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The d- and f- Block Elements Test - 44

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The d- and f- Block Elements Test - 44
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  • Question 1
    1 / -0
    Which element is a transition metal?
    Solution
    A transition metal must have high melting point with low density.\text{A transition metal must have high melting point with low density.}
    So option C is correct.\text{So option C is correct.}
  • Question 2
    1 / -0
    Compare magnetic moment of Mn,Mn+,Mn2+,Mn3+:Mn,{ Mn }^{ + },{ Mn }^{ 2+ },{ Mn }^{ 3+ }:
    Solution

  • Question 3
    1 / -0
    Which of the following pair has similar magnetic moment?
    Solution
    The magnetic moment is given as μ=n(n+2)\mu=\sqrt{n(n+2)}
    where, n=n= number of unpaired electrons

    Fe3+Fe^{3+} and Mn2+Mn^{2+} have an equal number of 5 unpaired electrons.

    Thus, they have a similar magnetic moment.
  • Question 4
    1 / -0
    How many electron present in penultimate shell of d-block element?
  • Question 5
    1 / -0
    Transition metal compounds are usually colored. This is due to the electronic transition
    Solution
    Colour in transition series metal compounds arises due to two types of transitions. they are:
    (a) Charge transfer transitions [Ligand-to-metal charge transfer (LMCT), Metal-to-ligand charge transfer]
    (b) ddd-d transition

    In transition metal complexes, all the dd- orbitals do not possess same energy. So, electrons can jump from a lower energy dd- orbital to a higher energy dd- orbital, by absorbing energy. When it returns to the ground state, excess energy is released, and a corresponding wavelength is found in the visible region. 

    Therefore, transition metals are colored due to the electronic transition within the dd-orbitals. 

    So, option D is the correct answer.
  • Question 6
    1 / -0
    Which of the following statements is correct for the complex, K4[Fe(CN)5O2]K_4[Fe(CN)_5O_2] having t2g6,eg0t^6_{2g}, e^0_g electronic configuration?
    Solution

  • Question 7
    1 / -0

    Directions For Questions

    A metal complex having composition Cr(NH3)4Cl2BrCr(NH_3)_4Cl_2Br has been isolated in two forms, (X) and (Y). The form (X) reacts with AgNO3AgNO_3 to give a white precipitate readily soluble in dilute aqueous ammonia, whereas (Y) gives a pale yellow precipitate soluble in concentrate ammonia.

    ...view full instructions

    Choose the true statement regarding compounds X and Y.
    Solution

  • Question 8
    1 / -0
    Among the following the lowest degree of paramagnetism per mole of the compound at 298298K will be shown by?
    Solution
    The degree of paramagnetism will depend on the number of unpaired electrons because spin magnetic moment =n(n+2)\sqrt{n(n+2)}B.M
     Water is a weak field ligand, so there will be no pairing of electrons as the interaction of the central metal with water molecules is very weak. All the metal ions are in +2+2 oxidation state. The valence shell electronic configuration of Cu+2Cu^{+2} is 3d94s03d^{9}4s^{0}. So, Cu2+Cu^{2+} has only one unpaired electron. 
    Mn2+Mn^{2+} has four unpaired electrons.
    Fe2+Fe^{2+} has four unpaired electrons.
    Ni+2Ni^{+2} has two unpaired electrons.

    Therefore, the lowest degree of paramagnetism per mole of the compound is shown by CuSO4.5H2OCuSO_4.5H_2O.

    Hence, the correct option is (C).

  • Question 9
    1 / -0
    Which of the following statements is correct?
    Solution
    The complex [Fe(CN)4(O2)]4[Fe(CN)_{4}(O_{2})]^{-4} is an octahedral complex. So, it may have the hybridization of sp3d2sp^{3}d^{2} or d2sp3d^{2}sp^{3}. As CNCN^{-} is a strong field ligand, the electronic configuration of Fe+3Fe^{+3} in the complex will be t2g6eg0t_{2g}^{6}e_{g}^{0} due to the pairing of electrons.

    So, it will be an inner-orbital complex involving the inner 3d3d orbitals (d2sp3d^{2}sp^{3} hybridisation). It is also a diamagnetic complex as all the t2gt_{2g} electrons are paired up. 

    So, option (A) is correct.
  • Question 10
    1 / -0
    An aqueous solution of titanium chloride, when subjected to magnetic measurement, measured zero magnetic moment. Assuming the complex as octahedral in aqueous solution, the formula of the complex is?
    Solution
    Magnetic moment of any complex arises due to the presence of unpaired electron(s) in the central metal ion or atom. An octahedral complex is a complex surrounded by six monodentate ligands inside the coordination sphere. In the compound [Ti(H2O)6]Cl4[Ti(H_{2}O)_{6}]Cl_{4}, TiTi is in +4+4 oxidation state. It has an electronic configuration of [Ar]3d0[Ar]3d^{0}. Hence, it has zero magnetic moment. So, the formula [Ti(H2O)6]Cl4[Ti(H_2O)_6]Cl_4 fits for the conditions mentioned in the question. 

    Therefore, the correct option is (B).

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