: kJ/mol) is less than the electron affinity of chlorine (348.3kJ/mol)(-348.3 \: kJ/mol).

    On moving from chlorine to bromine to iodine, the electron affinity decreases (becomes less negative). This is because the increase in atomic size decrease the effective nuclear charge. Hence, the additional electron feels less attraction by the large atom.
  • Question 4
    1 / -0
    Fluorine has low electron affinity than chlorine because of :
    Solution
    Fluorine has low electron affinity than chlorine because of smaller radius of fluorine, high charge density.
    There are strong interelectronic repulsions in the relatively compact 2p subshell of fluorine. Hence, the incoming electron does not feel much attraction.
  • Question 5
    1 / -0
    Electron gain enthalpy is positive when:
    Solution
    O(g)+e(g)EndothermicO2(g);ΔegHO^-(g)+e^-(g) \overset{Endothermic}{\rightarrow}O^{2-}(g);\Delta _{eg}H^{\circleddash} =744kJmol1.= 744 kJ mol^{-1}.

    Due to electrostatic repulsion on account of the same charge.

    Hence, the correct option is B\text{B}
  • Question 6
    1 / -0
    The standard emf for the cell reaction,

    2Cu+(aq)Cu(s)+Cu2+(aq)2Cu^+ (aq) \rightarrow Cu(s) + Cu^{2+} (aq)

    is + 0.36 V at 298 K. The equilibrium constant of the reaction is
    Solution

  • Question 7
    1 / -0
    Number of electrons present in 26Fe^{26} Fe is ___________.
    Solution
    Number of electron present in the Fe26Fe^{26} is 26 because its atomic number is 26 which represent no. of electrons or protrons. Option 'A' is correct.
  • Question 8
    1 / -0
    For electron affinity of halogens, which of the following is correct ?
    Solution
    Hint:\bf{Hint:} The amount of energy released or accepted when an electron is added to an isolated atom is known as electron affinity.

    Explanation:\bf{Explanation:}

    The electron affinity value depends on the following two factors:

    1. The size of an atom.
    2. Electronegativity of atom


    Generally, electron affinity decreases down the group as the size of the atom increases downwards and also electronegativity also decreases as we go down the group.
    As the electrons are far away from the nucleus so as we go down the group there is less affinity for the electrons.
    But there is an exceptional trend in the electron affinities of FF and ClCl. ClCl has more electron affinity than FF because in the case of FF as it is smaller in size there is more repulsion between the inner electrons and outer electrons.
    So, the order of electron affinities of the halogens as;
    Cl> F>Br>I\bf{Cl >  F > Br > I}

    Final answer:\bf{Final \ answer:} Option CC
  • Question 9
    1 / -0
    Electron addition would be easier in :
    Solution
    Electron addition would be easier in S2+S^{2+} because of the effective nuclear charge.
  • Question 10
    1 / -0
    The pair of amphoteric hydroxides is:
    Solution
    The pair of amphoteric hydroxides is Be(OH)2,Zn(OH)2Be(OH)_2, Zn(OH)_2.
    Amphoteric oxides reacts with acids as well as bases.
    Beryllium hydroxide is amphoteric in nature due to small size, high electronegativity and high ionisation energy of beryllium.
     Be(OH)2+2HClBeCl2+2H2O\displaystyle  Be(OH)_2 + 2HCl \rightarrow BeCl_2 + 2H_2O
     Be(OH)2+2NaOHNa2BeO2+2H2O\displaystyle  Be(OH)_2 + 2NaOH \rightarrow Na_2BeO_2 +2H_2O
    The amphoteric behaviour of zinc hydroxide is as shown.
    Zn(OH)2+2HClZnCl2+2H2O\displaystyle Zn(OH)_2 + 2HCl \rightarrow ZnCl_2 + 2H_2O
     Zn(OH)2+2NaOHNa2ZnO2sodium zincate+H2O\displaystyle  Zn(OH)_2 + 2NaOH \rightarrow \underset { \displaystyle \text {sodium zincate} } {Na_2ZnO_2} + H_2O
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