Ravindra Singh Raviyodaya

1. According to the law of triads, (a) The properties of the middle element were in between those of the other two members (b) Three elements arranged according to increasing weights have similar properties (c) The elements can be grouped in the groups of six elements (d) Every third element resembles the first element in periodic table. 2. Law of octaves stated, (a) Every eighth element had properties similar to the first element (b) Every third element had properties similar to the first element (c) The properties of the middle element were in between the other two members (d) The properties of the element were repeated after regular intervals of 3,4 or 8 elements. 3. The periodic table of today owes its development to two chemists namely (a) Rutherford and Moseley (b) Alexander Newlands and Dobereiner (c) Dmitri Mendeleev and Lothar Meyer (d) de Broglie and Neil Bohr. 4. The first periodic law stated by Mendeleev was (a) There is no correlation in the properties and atomic weights of the element (b) The properties of the elements are a periodic function of their atomic numbers (c) The properties of the elements are a periodic function of their atomic weights (d) The properties of the elements are a periodic function of their empirical formula. 5. Which of the following is not a merit of Mendeleev’s periodic table ? (a) It helped in correcting the atomic masses of some of the elements (b) He predicted the properties of some undiscovered elements and left gaps for them (c) He framed the periodic table with vertical and horizontal columns and gave shape to it (d) He gave separate places to isotopes in his periodic table. 6. What were the main demerits of Mendeleev’s periodic table ? (i) Hydrogen has been placed in group I through it resembled to group VII as well (ii) Position of some elements was not justified (iii) Isotopes were not given separate places (iv) Lanthanides and actinides were not included in the table. (a) (i), (ii) and (iii) (b) (i), (ii), (iii) and (iv) (c) (ii) and (iv) (d) (i), (iii) and (iv) 7. In the long form of periodic table, elements are arranged in the increasing order of (a) Atomic mass (b) Atomic number (c) Mass number (d) Metallic character. 8. The periodic to which an element belongs to in the long form of periodic table represents (a) Atomic mass (b) Atomic number (c) Principal quantum number (d) Azimuthal quantum number 9. Elements belonging to the same group of periodic table have (a) Same number of energy levels (b) Same number of valence electrons (c) Same number of electrons (d) Same ionization enthalpy. 10. What is the name and symbol of the element with atomic number 112 ? (a) Ununbium, Uub (b) Unnilbium, Unb (c) Ununnillum, Uun (d) Ununtrium, Uut 11. An element with atomic number 117 is known as (a) Nihonium (b) Flerovium (c) Tennessine (d) Roentgenium 12. Meitnerium is IUPAC official name of an element with atomic number (a) 113 (b) 118 (c) 104 (d) 109 13. Anything that influences the valence electrons will affect the chemistry of the element. Which one of the following factors does not affect the valence shell ? (a) Valence principal quantum number (n) (b) Nuclear charge (Z) (c) Nuclear mass (d) Number of core electrons 14. Which of the following element shown as pairs with their atomic numbers belong to the same period ? (a) Z = 19 and Z = 38 (b) Z = 12 and Z = 17 (c) Z = 11 and Z = 21 (d) Z = 16 and Z = 35 15. Match the atomic numbers of the elements given in column I with the periods given un column II and mark the appropriate choice. Column I (atomic number) Column II (period) (A) 31 (i) 5 (B) 50 (ii) 3 (C) 56 (iii) 4 (D) 14 (iv) 6 (a) (A) = (i), (B) = (ii), (C) = (iii), (D) = (iv) (b) (A) = (ii), (B) = (i), (C) = (iv), (D) = (iii) (c) (A) = (iii), (B) = (iv), (C) = (i), (D) = (ii) (d) (A) = (iii), (B) = (i), (C) = (iv), (D) = (ii) 16. To which group, an element with atomic number 88 will belong ? (a) Group 12 (b) Group 17 (c) Group 10 (d) Group 2 17. Match the following Column I Column II (A) 3d-transition series (i) Z = 58 to Z = 71 (B) Lanthanoid series (ii) Z = 39 to Z = 48 (C) Actinoid series (iii) Z = 21 to Z = 30 (D) 4d-transition series (iv) Z = 90 to Z = 103 (a) (A) = (i), (B) = (ii), (C) = (iii), (D) = (iv) (b) (A) = (ii), (B) = (iii), (C) = (iv), (D) = (i) (c) (A) = (iii), (B) = (i), (C) = (iv), (D) = (ii) (d) (A) = (iv), (B) = (iii), (C) = (i), (D) = (ii) 18. An element has atomic number 79, Predict the group and period in which the element is placed (a) 2nd group, 7th period (b) 11th group, 6th period (c) 13th group, 6th period (d) 12th group, 6th period 19. Match the following Column I (atomic number) Column II (period, group) (A) 14 (i) 3, 14 (B) 53 (ii) 5, 2 (C) 38 (iii) 6, 10 (D) 78 (iv) 5, 17 (a) (A) = (ii), (B) = (iv), (C) = (iii), (D) = (i) (b) (A) = (i), (B) = (iv), (C) = (ii), (D) = (iii) (c) (A) = (iii), (B) = (ii), (C) = (i), (D) = (iv) (d) (A) = (ii), (B) = (i), (C) = (iii), (D) = (iv) 20. Which of the following statement is correct ? (a) Elements of 3d and 4d series are kept separately in periodic table (b) Elements of 4f and 5f series are kept separately in periodic table (c) Elements of 5p and 6p series are kept separately in periodic table (d) All statements are correct. 21. An element X belongs to fourth period and fifteenth group of the periodic table. Which one of the following is true regarding the outer electronic configuration of X ? (a) It has partially filled d-orbitals and completely filled s-orbitals (b) It has completely filled s-orbitals and completely filled p-orbitals (c) It has completely filled s-orbitals and half-filled p-orbitals (d) It has half-filled d-orbitals and completely filled s-orbitals. 22. Match the following Atomic number Block (A)62 (i)d-block (B)47 (ii)p-block (C)56 (iii)f-block (D)53 (iv)s-block (a) (A) = (iii), (B) = (i), (C) = (iv), (D) = (ii) (b) (A) = (i), (B) = (ii), (C) = (iii), (D) = (iv) (c) (A) = (ii), (B) = (iv), (C) = (i), (D) = (iii) (d) (A) = (iv), (B) = (i), (C) = (ii), (D) = (iii) 23. Atomic numbers of few elements are given below. Which of the pair belongs to s-block ? (a) 7, 14 (b) 3, 20 (c) 8, 15 (d) 9, 17 24. Which of the following have the same number of electrons in outermost shell ? (a) Elements with atomic numbers 30, 48, 80 (b) Elements with atomic numbers 14,15,16 (c) Elements with atomic numbers 20,30,50 (d) Elements with atomic numbers 10,18,26 25. An element has the electronic configuration 1s2 2s2 2p4 3s2 3p4 3d4 4s2 What will be its position in the periodic table ? (a) Period 4, Group 10 (b) Period 2, Group 2 (c) Period 4, Group 2 (d) Period 2, Group 8 26. There are _____ groups and ______ periods in the extended form of periodic table. The group, all members of which are in gaseous state under ordinary conditions is _______ group. Most electropositive elements belong to _________ group. (a) 16, 8, 17, 2 (b) 18, 7, 18, 1 (c) 8, 7, 0, 2 (d) 16, 8, 18, 1 27. Which block of the periodic table contains elements with the general electronic configuration (n-2) f1-14 (n-1) d0-1 ns2 ? (a) S-block (b) P-block (c) D-block (d) F-block 28. Examples of elements belonging to s, p, d of f-block are given below. Identify the wrong example. (a) S-block element - Caesium (b) P-block element - Barium (c) D-block element – Chromium (d) F-block element – Thorium 29. Electronic configuration of few elements are given below. Mark the incorrect match. (a) 1s2 2s2 2p5 = most electronegative element (b) 1s2 2s2 2p3 = an element belonging to 3rd period and 5th group (c) 1s2 2s2 2p4 3s2 3p6 3d4 4s2 = a d-block element (d) 1s2 2s2 2p6 3s2 3p6 = an element from 18th group 30. Few general names are given along with their valence shell configurations. Mark the incorrect name. (a) ns2 np6 = Noble gas (b) ns2 np5 = Halogens (c) ns1 = Alkali metals (d) ns2 np2 = Chalcogens 31. electronic configuration of four elements is given below. Which of the following does not belong to the same group ? (a) [Kr] 4d10 5s2 (b) [Ar] 3d10 4s2 (c) [Xe] 5p6 6s2 (d) [Xe] 4f17 5d10 6s2 32. There are two rows of inner transition elements in the periodic table each containing 14 elements. The reason for this may be (a) F-orbital has seven values for magnetic quantum number, hence total electronics are 14 (b) In the periodic table there is space to accommodate 14 electrons only (c) Only 28 inner transition elements have been discovered till date (d) 28 is the maximum number of elements that any block can accommodate. 33. Which of the following ions contain minimum number of unpaired electrons ? (a) Fe2+ (b) Fe3+ (c) Co2+ (d) Co3+ 34. In the long form of periodic table, the non-metals are placed in (a) S-block (b) P-block (c) D-block (d) F-block 35. The electronic configuration of few elements is given below. mark the statement which is not correct about these elements. (i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p5 (iii) 1s2 2s2 2p6 (iv) 1s2 2s2 2p3 (a) (i) is an alkali metal (b) (iii) is a noble metal (c) (i) and (iv) form ionic compounds (d) (iv) has high ionization enthalpy. 36. Match the following Column I Column II Column III (A) bromine (i) Noble gas (p) amalgam (B) gold (ii) crystalline non metal (q) 4s2 4p5 (C) mercury (iii) liquid non metal (r) transition metal (D) iodine (iv) Liquid metal (s) violet (a) A = iii, q; B = i, r; C = iv, p; D = ii, s (b) A = ii, p; B = i, s; C = iii, q; D = iv, r (c) A = i, s; B = ii, p; C = iv, r; D = iii, q (d) A = iv, r; B = iii, q; C = ii, s; D = i, p 37. Which of the following is not correct statement for periodic classification of elements ? (a) The properties of elements are the periodic functions of their atomic number (b) Non metallic elements are less in number than metallic elements (c) For transition elements, the last electron enters into (n-2) d-subshell (d) None of these. 38. Indicate the wrong statement on the basis of the periodic table. (a) The most electronegative element in the periodic table is fluorine (b) Scandium is the first transition element and belongs to fourth period (c) There are three transition series in the periodic table each containing 10 elements (d) Along a period halogens have maximum negative electron gain enthalpy. 39. Which is the most non metallic element among the following ? (a) 1s2 2s2 2p6 3s1 (b) 1s2 2s2 2p5 (c) 1s2 2s2 2p6 3s2 (d) 1s2 2s2 2p3 40. Which of the following groups contains metals, non metals and metalloids ? (a) Group 17 (b) Group 14 (c) Group 13 (d) Group 12 41. Few values are given in the table in the direction from left to right and top to bottom. Predict the property which could be depicted in the table. 152 - 231 244 262 (a) Atomic number (b) Ionization enthalpy (c) Atomic radius (d) Electron gain enthalpy 42. Which of the following statement regarding the variation of atomic radii in the periodic table is not true ? (a) In a group, there is continuous increase in size with increase in atomic number. (b) In 4f-series, there is a continuous decrease in size with increase in atomic number. (c) The size of inert gases is larger than halogens. (d) In 3rd period, the size of atoms increases with increase in atomic number. 43. Ionic radius in a group while moving down (a) Remains same from top to bottom (b) Decreases from top to bottom (c) Increases from top to bottom (d) First increase and then decreases. 44. K+ and Cl- ions are isoelectronic. Which of the statements is not correct ? (a) Both K+ and Cl- ions contains 18 electrons (b) Both K+ and Cl- ions have same configuration (c) K+ ion is bigger than Cl- ion in ionic size (d) Cl- ion is bigger than K+ ion in size 45. Which of the following transitions will involve maximum amount of energy ? (a) M = M+ + e- (b) M- = M+ + 2e- (c) M2+ = M3+ + e- (d) M+ = M2+ + e- 46. What is the order of successive ionization enthalpies ? (a) IEIII > IEII > IEI (b) IEI > IEII > IEIII (c) IEII > IEI > IEIII (d) IEIII > IEI > IEII 47. Which group of elements show lowest ionisation enthalpy ? (a) Alkali metals (b) Alkaline earth metals (c) Halogens (d) Noble gases 48. The first ionization enthalpy of the elements are in the order of (a) C Sb > As > P > N (b) Bi < Sb < As < P < N (c) N < P < Sb < Bi < As (d) Bi > Sb~ N ~ P > As 62. Which of the following will have lowest electron affinity ? (a) Nitrogen (b) Oxygen (c) Argon (d) Boron 63. Which of the following arrangements represents the correct order of electron gain enthalpy ? (a) O < S < F < Cl (b) Cl < F < S < O (c) S < O < Cl < F (d) F < Cl < O < S 64. Which of the following statements is not correct about the electron gain enthalpy ? (a) In general, the electron gain enthalpy becomes less negative in going from top to bottom in a group (b) The electron gain enthalpy becomes less negative in a period from left to right (c) The elements having stable configuration like noble gases have large positive electron gain enthalpies (d) Electron gain enthalpy of O or F is less than that of succeeding element. 65. Why is the electron gain enthalpy of O of F less than that of S or Cl ? (a) O and F are more electronegative than S and Cl (b) When an electron is added to O or F, it goes to a smaller (n=2) level and suffers more repulsion than the electron in S or Cl in large level (n=3) (c) Adding an electron to 3p-orbital leads to more repulsion than 2p-orbital (d) Electron gain enthalpy depends upon the electron affinity of the atom. 66. Which of the following statements regarding an anion is not true ? (a) The gain of an electron leads to the formation of an anion (b) The radius of the anion is larger than the atomic radius of its parent atom (c) The effective nuclear charge increases when an anion is formed (d) Electron cloud expands due to increased repulsion among the electrons. 67. Which of the properties of isotopes of an element is different ? (a) First ionization enthalpy (b) Effective nuclear charge (c) Electron affinity (d) Melting point and boiling point 68. Given the below are the names of few elements based on their position in the periodic table. Identify the element which is not correctly placed. (a) An element which tends to lose three electrons – aluminium (b) An element which tends to gain two electrons – iodine (c) An element with valency four – silicon (d) A transuranium element – plutonium 69. Why do noble gases have positive electron gain enthalpy ? (a) It is difficult to add an electron due to small size (b) It is difficult to add an electron due to high electronegativity (c) It is difficult to add an electron due to stable configuration (d) It is difficult to add an electron due to high electron affinity. 70. As we move from left to right, the electronegative has (a) Large size (b) Low electron affinity (c) High ionisation enthalpy (d) Low chemical reactivity 71. Which of the following is not a periodic property for the elements ? (a) Electronegativity (b) Atomic size (c) Occurrence in nature (d) Ionization energy 72. Fill in the blanks with appropriate option. The ability of an atom to attract shared electrons to itself is called ____ (i). it is generally measured on the ____(ii) scale. An arbitrary value of____(iii) is assigned to fluorine (have greatest ability to attract electrons). It generally ____(iv) across a period and ____(v) down a group. i ii iii iv v a polarity pauling 2.0 decreases increases b Electro-negativity pauling 4.0 increases decreases c valency mulliken 1.0 decreases increases d Electron affinity mullliken 2.0 increases decreases 73. In which of the following, the order is not in accordance with the property mentioned. (a) Li < Na < K < Rb – Atomic radius (b) F > N > O > C – Ionisation enthalpy (c) Si < P < S < Cl – Electronegativity (d) F < Cl < Br < I – Electronegativity 74. Choose the incorrect statement. (a) Chemical reactivity tends to be high in group I metals, lower in elements in middle and increase to maximum in the group 17. (b) Halogens have very high negative electron gain enthalpy (c) Noble gases have large positive electron gain enthalpy (d) Decrease in electronegativities across a period is accompanied by an increase in non-metallic properties. 75. In the periodic table, the maximum chemical reactivity is at the extreme left (alkali metals) and extreme right (halogens). Which properties of these two groups are responsible for this ? (a) Least ionization enthalpy on the left and highest negative electron gain enthalpy on the right (b) Non-metallic character on the left and metallic character on the right. (c) High atomic radii on the left and small atomic radii on the right (d) Highest electronegativity on the left and least electronegativity on the right. 76. An element X has atomic number 19, what will be the formula of its oxide ? (a) X2O (b) XO (c) XO2 (d) X2O3 77. An element P has atomic number 56. What will be the formula of its halide ? (a) PX (b) PX2 (c) PX3 (d) P2X3 78. Predict the formula of stable compound formed by an element with atomic number 114 and fluorine. (a) AF3 (b) AF2 (c) AF (d) AF4 79. Predict the formula of a compound formed by aluminium and sulphur. (a) Al2S2 (b) Al3S3 (c) Al2S3 (d) AlS 80. There are many elements in the periodic table which exhibit variable valency. This is a particular characteristic of (a) Representative elements (b) Transition elements (c) Noble gases (d) Non-metals 81. Predict the formulae of the binary compounds formed by combination of the following pairs of elements: (i) Magnesium and nitrogen (ii) Silicon and oxygen (a) MgN2, SiO2 (b) Mg3N2, SiO2 (c) Mg2N3, Si2O3 (d) MgN, SiO2 82. The first element of the groups 1 and 2 are different from other members of the respective groups. Their behaviour is more similar to the second element of the following groups. What is this relationship known as ? (a) Anomalous relationship (b) Periodic relationship (c) Diagonal relationship (d) Chemical relationship 83. The oxidation state of an element in a particular compound can be defined as (a) The charge acquired by its atom on the basis of electronegative consideration from other atoms in the molecule (b) The residual charge acquired by it s-atom after removing all electronegative atoms from the molecule (c) The valency of the most electronegative atom present in the molecule (d) Total number of electrons accepted by an atom to form a molecule. 84. Which of the following statements is true about the variation of density of elements in the periodic table ? (a) In a period from left to right density first increases upto the middle and then starts decreasing. (b) In a group on moving down the density decreases from top to bottom (c) A less closely packed solid has higher density. (d) Density of elements is not a periodic property. 85. The main reason for showing anomalous properties of the first member of a group in s or p-block is (a) Maximum chemical reactivity (b) Maximum electronegativity and different configurations (c) Small size, large charge / radius ratio (d) Tendency to form multiple bonds. 86. When we go from left to right in a period, (a) The basic nature of the oxides increases (b) The basic nature of the oxides decreases (c) There is no regular trend in the nature of oxide (d) Oxides of only first two groups are basic in nature. 87. Which of the following oxides is neutral in nature ? (a) SrO (b) Al2O3 (c) CO2 (d) CO 88. What is the common property of the oxides CO, NO, N2O ? (a) All are acidic oxides (b) All are basic oxides (c) All are neutral oxides (d) All are amphoteric oxides 89. The correct order of acidic character of oxides in third period of periodic table is (a) SiO2< P4O10 p > d > f (b) f > d > p > s (c) p < d < s > f (d) f > p > s > d 99. the first ionization enthalpies of Na, Mg, Al and Si are in the order (a) NaAlMg>Al>Si (c) NaMg>Al