Title 08. THE D- & F-BLOCK ELEMENTS.pdf ✅

(1.) Which of the following does not represent correct transition metals series? [Page: 215] (a) 3d series (Sc to Zn ) (b) 4d series (Y to Cd ) (c) 5d series (La and Hf to Ag ) (d) 6d series (Ac and Rf to Cn ) (2.) Which of the following group does not represent transition metals? [Page: 215] (a) Zn, Cd, Hg (b) Au, Ag, Rg (c) Tc, Ru, Rh (d) Co, Ni, Cu (3.) The general electronic configuration of d − block elements is [Page: 216] (a) ( ) 1 10 0 n 1 d ns − − (b) ( ) 1 10 1 2 n 1 d ns − − − (c) ( ) 1 2 1 10 n 1 s nd − − − (d) ( ) 0 9 2 n 1 d ns − − (4.) The electronic configuration of Cu and Cr is respectively [Page: 216] (a) Ar   9 2 4 2 3d 4s , Ar 3d 4s (b) Ne   10 1 5 1 3d 4s , Ne 3d 4s (c) Ne   9 2 4 2 3d 4s , Ne 3d 4s (d) Ar   10 1 5 1 3d 4s , Ar 3d 4s (5.) Electronic configuration of a transition element X in +2 oxidation stare is Ar 5 3d . The atomic number of element X is [NCERT Exemplar Modified, Page: 216] (a) 25 (b) 26 (c) 27 (d) 24 (6.) An atom has electronic configuration 2 2 6 2 6 2 2 1s 2s 2p 3s 3p 3d 4s . In which group this element should be placed? [Page: 216] (a) fifth (b) fourth (c) third (d) second (7.) Which is the correct order of increasing energy of the listed orbitals in the atom of titanium? (At. No. 22) [AIPMT‐2015, Page: 216]
(a) 3s3p3d4s (b) 3s3p4s3d (c) 3s4s3p3d (d) 4s3s3p3d (8.) Electronic configuration of Cu is given as Ar 10 2 3d 4s . Then which of the following is correct about Cu I( ) and Cu II ( ) ? [NCERT Exemplar Modified, Page: 216] (a) E.C. of Cu I( ) is 9 3d and Cu II ( ) is 10 3d . (b) Cu II ( ) is more stable than Cu I . ( ) (c) Cu I( ) and Cu II ( ) are equally stable. (d) Stability of Cu I ( ) and Cu II ( ) depends on nature of copper salts. (9.) Identify the transition element out of the given configurations. [Page: 217] (a) 2 2 6 2 6 2 1s , 2s 2p ,3s 3p , 4s (b) 2 2 6 2 6 10 2 6 1s , 2s 2p ,3s 3p 3d , 4s 4p (c) 2 2 6 2 6 10 2 1s , 2s 2p ,3s 3p ,3d , 4s (d) 2 2 6 2 6 2 2 1s , 2s 2p ,3s 3p 3d , 4s (10.) Which of the following elements represent anomalous values of melting point for d‐block Elements? [Page: 218] (a) W & Mo (b) Mn & Tc (c) Mn & W (d) Cu & Pt (11.) The melting point of copper is higher than that of zinc because [Page: 218] (a) the atomic structure of copper is much denser than zinc (b) the atomic volume of copper is high (c) involvement of lesser number of electrons in metallic bonding (d) involvement of ( n 1 − ) d electrons in metallic bonding. (12.) The reason for occurrence of much more frequent metal‐metal bonding in compounds of the heavy transition metals is [Page: 219] (a) greater enthalpies of atomisation of heavy T.M. (b) smaller enthalpies of atomisation of heavy T.M. (c) greater number of d‐electrons of heavy transition metals (d) greater electrode potential of heavy transition metals. (13.) The metallic radius of gold is almost identical with that of silver because of [Page: 219] (a) transition metal contraction (b) the same crystal structure of silver and gold (c) the high electropositive character of gold in comparison to silver
(d) the effect of lanthanoid contraction. (14.) The reason behind the same physical and chemical properties of zirconium (4d − series) and hafnium (5d − series) is [NCERT Exemplar Modified, Page: 220] (a) same number of valence electrons (b) same value of electrode potential (c) almost similar atomic radius (d) same enthalpy of atomisation. (15.) The correct reason for lanthanoid contraction is [Page: 220] (a) imperfect shielding effect of f ‐orbitals (b) increasing nuclear charge (c) decreasing nuclear charge (d) decreasing in metallic radius. (16.) Atomic radius for few transition elements is [NCERT Exemplar Modified, Page: 220] ( ) Element : Ti Cr Fe Zn Radius pm : 147 129 126 137 Which of these elements will have highest density (a) Ti (b) Cr (c) Fe (d) Zn (17.) Which of the following factors is responsible for the value of ionisation enthalpy. [Page: 221] (a) Attraction of each electron towards nucleus (b) Repulsion between the electrons (c) Exchange energy (d) All of these (18.) March the following. [Page: 221] Column I Column II (P) element with highest second ionisation enthalpy (I) Zn (Q) element with highest third ionisation enthalpy (II) Sc (R) element with lowest first ionisation enthalpy (III) Ti (S) Maximum radius 3 M + ion (IV) Cu (a) P-I, Q-II, R-IV, S-III (b) P-II, Q-III, R-I ,S-IV (c) P-II, Q-IV, R-III, S-I
(d) P-IV, Q-I R-II, S-II (19.) Consider the given statements: [Page: 222] I Ionisation enthalpy increase with loss of exchange energy because loss of exchange energy increases the stability. II Ionisation enthalpy of Mn + is lower than Cr + as there is great loss of exchange energy at 6 d configuration. III (III)Third ionisation enthalpy of Fe is lower than that of Mn . Which of the given statement(s) is/are incorrect? (a) I & III (b) Only II (c) I & II (d) None of these (20.) Among the following pairs of ions, the lower oxidation state in aqueous solution is more stable than the other, in [Page: 223] (a) 3 Ti ,Ti + + (b) 2 Cu ,Cu + + (c) 2 3 Cr ,Cr + + (d) 2 2 V , VO + + (21.) In the form of dichromate, Cr VI ( ) is a strong oxidising agent in acidic medium but Mo VI ( ) in MoO3 and W VI ( ) in WO3 are not because [NCERT Exemplar Modified, Page: 223] (I) Mo VI ( ) and W VI ( ) are more stable than Cr VI ( ) (II) Higher oxidation states of heavier members of group‐6 of transition series are more stable. (III)Lower oxidation states of heavier members of group‐6 of transition series are more stable. (a) I only (b) I & II (c) I & III (d) None of these (22.) Out of the given statements, the correct one is/are [Page: 223] (I) Titanium (IV) is more stable than Ti III ( ) or Ti II . ( ) (II) In the d‐block elements the lower oxidation states are favoured by the heavier members. (III) Low oxidation states are found when complex compound has ligands capable of π ‐ acceptor character in addition to the o -bonding. (a) Only I (b) Only II & III (c) I & III (d) All of these