Periodic Classification of Elements Questions PDF

622 Chemical Periodicity  The electron affinity of exactly half-filled configuration is approximately zero and...

622 Chemical Periodicity  The electron affinity of exactly half-filled configuration is approximately zero and exactly zero for fully filled configuration.  The electron affinities of gaseous anions are always negative.  Some of the polar crystals when heated produce electric current. This phenomena is termed as piezoelectric effect.  The IUPAC nomenclature of elements > 100  All the elements of f- block (4f series – Lanthanides and 5f series – In IUPAC system, the names are derived by using roots for the three Actinides) are placed in 3rd group (IIIB) and form a separate block digits in the atomic number of the element and adding the ending : ium. at the bottom of the periodic table. The roots for the numbers are Number 0 1 2 3 4 5 6 7 8 9 Root nil un bi tri quad pent hex hept oct enn Atomic Number Name Symbol 101 un-nil-unium Unu 102 un-nil-bium Unb Extended or long form of periodic table 103 un-nil-trium Unt 104 un-nil-quadium Unq 1. Which of the following statement is not correct for the element 105 un-nil-pentium Unp having electronic configuration 1s 2 ,2 s 2 p 6 , 3 s1 106 un-nil-hexium Unh (a) It is a monovalent electropositive (b) It forms basic oxide 107 un-nil-septium Uns (c) It is a non-metal 108 un-nil-octium Uno (d) It has low electron affinity 109 un-nil-ennium Une 2. Which of these dose not reflect the periodicity of the elements [UPSEAT 2001; BI 110 un-un-nilium Uun (a) Bonding behaviour (b) Electronegativity (c) Ionization energy (d) Neutron/proton ratio 111 un-un-unium Uuu 3. If an atom has electronic configuration 112 un-un-bium Uub 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 3d 3 4 s 2 , it will be placed in 113 un-un-trium Uut [CBSE PMT 2002] 114 un-un-quadium Uuq (a) Second group (b) Third group (c) Fifth group (d) Sixth group 115 un-un-pentium Uup 4. All the s–block elements of the periodic table are placed in the 116 un-un-hexium Uuh groups … [Orissa JEE 2002] 117 un-un-septium Uus (a) IA and IIA (b) IIIA and IVA (c) B sub groups (d) VA to VIIA 118 un-un-octium Uuo 5. The electronic configuration of halogen is 119 un-un-ennium Uue [MP PET/PMT 1998; Pb. PMT 2001]  Elements of second period are known as Bridge elements. Their (a) ns 2 np 6 (b) ns 2 np 3 properties resemble with the properties of diagonal elements of third period. (c) ns 2 np 5 (d) ns 2  For isoelectronic ions the size depends on the nuclear charge. 6. Hydrogen by donating one electron forms H . In this property, it Greater is the nuclear charge smaller is the size. resembles with (a) Transitional metals (b) Alkaline earth metals  The incease in magnitude of radii is more in the beginning of a (c) Alkali metals (d) Halogens group because the difference in energy between energy shells is more. 7. The tenth elements in the periodic table resembles with the [CPMT 1988]  The ionisation potentials provide an indication about the number of (a) First period (b) Second period valence electrons (s) in an atom e.g., Na has IE >>> IE (because it 2 1 (c) Fourth group (d) Ninth group has one valence electron) while Mg has IE >>> IE > IE because it 3 2 1 8. The element with quantum numbers n  2, l  1, m  1, s  1 / 2 has two valence electrons and attains noble gas configuration after has the following position in the periodic table losing 2 electrons. (a) Group VII-A, period II (b) Group 0, period II  The highest I.E. in a period is shown by noble gas. (c) Group VII-A, period III (d) Group 0, period III 9. Who developed the long form of periodic table  The electronegativity of a series of transition metals is almost [MP PET 1997] similar. The electronegativity of all lanthanide’s are identical (1.1). (a) Lothar Meyer (b) Niels Bohr (c) Mendeleef (d) Moseley  The most electronegative elements is Fluorine (value is 4.0 on the 10. The electronic configuration of an element is Pauling scale). The least electronegative elements is Cs and Fr with 1s 2 , 2 s 2 2 p 6 , 3 s 2 3 p 3. What is the atomic number of the a value of 0.700. element which is just below the above element in the periodic table[CBSE PMT  Chemical Periodicity 623 (a) 33 (b) 34 25. Which of the following elements is a lanthanide (Rare–earth (c) 31 (d) 49 element) [Manipal MEE 1995] 11. In the periodic table, the element with atomic number 16 will be (a) Cadmium (b) Californium placed in the group [MP PET/PMT 1998] (c) Cerium (d) Cesium (a) Third (b) Fourth 26. Mendeleef's periodic law is based on (c) Fifth (d) Sixth (a) Atomic weight (b) Atomic number 12. The first element of rare–earth metals is [AFMC 1992] (c) Number of neutrons (d) None of the above (a) Cerium (b) Actinium 27. The heaviest atom amongst the following is (c) Uranium (d) Lanthanum [CPMT 1976; NCERT 1976] 13. The d -block elements consists mostly of [MP PMT 1994] (a) U (b) Ra (a) Monovalent metals (c) Pb (d) Hg (b) All non-metals 28. Which of the following pairs has both members from the same group of the periodic table (c) Elements which generally form stoichiometric metal oxide [CPMT 1985; MP PET/PMT 1998] (d) Many metals with catalytic properties (a) Mg  Ba (b) Mg  Na 14. “The 6 properties of the elements are periodic function of their atomic numbers.” The statement was given by (c) Mg  Cu (d) Mg  K [MNR 1995] 29. Which of the following pairs has both members from the same (a) N. Bohr (b) J.W. Dobereiner period of the periodic table (c) D.I. Mendeleef (d) H.G.J. Moseley [CPMT 1985; UPSEAT 2001; BHU 2003] 15. The long form of periodic table has (a) Na  Ca (b) Na  Cl [CPMT 1986; KCET 1998] (c) Ca  Cl (d) Cl  Br (a) Eight horizontal rows and seven vertical columns 30. Diagonal relationship is shown by [DPMT 1984] (b) Seven horizontal rows and eighteen vertical columns (a) Elements of first period (c) Seven horizontal rows and seven vertical columns (b) Elements of second period (d) Eight horizontal rows and eight vertical columns (c) Elements of third period 16. The telluric helix was given by [AFMC 1990] (d) (b) and (c) both (a) De Chan Courtois (b) Newlands 31. The elements having the electronic configuration, [ Kr ] (c) L. Meyer (d) Mendeleef 4 d 10 f 14 , 5 s 2 p 6 d 2 , 6 s 2 belongs to [CPMT 1982] 17. Which one of the following belongs to representative group of (a) s-block (b) p-block elements in the periodic table [Kurukshetra CEE 1991] (c) d-block (d) f-block (a) Lanthanum (b) Argon 32. Chemical property of Li and Mg similar because (c) Chromium (d) Aluminium [RPMT 2002] 18. An element of atomic number 29 belongs to (a) These belong to same group [CPMT 1991; Kurukshetra CEE 1991; MP PET 2001] (b) Both ionisation potential is same (a) s -block (b) p -block (c) Shows diagonal relationship (c) d -block (d) f -block (d) Both electron affinity is same 19. The element californium belongs to the family 33. According to the periodic law of elements, the variation in [MNR 1987] properties of elements is related to their [AIEEE 2003] (a) Actinide series (b) Alkali metal family (a) Atomic masses (c) Alkaline earth family (d) Lanthanide series (b) Nuclear masses 20. On moving from left to right across a period in the table the (c) Atomic numbers metallic character [CPMT 1986] (d) Nuclear neutron-proton number (a) Increases 34. The element with atomic number 36 belongs to …… block in the (b) Decreases periodic table [KCET 2003] (c) Remains constant (a) p (b) s (d) First increases and then decreases (c) f (d) d 21. An element with atomic number 20 will be placed in which period 35. Which group of the periodic table contains only metals of the periodic table [MNR 1986; UPSEAT 1999] [UPSEAT 2003] (a) 4 (b) 3 (a) IIA (b) IB (c) 2 (d) 1 (c) IA (d) None of these 22. The electronic structure (n  1) d 110 ns 0  2 is characteristic of 36. The elements in which s and p-orbitals are present [CET Pune 1998] (a) Common elements (a) Transition elements (b) Lanthanides (b) Inert gases (c) Actinides (d) Rare gases (c) Halogens 23. The elements with atomic number 10, 18, 36, 54 and 86 are all[CPMT 1976] (d) Transitional elements (a) Light metals (b) Inert gases 37. Aluminium is diagonally related to (in periodic table) (c) Halogens (d) Rare–earths [MP PET 1993] 24. Elements of atomic number 6 is placed in [CPMT 1978] (a) Li (b) C (a) IV group (b) IV period (c) B (d) Be (c) VI group (d) III group  624 Chemical Periodicity 38. An element has the electronic configuration 1s 2 , 2 s 2 2 p 6 , (c) As , Bi (d) Pb , Sb 50. Dobereiner traids is [RPMT 1997] 3 s 2 3 p 6 3d 5 , 4 s 1. It is a (a) Na , K , Rb (b) Mg, S , As (a) s-block element (b) p-block element (c) Cl , Br, I (d) P, S , As (c) d-block element (d) Inert gas 51. As per the modern periodic law, the physical and chemical 39. Which of the following show diagonal relationship properties of elements are periodic functions of their [KCET 2003; MP PMT 2003] [RPMT 1997; EAMCET 1998] (a) B and Si (b) B and Al (a) Atomic volume (c) B and Ga (d) B and C (b) Electronic configuration 40. Which of the following dinegative anion is quite common (c) Atomic weight [CPMT 2000] (d) Atomic size (a) S 2 (b) Se 2 52. Elements after atomic number 103 have been discovered till now. If an element with atomic number 106 were ever discovered which of (c) Te 2  (d) O 2 the following electronic configuration will it possess [AIIMS 1982] 41. An element has electronic configuration 1s 2 2 s 2 2 p 6 3 s 2 3 p 4. (a) [Rn] 5 f 14 6 d 4 7 s 2 (b) [Rn] 5 f 14 6 d 5 7 s1 Predict their period, group and block [CPMT 2000] (c) [Rn] 5 f 14 6 d 6 7 s 0 (d) [Rn] 5 f 14 6 d 1 7 s 2 7 p 3 (a) Period = 3 , block = p, group = 16 rd 53. The element X, Y, Z and T have the indicated electronic configurations. Starting with the innermost shell, which is the most (b) Period = 5 , block = s, group = 1 th metallic element [CPMT 1979, 93] (c) Period = 3 , block = p, group = 10 rd (a) X  2, 8, 4 (b) Y  2, 8, 8 (d) Period = 4 , block = d, group = 12 th 42. If the atomic number of an element is 33, it will be placed in the (c) Z  2, 8, 8, 1 (d) T  2, 8, 8, 7 periodic table in the [RPET 1999; UPSEAT 2001, 02] 54. Which pair of atomic numbers represents s -block elements (a) First gp (b) Third gp [EAMCET 1990; RPMT 1997; MP PET 2003] (c) Fifth gp (d) Seventh gp (a) 7, 15 (b) 6, 12 43. Which of the following is the atomic number of a metal (c) 9, 17 (d) 3, 12 [AIIMS 2000] 55. Which pair of elements has same chemical properties (a) 32 (b) 34 [EAMCET 1987] (c) 36 (d) 38 (a) 13, 22 (b) 3, 11 44. Which of the following statement is not correct regarding hydrogen (c) 4, 24 (d) 2, 4 atom [AIIMS 2000] 56. Mosley's name is most closely associated with the discovery of (a) It resembles halogens in some properties (a) Positron (b) Deutrons (b) It resembles alkali metals in some properties (c) Atomic number (d) Atomic weight (c) It can be placed in 7 group of periodic table th 57. In the periodic table going down in fluorine group (d) It can not be placed in first group of periodic table [CPMT 1981] 45. Lithium shows similarities to magnesium in its chemical behaviour (a) Reactivity will increase because [AFMC 2000] (b) Electronegativity will increase (a) Similar size, same electronegativity and lower polarizing power (c) Ionic radius will increase (b) Similar size, greater electronegativity and similar polarizing (d) Ionization potential will increase power 58. Beryllium resembles much with [CPMT 1988] (c) Similar size, same electronegativity and similar high polarizing (a) Zn (b) Al power (c) Li (d) Ra (d) None of these 59. The last member in each period of the periodic table is 46. On going left to right in a period, in transition metals, their atomic volumes [MP PMT 2003] [DPMT 2001] (a) Decrease (b) Increase (a) An inert gas element (b) A transition element (c) Remain same (d) None of these of correct (c) A halogen (d) An alkali metal 47. Electronic configuration of chalcons in their outermost orbit is 60. Which one of the following combination represents a metallic element [EAMCET 1979] (a) s2 p3 (b) s2 p4 (a) 2, 8, 7 (b) 2, 8, 8 (c) s 2 p 5 (d) s 2 p 6 (c) 2, 8, 4 (d) 2, 8, 2 48. Which configuration represents a noble gas [DPMT 2000] 61. The electronic configuration of an atom A is 1s 2 , 2s 2 p 6 , (a) 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 3d 10 4 s 2 3 s 2 p 6 d 10 , 4 s 2 p 3. The chemistry of A is therefore likely to be similar to that of [MP PMT 1995] (b) 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 (a) Chlorine (b) Nitrogen (c) 1s 2 2 s 2 2 p 6 3 p 6 (c) Oxygen (d) Boron (d) 1s 2 2 s 2 2 p 6 3 s 2 62. The element having the electronic configuration 1s 2 , 49. Which of the following pair has elements containing same number 2 s 2 2 p 6 , 3 s 2 3 p 1 is of electrons in the outermost orbit (a) A transition element [Kurukshetra CEE 1998; AFMC 2000] (b) A representative element (a) N, O (b) Na , Ca (c) An inert gas  Chemical Periodicity 625 (d) An inner–transition element 75. Chemical behaviour of an atom is determined by 63. 2 2 6 2 The element with configuration 1s , 2 s p , 3 s would be (a) Atomic number (b) Mass number (c) Binding energy (d) Number of isotopes [CPMT 1986; MP PMT 1993] 76. Which of the following is a inert element (a) A metal (b) A non-metal (a) Na (b) Fe (c) An inert gas (d) A metalloid 64. The long form of periodic table is based on [CPMT 1997] (c) Li (d) He 77. The lightest metal is (a) Shape of the atom [CPMT 1976; NCERT 1976; AFMC 1988] (b) Mass of the atom (c) Atomic number of the atom (a) Li (b) Mg (d) Electronegativity (c) Ca (d) Na 65. Chloride of an element A gives neutral solution in water. In the 78. Choose the typical element periodic table, the element A belongs to (a) K (b) Na [AIIMS 1992; UPSEAT 2001] (c) Sc (d) He (a) First group (b) Third group 79. Of the following pairs, the one containing example of metalloid (c) Fifth group (d) First transition series elements in the periodic table is 66. The fundamental basis of the present-day Periodic Table is that (a) Sodium and potassium elements are [JIPMER 1999] (b) Fluorine and chlorine (a) Arranged in the order of increasing atomic weights (c) Calcium and magnesium (b) Grouped according to chemical properties (d) Boron and silicon (c) Arranged in the order of increasing number of neutrons in the 80. The number of elements in each of the long periods in the periodic atomic nucleus table is (d) Arranged in the order of increasing number of protons in the (a) 2 (b) 8 nucleus (c) 18 (d) 32 67. 81.MP PET All the elements in a group in the periodic table have the same [NCERT 1974; In the 1996;long form 1996] MP PMT of the periodic table, all the non- metals are placed (a) Atomic number under [EAMCET 1988] (b) Electronic configuration (a) s-block (b) p-block (c) Atomic weight (c) d-block (d) f-block (d) Number of electrons in the outermost shell or number of 82. Elements with outer electronic configuration ns 2 np 6 are electrons for bonding [MP PET/PMT 1998] 68. The most predominantly ionic compounds will be obtained from the (a) Alkaline earth metals (b) Transition elements combination of elements belonging to (c) Chalcogenes (d) Noble gases (a) 1 and 7 groups (b) 2 and 6 groups 83. Highest density is of ………. [RPET 2000] (c) 3 and 5 groups (d) 0 and 7 groups 69. An atom with atomic number 21 belongs to the category of (a) Ir (b) Os [Kurukshetra CEE 1991] (c) Pb (d) Hg (a) s -block elements (b) p -block elements 84. Lithium shows diagonal relationship with (c) d -block elements (d) f -block elements [MP PET 1995, 96; EAMCET 1990] (a) Al (b) Mg 70. Which metal has 2 electrons in the outermost orbit (c) Be (d) B (a) Na (b) Cu (c) Au (d) Be 85. 1s 2 2 s 2 2 p 6 3 s 2 is the electronic configuration of the metal 71. In the modern periodic table, elements are arranged in [RPET 2000] [MP PMT 1990; MP PET 1995; CPMT 1971, 73, 78, 80] (a) Na (b) Mg (a) Increasing mass (c) Fe (d) Al (b) Increasing volume 86. Element having atomic number 17 is placed in (c) Increasing atomic number [MP PET 1995] (d) Alphabetically (a) I-group (b) V-group 72. Alkali metals in each period have [MP PMT 1995] (c) VIII-group (d) VII-group (a) Smallest size 87. The most importasnt active step in the development of periodic (b) Lowest ionization potential table was taken by [CPMT 1976] (c) Highest ionization potential (a) Mendeleef (b) Dalton (d) Highest electronegativity (c) Avogadro (d) Cavendish 73. The elements on the right side of the periodic table are 88. Who is called the father of chemistry [CPMT 1972] [CPMT 1976] (a) Faraday (b) Priestley (a) Metals (b) Metalloids (c) Rutherford (d) Lavosier (c) Non-metals (d) Transition elements 89. The total number of rare–earth elements is [CPMT 1993] 74. The screening effect of d-electons is [RPMT 2000] (a) 8 (b) 32 (a) Equal to that of p-electrons (c) 14 (d) 10 (b) More than that of p-electrons 90. Which is metalloid [Bihar MEE 1997] (c) Same as f-electrons (a) Pb (b) Sb (d) Less than p-electrons  626 Chemical Periodicity (c) Bi (d) Zn 104. To which block is related an element having electronic configuration (e) Mg 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 3d 10 4 s 1 in the periodic table [MP PMT 1995] 91. The element or elements whose position is anomalous in the (a) s - block (b) p - block periodic table is (c) d - block (d) f – block (a) Halogens (b) Fe, Co and Ni 105. Ce  58 is a member of (c) Inert gases (d) Hydrogen (a) s-block elements (b) p-block elements 92. An element M has an atomic mass 19 and atomic number 9. Its ion (c) d-block elements (d) f-block elements is represented by 106. Atomic number of elements represent (a) M (b) M (a) Number of protons in the nucleus (c) M 2  (d) M 2  (b) Number of neutrons in the nucleus 93. The number of elements in the 5th period of the periodic table are (c) Number of protons and neutrons in nucleus (a) 8 (b) 10 (d) The valency of an element (c) 18 (d) 32 107. As we go from left to right in period two of the periodic table, gram atomic volume of the elements 94. The element with atomic number 55 belongs to [MP PMT 1995] (a) Will change indefinitely (a) s-block (b) p-block (b) Increases at a constant rate (c) d-block (d) f-block (c) First increases then decrease 95. Coloured salts are formed by [Bihar MEE 1996] (d) Decreases (a) Alkali metals (b) Lanthanides 108. The electronic configuration of the element which is just above the (c) Actinides (d) Transition metals element with atomic number 43 in the same periodic group is[MNR 1992; UPSEA (e) None of these (a) 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 5 4 s 2 96. Which one of the following is an s - block element [MP PMT 1999] (b) 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 3d 10 4 s 2 4 p 5 (a) Aluminium (b) Chromium (c) 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 6 4 s 1 (c) Niobium (d) Potassium 97. In the modern periodic table, the place of the element with atomic (d) 1s 2 2 s 2 2 p 6 3 s 2 3 p 6 3d 10 4 s 1 4 p 6 number 31 is in [MP PMT 1999] 109. The elements indicating following atomic numbers belong to same (a) s - block (b) d- block group [RPMT 1997] (c) p -block (d) f – block (a) 11 and 37 (b) 19 and 15 98. Last element of group-IV is found to be [DPMT 1996] (c) 39 and 88 (d) None of these (a) Strong metallic 110. Elements in which 4 f orbitals are progressively filled are called as[MP PET 199 (b) Weak metallic (a) Transition elements (b) Lanthanides (c) Strong non-metallic (c) Actinides (d) Inert gases (d) Weak non-metallic 111. Hydrogen can be put in halogen group because 99. Elements of d group are called [DPMT 1996] [RPMT 2000] (a) Transition elements (b) Transuranic elements (a) It has deuterium and tritium as isotopes (c) Metals (d) Metalloids (b) It forms hydrides like chlorides 100. Which of the following is a normal element (c) It contains one electron only (a) Ce (b) He (d) It is light (c) Li (d) Ar 112. In the main group elements (i) as we proceed down the same group 101. Which of the following is metalloid [BHU 1996; AMU 2000] in the periodic table and (ii) as we proceed from left to right in the (a) Pb (b) Zn same period, the atomic radius (c) As (d) None of these (a) (i) Increase continuously; (ii) Decreases continuously 102. Under normal condition which of the following electronic (b) (i) Decreases continuously; (ii) Increases continuously configuration is able to form dipositive ion [RPET 2000] (c) (i) Increases continuously; (ii) Decreases upto the group IV and (a) [ Ar] 4 s1 (b) [ Ne ] 2 s 2 3 p 6 then increases upto the end of the period. (d) (i) Decreases continuously; (ii) Decreases upto the group IV (c) [ Ne ] 3 s 2 (d) None of these and then increases upto the end of the period. 103. The statement that is true for the long form of the periodic table is[IIT 1988] 113. Cause of diagonal relationship is (a) It reflects the sequence of filling the electrons in the order of (a) Similar electronic configuration of the elements sub-energy levels s, p, d and f (b) Similar e / r ratio of the elements (b) It helps to predict the stable valency states of the elements (c) It reflects trends in physical and chemical properties of the (c) Same number of valency electrons in the elements elements (d) Same atomic weights of the elements (d) It helps to predict the relative ionicity of the bonds between any two elements 114. From which of the following the hydration energy of Mg 2  is larger [MP PET 2000]  Chemical Periodicity 627 (a) Na  (b) Al 3  (b) Number of protons (c) Number of neutrons (c) Be 2 (d) Cr 3  (d) Number of isotopes 115. Group comprising of all metals is [RPET 2000] (e) Number of nucleons (a) IIIA (b) IVA 127. Beryllium shows diagonal relationship with [Pb.CET 2003] (c) VIIA (d) IIA (a) Mg (b) Na 116. Whose name is not associated with the development of Periodic (c) B (d) Al Table [DCE 1999] 128. Which of the properties remains unchanged on descending a group (a) Prout’s (b) Newlands in the periodic table (c) Rutherford (d) Loother Meyer [MP PMT 1997; RPMT 2002] 117. Element of atomic number 23 is placed in the periodic table in [MP PMT 1996] (a) Atomic size (b) Density (a) s - block (b) p – block (c) Valence electrons (d) Metallic character (c) d - block (d) f - block 129. Which of the following element does not occur in liquid form [RPMT 2002] 118. In which of the following groups all the three members are of the alkaline earth metals family (a) Hg (b) Li (c) Ga (d) Br (a) Al, Sr , Ti (b) Li, Na, K 130. The cause of periodicity of properties is (c) Mg, Ba, Ca (d) Rb, Cs, Fr (a) Increasing atomic radius 119. Astatine is a [RPET 2000] (b) Increasing atomic weights (c) Number of electrons in the valency orbit (a) Halogen (d) The re-occurrence of similar outer electronic configuration (b) Rare earth element 131. The chemistry of lithium is very similar to that of magnesium even (c) Alkaline earth metal though they are placed in different groups (d) None of these [NCERT 1982] 120. The nitride ion in lithium nitride is composed of (a) Both are found together in nature [CBSE PMT 2001] (b) Both have nearly the same size (c) Both have similar electronic configuration (a) 7 P  7e (b) 10 P  7 e (d) The ratio of their charge to size is nearly the same (c) 7 P  10e (d) 10 P  10e 121. Which set has the same number of unpaired electrons in their Atomic and Ionic radii ground state [JIPMER 2000] (a) Cl  , Fe3  , Cr 3  (b) Na  , Mg 2  , Al 1. The ratio between radii of He  ion and H atom is [MP PET 1996] (c) Na, P, Cl (d) N , P, V 1 (a) (b) 1 122. Which of the following doesn’t decompose on heating 2 [AMU 2002] 3 (c) (d) 2 (a) MgCO3 (b) Na 2 CO 3 2 2. The smallest among the following ions is [JIPMER 1999] (c) Li2 CO 3 (d) Ca (HCO 3 )2  2 (a) Na (b) Mg 123. Which of the following has smallest bond angle 2 (c) Ba (d) Al 3  [AMU 2002] 3. Which is smallest in size [RPMT 1997] (a) H 2O (b) NH 3 2 4 (a) O (b) C (c) CH 4 (d) CO 2 (c) F  (d) N 3  4. Which of the following has largest size 124. The metal-having highest melting point is [MP PMT 1995, 2003; JIPMER (Med.) 2002] [AMU 2002] (a) Al (b) Al  (a) Chromium (b) Tungston 2 (c) Al (d) Al 3 (c) Diamond (d) Silver 5. Of the following, the one with largest size is 125. The elements with atomic numbers 9, 17, 35, 53, 85 are all [EAMCET 1997; BHU 1999] [KCET 2004]  (a) Cl (b) Ar (a) Noble gases (b) Halogens (c) K  (d) Ca 2  (c) Heavy metals (d) Light metals 6. Which cation has smallest radius [RPET 2000] 126. The atomic number of an element is derived from (a) K (b) Na  [Kerala PMT 2004] (c) Li  (d) Be 2  (a) Number of electrons  2 7. The radii of F, F , O and O are in the order of  628 Chemical Periodicity [AIIMS 1999; CPMT 1999] (a) Mg 2   Na   F   Al (a) O 2  F   O  F (b) O 2  F   F  O (b) F   Al  Na   Mg 2  (c) F   O 2  F  O (d) O 2  O  F   F 8. Which of the following has the smallest size (c) Al  Mg  F   Na  [CBSE PMT 1996] (d) Na   Al  F   Mg 2  (a) Na  (b) Mg 2 21. In K  F  ionic radius of F  is more while atomic radius of K  (c) Cl  (d) F is [CPMT 1997] 9. Which of the following is largest [CBSE PMT 1996] (a) Less than F  (b) More than F  (a) Cl  (b) S 2 (c) Equal of F  (d) None of these (c) Na  (d) F  22. Which one of the following species possesses maximum size 10. Which of the following property displays progressive increase down [EAMCET 1993; MP PET 2001] a group in the Bohr's periodic table  (a) Electronegativity (b) Electron affinity (a) Na (b) F (c) Ionization potential (d) Size of the atom (c) Ne (d) O 2  11. Atomic radii of fluorine and neon in angstrom units are respectively 23. The ionic radii of N 3  , O 2  , F  and Na  follow the order[MP PET/PMT 19 given by [IIT 1987] (a) 0.762, 1.60 (b) 1.60, 1.60 (a) N 3   O 2   F   Na  (c) 0.72, 0.72 (d) None of these values (b) N 3   Na   O 2   F  12. Which ion has greatest radius in the following (c) Na   O 2  N 3   F  [CPMT 1976; NCERT 1977] (d) O 2   F   Na   N 3  (a) H (b) F 24. On moving down a group of regular elements, both atomic and ionic (c) Br  (d) I  radii increases with increasing [BMEE 1995] 13. Which has the maximum atomic radius (a) Atomic number (b) Atomic weight [CPMT 1975; AIIMS 1982; DPMT 1982] (c) Atomic mass (d) None of these (a) Al (b) Si 25. Which one of the following indicates the correct order of atomic size[EAMCET 1 (c) P (d) Mg (a) Be > F > C > Ne (b) Be < C < F < Ne 14. Which one of the following ions has the highest value of ionic radius (c) Be > C > F > Ne (d) F < Ne < Be < C [AIEEE 2004] 26. Which has the smallest size [MP PET 1999] 2 3 (a) O (b) B (a) Na  (b) Mg 2    (c) Li (d) F (c) Al 3  (d) P 5  15. On going down a main sub-group in the periodic table (example Li 27. A sodium cation has a different number of electrons from to Cs in IA or Be to Ra in IIA), the expected trend of changes in atomic radius is a (a) O 2 (b) F [CPMT 1981; NCERT 1979] (c) Li  (d) Al 3  (a) Continuous increase 28. Which of the following statement concerning lanthanides elements is (b) Continuous decrease false [CBSE PMT 1994] (c) Periodic one, an increase followed by a decrease (a) Lanthanides are separated from one another by ion exchange (d) A decrease followed by increase method 16. Which one of the following is the smallest in size (b) Ionic radii of trivalent lanthanides steadily increases with [IIT 1989] increase in the atomic number (a) N 3 (b) O 2 (c) All lanthanides are highly dense metals (c) F  (d) Na  (d) More characteristic oxidation state of lanthanide elements is 17. Which one is the correct order of the size of the iodine species +3 [Pb. CET 1986; CBSE PMT 1997; Kurukshetra CEE 1998; 29. The lanthanide contraction is responsible for the fact that RPMT 1999; DCE 1999; MP PET 2000; [CBSE PMT 1997] MP PMT 2001; BCECE 2005] (a) Zr and Y have about the same radius (a) I  I  I (b) I  I  I (b) Zr and Nb have similar oxidation state   (c) I  I  I (d) I  I  I (c) Zr and Hf have about the same radius 18. Which one has larger radius [CPMT 1997; KCET 2005] (d) Zr and Zn have the same oxidation state (a) Na  (b) F 30. Elements of which group form anions most readily [CBSE PMT 1992] (c) F  (d) Na (a) Oxygen family (b) Nitrogen group 19. In third row of periodic table the atomic radii from Na to Cl (c) Halogens (d) Alkali metals [MP PMT 1986] 31. The unit representing atomic radii and ionic radii is (a) Continuosly decreases (b) Continuosly increases (a) nm (b) cm (c) Remains constant (c) Å (d) m (d) Increases but not continuously 32. The atomic radii in periodic table among elements from right to left[MP PET 199 20. The size of the following species increases in the order (a) Decreases [IIT-JEE 1990; AFMC 1995]  Chemical Periodicity 629 (b) Increases 44. Which is helpful in the formation of ionic bond (c) Remain constant (a) Only small cation (d) First decreases and then increases (b) Only small anion 33. Of the following the ion with the smallest ionic radius is (c) Small cation and small anion both [MP PET 1996] (d) Low positive charge, large cation and small anion  2 45. Which of the following has largest ionic radius (a) K (b) Ca [AFMC 1999; BHU 2003] (c) Ti 3  (d) Ti 4    34. Which of the following does not represent the correct order of the (a) Cs (b) Li property indicated [CBSE PMT 1997] (c) Na  (d) K  (a) Sc 3   Cr 3   Fe 3   Mn 3  ionic radii 46. Point out the wrong statement : (b) Sc  Ti  Cr  Mn Density On moving horizontally from left to right across a period in the periodic table (c) Mn 2   Ni 2   Co 2  Fe 2 ionic radii (a) Metallic character decreases (d) FeO  CaO  MnO  CuO Basic nature (b) Electronegativity increases 35. The order of magnitude of ionic radii of ions Na  , Mg 2 , Al 3  (c) Gram atomic volume first decreases and then increases (d) Size of the atoms increases for normal elements and Si 4  is [MP PMT 1996] 47. Which of the following statements is correct  2 3 4 (a) Na  Mg  Al  Si [MP PET 1997] 2  3 4  (b) Mg  Na  Al  Si (a) X ion is larger in size than X atom 3  4 2  (c) Al  Na  Si  Mg (b) X ion is larger in size than X atom  (d) Na   Mg 2   Al 3   Si 4  (c) X ion is larger in size than X  ion (d) X and X  ions are equal in size  36. The order of the magnitude of ionic radii of ions N 3  , O 2  and 48. The atomic radius of elements of which of the following series F  is [MP PMT 1996] would be nearly the same [MP PET 1997] (a) N 3   O 2  F  (b) N 3   O 2  F  (a) Na K Rb Cs (b) Li Be B C (c) N 3   O 2   F  (d) N 3   O 2  F  (c) Fe Co Ni Cu (d) F Cl Br I 37. Which statement is correct 49. The decreasing order of size of isoelectronic series K  , Ca 2  , Cl  (a) For potassium, the atomic radius < ionic radius; but for bromine, the atomic radius > ionic radius and S 2  is [Roorkee 1995] (b) For potassium and bromine both, the atomic radii > ionic radii  2 2  (a) K  Ca S  Cl (c) For potassium and bromine both, the atomic radii < ionic radii  2 (d) For potassium, the atomic radius > ionic radius but for (b) K  Ca  Cl  S 2   2 bromine, the atomic radius < ionic radius (c) Ca  K  Cl   S 2   38. Which of the following ion is the smallest ion (d) S 2   Cl   K   Ca 2  [AIIMS 2001] 50. Which of the following sets of elements have the strongest tendency (a) O 2 (b) O 2 to form anions [MP PET 1993] (c) O 2 (d) O 22 (a) N, O, F (b) P, S, Cl (c) As, Se, Br (d) Sb, Te, I 39. The correct order of radii is [IIT-JEE (Screening) 2000] 51. Radius of the isoelectronic species [MP PET 1994] (a) N  Be  B (b) F   O 2  N 3  (a) Increases with the increase of nuclear charge (c) Na  Li  K (d) Fe3  Fe 2  Fe4  (b) Decreases with the increase of nuclear charge 40. Which one of the following should be most stable (c) Is the same for all [MP PET 2000] (d) First increases and then decreases (a) H 2 (b) H  52. In which of the following pairs the difference between the covalent radii of the two metals is maximum (c) H (d) H  [MP PET 1994] 41. Which of the following is the correct order of ionic radii (a) K, Ca (b) Mn , Fe [BHU 2002] (c) Co , Ni (d) Cr , Mn (a) F  Li  Na  K (b) F  K  Na  Li 53. An atom of an element has electronic configuration 2, 8, 1. Which of the following statement is correct [MP PMT 1994] (c) Na  K  F  Li (d) Li  Na  K  F (a) The element's valency is 7 42. Smallest among these species is [KCET 2002] (b) The element exists as a diatomic molecule (a) Lithium ion (b) Hydrogen (c) The element is of non-metallic nature (c) Lithium (d) Helium (d) The element forms a basic oxide 43. Which of the following ionic radius would be maximum 54. Which of the following ions has the smallest radius [MP PET 1997] [KCET 1992] (a) C 4 (b) N 3 2  (a) Be (b) Li (c) O 2 (d) Mg 2  (c) O 2 (d) F  630 Chemical Periodicity 55. Point out the wrong statement : 67. The trivalent ion having largest size in lanthanide series is In a given period of the periodic table the s - block element has, in [Pb.PMT 2004] general, a lower value of [MP PMT 1997] (a) Ti (b) Zr (a) Ionisation energy (b) Electronegativity (c) Hf (d) La (c) Atomic radius (d) Electron affinity 68. Which of the following alkali metal ions has lowest ionic mobility in 56. Arrange the following in increasing order of their atomic radius : aqueous solutions [DPMT 2004] Na, K, Mg, Rb [AFMC 1995, 97; CPMT 1999] (a) Mg < K < Na < Rb (b) Mg < Na < K < Rb (a) Rb  (b) Cs  (c) Mg < Na < Rb < K (d) Na < K < Rb < Mg (c) Li  (d) Na  3 2 57. In the isoelectronic species the ionic radii (Å) of N , O and 69. Ionic radii are [CBSE PMT 2003, 04] F  are respectively given by [Pb. CET 1989] (a) Directly proportional to effective nuclear charge (a) 1.36, 1.40, 1.71 (b) 1.36, 1.71, 1.40 (b) Directly proportional to square of effective nuclear charge (c) 1.71, 1.40, 1.36 (d) 1.71, 1.36, 1.40 (c) Inversely proportional to effective nuclear charge 58. Al 3  has a lower ionic radius than Mg 2  because (d) Inversely proportional to square of effective nuclear charge. [EAMCET 1992] 70. The correct sequence of increasing covalent character is represented (a) Mg atom has less number of neutrons than Al by [CBSE PMT 2005] (b) Al 3  has a higher nuclear charge than Mg 2  (a) LiCl  NaCl  BeCl 2 (b) BeCl 2  NaCl  LiCl (c) Their electronegativities are different (c) NaCl  LiCl  BeCl (d) BeCl 2  LiCl  NaCl (d) Al has a lower ionisation potential than Mg atom 71. Correct energy value order is [Orissa JEE 2004] 59. When a neutral atom is converted into cation, there is [EAMCET 1986] (a) ns np nd(n  1) f (b) ns np(n  1)d (n  2) f (a) Decrease in the atomic number (c) ns np(n  1)d (n  1) f (d) ns(n  1)d n(n  1) f (b) An increase in the atomic number (c) A decrease in size 72. The ionic conductance of following cation in a given concentration (d) An increase in size are in the order [Orissa JEE 2004] 60. A trend common to both groups I and VII elements in the periodic (a) Li   Na   K   Rb  table as atomic number increases is [NCERT 1981; EAMCET 1980] (b) Li   Na   K   Rb  (a) Oxidising power increases (b) Atomic radius increases (c) Li   Na   K   Rb  (c) Maximum valency increases (d) Li   Na   K   Rb  (d) Reactivity with water increases 61. Increasing order of atomic radii is [RPET 2003] (a) Mg 2  Na   Ne  F   O 2 Ionisation energy (b) Na   Mg   Ne  F   O 2 1. The incorrect statement among the following is (c) O 2  F   Ne  Na   Mg 2 [IIT-JEE 1997] 2   2 (a) The first ionisation potential of Al is less than the first (d) Ne  O  F  Na  Mg 62. Chloride ion and potassium ion are isoelectronic. Then ionisation potential of Mg [KCET 2002] (b) The second ionisation potential of Mg is greater than the (a) Potassium ion is relatively bigger second ionisation potential of Na (b) Depends on the other cation and anion (c) Their size are same (c) The first ionisation potential of Na is less than the first (d) Chloride ion is bigger than potassium ion ionisation potential of Mg 63. Which of the following has the largest ionic radius (d) The third ionisation potential of Mg is greater than the third [Pb. PMT 2002; BHU 2003] ionisation potential of Al (a) Na  (b) Ni  2. The second ionisation potential of an element M is the energy (c) Cs  (d) Mg 2 required to [JIPMER 1997] 64.    (a) The ionic radii of Li , Na , K are in which of the following order [MP PMT 2002] Remove one mole of electron from one mole of gaseous anion (b) Remove one mole of electron from one mole of gaseous cation (a) K   Na   Li  (b) K   Na   Li  of the element    (c) K  Na  Li (d) Li   Na   K  (c) Remove one mole of electron from one mole of monovalent 65. Which of the following has smallest size gaseous cation of the element [JIPMER (Med.) 2002] (d) Remove 2 moles of electrons from one mole of gaseous atoms (a) Mg 2 (b) Na  3. The ionization energy of an element is (a) The same as the electron affinity of the element (c) Al 3  (d) Si 4  (b) Equal in magnitude but of opposite sign to the electron affinity 66. Which one of the following is expected to have largest size of the element [UPSEAT 2004] (c) The energy released when an electron is added to an atom of (a) F  (b) O 2 the element (c) Al 3 (d) N 3  Chemical Periodicity 631 (d) The energy required to remove the outermost electron of an (c) Boron has only one electron in p-sub-shell atom of the element (d) Atomic size of boron is less than that of beryllium 4. The first ionisation energies of alkaline earth metals are higher than those of the alkali metals. This is because 13. A A   e, E1 and A  A 2   e, E 2. The energy required [MP PET 1996] to pull out the two electrons are E1 and E 2 respectively. The (a) There is increase in the nuclear charge of the alkaline earth correct relationship between two energy would be metals (a) E1  E 2 (b) E1  E 2 (b) There is a decrease in the nuclear charge of the alkaline earth metals (c) E1  E 2 (d) E1  E 2 (c) There is no change in the nuclear charge 14. Which of the following element has maximum, first ionisation (d) None of the above potential [AIIMS 2001] 5. The statement that is not correct for the periodic classification of (a) V (b) Ti elements is [IIT-JEE 1992] (c) Cr (d) Mn (a) The properties of elements are the periodic functions of their 15. Highest energy will be absorbed to eject out the electron in the atomic numbers configuration [RPMT 2000] (b) Non-metallic elements are lesser in number than metallic (a) 1s 2 2 s 2 2 p 1 (b) 1s 2 2 s 2 2 p 3 elements (c) The first ionisation energies along a period do not vary in a (c) 1s 2 2 s 2 2 p 2 (d) 1s 2 2 s 2 2 p 4 regular manner with increase in atomic number 16. In which of the following process highest energy is absorbed (d) For transition elements the d -sub-shells are filled with [RPET 2000] electrons monotonically with increase in atomic number (a) Cu Cu  (b) Br Br  6. Choose the correct statement (c) I I  (d) Li Li  (a) Ionization energy and electron affinity increases across a period 17. The first ionization potential of Na, Mg, Al and Si are in the order[IIT 1988; MP (b) Ionization energy increases but electron affinity decreases along a period (a) Na < Mg > Al < Si (b) Na > Mg > Al > Si (c) Na < Mg < Al > Si (d) Na > Mg > Al < Si (c) Ionization energy decreases but electron affinity increases 18. How many ionisation energies can carbon have (d) Both decreases along a period (a) 1 (b) 2 7. In halogens, with the increase of atomic number which habit is (c) 4 (d) 6 found 19. Which of the following gaseous atoms has highest value of IE (a) Habit to loose electrons decreases [JIPMER 1997; CPMT 1997; AIIMS 2000] (b) Ionic radii decreases (a) P (b) Si (c) Ionization potential decreases (c) Mg (d) Al (d) In MX 2 (M  metal and X  halogen), covalent properties 20. Hydrogen has high ionization energy than alkali metals, due to its [AIIMS 1999] decreases (a) Large size (b) Small size 8. Ionization potential is lowest for (c) Ionic bond (d) Covalent bond The first ionization potentials eV  of Be and B respectively are[CBSE PMT [CPMT 1989; MP PET 2001] 21. (a) Halogens (b) Inert gases (c) Alkaline earth metals (d) Alkali metals (a) 8.29eV , 9.32eV (b) 9.32eV , 9.32eV 9. Which of the following explanation is best for not placing hydrogen (c) 8.29eV , 8.29eV (d) 9.32eV , 8.29eV in either the group of alkali metals or halogens 22. Which ionisation potential IP  in the following equations involves [NCERT 1978] the greatest amount of energy [Pune CET 1998] (a) The ionization energy of hydrogen is to high for group of alkali (a) Na Na   e  (b) K  K 2  e  metals, but too low of halogen group (b) Hydrogen can form compounds with all other elements (c) C 2  C 3   e  (d) Ca  Ca 2   e  23. Which of the following has maximum ionization potential (c) Hydrogen is much lighter element than the alkali metals or the [MH CET 1999] halogens (a) K (b) Na (d) None of the above (c) Al (d) Mg 10. The ionization energy of nitrogen is more than that of oxygen 24. The first four ionization energy values of an element are 191, 578, because [MP PET 1993] 872 and 5962 kcal. The number of valence electrons in the element (a) Nitrogen has half filled p-orbitals is (b) Nitrogen is left to the oxygen in the same period of the (a) 1 (b) 2 periodic table (c) 3 (d) 4 (c) Nitrogen contains less number of electrons 25. Which of the following has least ionization potential (d) Nitrogen is less electronegative [CPMT 1982, 93] 11. The energy required to remove an electron of a gaseous atom from (a) Li (b) Cs its ground state is called [CPMT 1989, 94] (c) Cl (d) I (a) Potential energy (b) Ionization energy 26. Which of the following element has the lowest ionization potential [CPMT 1976; (c) Electrode potential (d) Activation energy (a) Fe (b) H 12. The first ionization energy of boron is less than that of beryllium (c) Li (d) He because 27. As one moves along a given row in the periodic table, ionization (a) Boron has higher nuclear charge energy (b) Atomic size of boron is more than that of beryllium [CPMT 1976, 89; NCERT 1978; EAMCET 1985] (a) Remains same  632 Chemical Periodicity (b) Increases from left to right (a) B (b) Li (c) First increases, then decreases (c) Ne (d) F (d) Decreases from left to right 42. The set representing the correct order of first ionisation potential is [IIT-JEE (S 28. Ionization energy is highest for [AFMC 2001; BVP 2003] (a) K  Na  Li (b) Be  Mg  Ca (a) Noble gases (b) Platinum metals (c) B  C  N (d) Ge  Si  C (c) Transition elements 43. Among the following options, the sequence of increasing first (d) Inner–transition elements ionisation potential will be 29. Which one of the following elements has the highest ionisation [AIIMS 2000; MP PMT 2002] energy [IIT-JEE 1990] (a) B  C  N (b) B  C  N (a) [ Ne ] 3 s 2 3 p 1 (b) [ Ne ] 3 s 2 3 p 2 (c) C  B  N (d) N  C  B (c) [ Ne ] 3 s 2 3 p 3 (d) [ Ar] 3d 10 4 s 2 4 p 2 44. The decreasing order of the ionisation potential in the following elements is [MP PMT 2001] 30. Which of the following elements has the lowest ionistion potential [EAMCET 1993] (a) Ne  Cl  P  S  Al  Mg (a) N (b) O (c) F (d) Ne (b) Ne  Cl  P  S  Mg  Al 31. Which of the following has lowest first ionisation potential (c) Ne  Cl  S  P  Mg  Al [CPMT 1993] (a) B (b) C (d) Ne  Cl  S  P  Al  Mg (c) N (d) O 45. Which is the correct order of the first ionization potential of N, O 32. If first orbit energy of He  is – 54.4 eV, then the second orbit and C [AMU 2000] energy will be [Roorkee 1995] (a) C  N  O (b) C  N  O (a) – 54.4 eV (b) – 13.6 eV (c) O  N  O (d) C  N ~ O (c) – 27.2 eV (d) + 27.2 eV 46. Which of the following order is wrong [CBSE 2002] 33. The screening effect of inner electrons of the nucleus causes [MP PMT 1994] (a) NH 3  PH 3  AsH 3 -acidic nature (a) A decrease in the ionisation potential (b) Li   Na   K   Cs  -ionic radius (b) An increase in the ionisation potential (c) Al2 O3  MgO  Na 2 O  K 2 O -basic (c) No effect on the ionisation potential (d) An increase in the attraction of the nucleus to the electrons (d) Li  Be  B  C -1 ionisation potential st 34. Which of the following has highest first ionization energy 47. Which of the following has the least ionization potential [MP PET 1994] [MP PET 2002] (a) Sulphur (b) Oxygen (a) Lithium (Li) (b) Helium (He) (c) Nitrogen (d) Phosphorus (c) Nitrogen (N) (d) Zinc (Zn) 35. The second ionization potential is 48. The first ionisation energy of lithium will be [Bihar CEE 1995; CET Pune 1998] [EAMCET 1990] (a) Less than the first ionization potential (a) Greater than Be (b) Less than Be (b) Equal to the first ionization potential (c) Greater than the first ionization potential (c) Equal to that of Na (d) Equal to that of F 2 (d) None of these 49. Spectrum of Li is similar to that of [AIIMS 2002] 36. When the first ionization energies are plotted against atomic (a) H (b) He number the peaks are occupied [CET Pune 1998] (c) Be (d) Ne (a) Alkali metals (b) Halogens 50. Highest ionisation energy stands for [DPMT 2000] (c) Rare gases (d) Transition elements (a) He (b) C 37. Among the following which has the hi