CLASSIFICATION OF ELEMENTS

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1 Some Basic Concepts & Classification of Elements Test No. 15 Time: 2 Hrs. Total Marks: 311 Date: 07/07/2013 Name Batch: CLASSIFICATION OF ELEMENTS Section A (Objective Question only one correct answer) (3, -1 Marks) MM: 197 Q1. Which of the following is not a chalcogen? (a) Sulphur Selenium (c) Tellurium All are chalcogens O S Se Te Po Q2. The first elements of rare earth metals is (a) Cerium Actinium (c) Uranium Lanthanum (c) Q3. Which of the following is a bridge element? (a) Be Cl (c) K P Be (Elements of 2 nd period behave bridge elements) Q4. Which pair of atomic numbers represents s-block elements? (a) 7,15 6, 12 (c) 9, 17 3, 12 S block is group I & II Li 3 Be 4 Na 11 Mg 12 K 19 Ca 20 Rb 37 Sr 38 CS 55 Ba 56 Fr 87 Ra 88 Q5. In the modern periodic table one of the following does not have appropriate position: (a) inert gases inner-transition elements (c) transition elements fluorine Lanthanides & Actinides Q6. An element with atomic number 82 belongs to group (a) (c) 14 2 (c) He 2 Ne 10 Ar 18 Kr 36 Xe Rn 86 Gp-14 gp-15 gp-16 gp-17 gp-18 S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

2 Q7. Which of the following is a transition element? (a) Al As (c) Ni Rb (c) Q8. The 14 elements have been placed in VIth period and third group of the periodic table. They are called: (a) alkaline earth metals inert gases (c) alkali metals rare earth metals Q9. Element X belongs to 4 th period. It contains 18 and 1 electron in the penultimate and ultimate orbit. The element X should be: (a) normal element transition element (c) inert gas inner transition element Q10. Element having electronic configuration 1s 2, 2s 2, 2p 6,3s 2,3p 6, 3d 1, 4s 2 belongs to group and period (a) 3,4 5, 6 (c) 4, 2 3,1 (a) pd 4 highest value of n Block = d block Group = (n 1)d + ns = = 3 Q11. From electronic configuration of elements A; 1s 2, 2s 2, 2p 6, 3s 2 B; 1s 2, 2s 2, 2p 6, 3s 1 C; 1s 2, 2s 2 D; 1s 2, 2s 2, 2p 6, 3s 2, 3p 6, 4s 2, 3d 1 Elements belong to same period (a) C, B A, B (c) C, A C, D A, B same value of n Q12. The halogens are: (a) normal elements noble elements (c) transition elements Inner transition elements (a) Q13. An element with half-filled 4p subshell belongs to group (a) (c) (a) 4p 3 4s 2 4p 3 ns 2 np 3 gp 15 Q14. In the sixth period, the orbitals being filled are (a) 5s, 5p, 5d 6s, 6p, 6d, 6f (c) 6s, 5f, 6d, 6p 6s, 4f, 5d, 6p 6s + 4f + 5d + 6p Q15. The elements with atomic numbers 21 to 30 belong to (a) halogens noble gas (c) first transition elements lanthanides (c) Q16. An element X belongs to Group 14 and 2 nd period of the periodic table. Its atomic number will be (a) 6 14 (c) (a) gp 14 C ns np S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

3 Q17. Without looking at the periodic table, select the elements of IIIA group of the periodic table (Atomic numbers are given): (a) 3, 11, 19, 37 5, 13, 21, 39 (c) 7, 15, 31, 49 5, 13, 31, 49 III A 13 B(5) Q18. Lanthanoids are Al (13) Ga (31) In (49) Tl (a) 14 elements in the sixth period (atomic no. = 90 to 103) that are filling 4f-sublevel 14 elements in the seventh period (atomic no. = 90 to 103) that are filling 5fsublevel (c) 14 elements in the sixth period (atomic no. = 58 to 71) that are filling 4f-sublevel 14 elements in the seventh period (atomic no. = 58 to 71) that are filling 4fsublevel (c) Q19. The general outer electronic configuration of transition metals is (a) ns 2 nd 1-10 ns 2 np 1 (n -1) d 1-10 (c) ns 2 np 6 (n 1) d 1-10 ns 0-2 (n -1) d 1-10 Q20. Element with valence shell electronic configuration as (n 1) d 5 ns 1 is placed in (a) IA, s-block VIA, s-block (c) VIIB, s-block VIB, d-block Q21. An element with atomic number 106 has been discovered recently. Which of the following electronic configurations will it possess? (a) [Rn] 5f 14 6d 4 7s 2 [Rn] 5f 14 6d 5 7s 1 (c) [Rn] 5f 14 6d 6 7s 0 [Rn] 5f 14 6d 1 7s 2 7p 3 (a) 106 gp-6 Q22. The elements with atomic numbers 9, 17, 35, 53, 85 are all (a) noble gases halogens (c) heavy metals light metals Q23. The ionic radii of Li +, Be 2+ and B 3+ follow the order: (a) 3 Li + < 4 Be 2+ < 5 B 3+ B 3+ < Be 2+ < Li + (c) Li + < B 3+ < Be 2+ B 3+ < Li + < Be 2+ Li + Bl 2+ B 3+ z 3 e Q24. The correct order of radii is: more e z force of attraction small radii B 3+ < Be 2+ < Li + (a) N < Be < B F - < O 2- < N 3- (c) Na < Li < K Fe 3+ < Fe 3+ < Fe 4+ same reason as Q. 23 of isoelectronic species Q25. Of the following sets which one does not contain isoelectronic species? (a) BO 3 3-, CO 3 2-, NO 3 - SO 3 2-, CO 3 2-, NO 3 - (c) CN -, N 2, C 2 2- PO 4 3-, SO 4 2-, ClO 4 - S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

4 Q26. Which one is largest in size? (a) S 2- O 2- (c) Mg 2+ (c) Na + (a) radii increases Q27. Which of the following ions has the highest value of ionic radius? (a) Li + B 3+ (c) O 2- F - Li + B 3+ O 2 F n e z e Q28. The correct order of ionic radii for the following ions is (a) N 3- < F - < O 2- < Na + Na + > F - > O 2- > N 3- (c) N 3- > O 2- > F - > Na + (c) The correct order cannot be predicted. Q29. For which of the elements of different groups, the change in nonpolar covalent radii is maximum? (a) Group 1 & 2 Groups 13 & 14 (c) Groups 14 & 15 Groups 16 & 17 (a) They are after noble gases Q30. The ions O 2-, F -, Na +, Mg 2+ and Al 3+ are isoelectronic. Their ionic radii show (a) a significant increase from O 2- to Al 3+ a significant decrease from O 2- to Al 3+ (c) an increase from O 2- to F - and then decrease from Na + to Al 3+ a decrease from O 2- to F - and then increase from Na + to Al 3+ Q31. The ionic radii of Cl -, S 2- and P 3- follow the order (a) Cl - > S 2- > P 3- Cl - < S 2- < P 3- (c) Cl - > P 3- > S 2- Cl - < P 3- < S 2- same as isoelectronic Q32. The first ionization potential of Na, Mg, Al and Si are in the order (a) Na < Mg > Al < Si Na > Mg > Al > Si (c) Na > Mg < Al > Si Na > Mg > Al < Si (a) Na Mg Al Si Exception I.E. inc Na < Al < Mg < Si Q33. Among the following elements (whose electronic configurations are given below), the one having the highest ionization energy is (a) [Ne] (3s) 2 (3p) 1 [Ne] (3s) 2 (3p) 3 (c) [Ne] (3s) 2 (3p) 2 [Ar] (3d) 10 (4s) 2 (4p) 3 (a) Al P (c) Si Ar Exception Al P Si S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

5 As Q34. In the periodic table, the ionization energy of elements (a) decreases (i) from left to right across a period and (ii) on descending a group decreases from left to right across a period and increases on descending a group (c) increases, (i) from left to right across period and (ii) on descending a group increases from left to right across a period and decreases on descending a group. Q35. The first ionization energy of K, Ca and Ba follows the order (a) K > Ca > Ba Ca > Ba > K (c) Ba > K > Ca K > Ba > Ca ns 2 K Ca Ca > Ba > K Ba Q36. If the ionization potential of Na is 5.48 ev. Potassium is expected to have a value of (a) 5.48 ev 4.34 ev (c) 5.68 ev 8.4 ev K < Na dec. Q37. The set representing the correct order of first ionization potential is (a) K > Na > Li Be > Mg > Ca (c) B > C > N Ge > Si > C Q38. The third ionization energy amongst Li, Be, B and C is lowest for (a) Li Be (c) B C Li Be B C He Li Be B H He Li Be Q39. Which represents alkalies metals based on (IE) 1 and (IE) 2 values? (IE) 1 (IE) 2 (IE) 1 (IE) 2 (a) X Y (c) Z M (c) Concept I I.E, least Concept II I.E 2 I.E, max. Q40. The first ionisation energy of sodium is 500 KJ mol -1. This denotes the energy: (a) Given out when 1 mole of sodium atoms dissolves in water to form sodium ions Required to remove one electron to infinity from one atom of sodium (c) Required to raise the electrons in one mole of gaseous sodium atoms to a higher energy level Required to change one mole of gaseous sodium atoms into gaseous ion (Na + ) definition Max I. E. Q41. First ionization energy of carbon is equal to the enthalpy change for the equation (a) C diamond C + (g) + e - C graphite C + (g) + e - (c) C (g) C + (g) + e - C + (g) C 2+ (g) + e - S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

6 (c) definition Q42. The successive ionisation energies for an element X are given below: A. 1 st IE = 410 kj/mol B. 2 nd IE = 820 kj/mol [PET Kerala 2006] C. 3 rd IE = 1100 k/mol D. 4 th IE = 1500 kj/mol E. 5 th IE = 3200 kj/mol Find out the number of valence electrons for the atom X (a) 4 3 (c) 5 2 (a) after losing 4 e 1 s it is acquiring noble gas configuration. Q43. Which of the following elements has the lowest ionisation enthalpy: (a) Na K (c) Mg Al Na Mg Al K Q44. Which of the following has the lowest ionisation enthalpy: (a) 4s 1 3d 2 (c) 3p 6 2p 6 (a) alkali metals have least I. E. Q45. The transition elements have a characteristic electronic configuration which can be represented as: (a) (n 2)s d 1-10 (n 1)s 2 p 6 ns 2 (n -2)s 2 p 6 d 1-10 (n 1)s 2 p 6 d 1 or 2 ns 1 (c) (n 1)s 2 p 6 d 10 ns 2 np 6 nd 1-10 (n 2)s 2 p 6 d 1-10 ns 1 or 2 (n -1)s 2 p 6 ns 2 Q46. The radii of F, F -, O and O 2- are in the order of: (a) O 2- > F - > F > O F - > O 2- > F > O (c) O 2- > F - > O > F O 2- > O > F - > F (c) O F O 2 > F n e 10 Q47. The first ionisation enthalpies in electron volt of nitrogen and oxygen atoms are respectively given by: (a) 14.6, , 14.6 (c) 13.6, , 14.6 (a) N > O Q48. The incorrect statement among the following is: (a) The first ionisation enthalpy of Al is less than the first ionisation enthalpy of Mg. The second ionisation enthalpy of Mg is greater than the second ionisation enthalpy of Na. (c) The first ionisation enthalpy of Na is less than the first ionisation enthalpy of Mg. The third ionisation enthalpy of Mg is greater than the third ionisation enthalpy of Al. Section B (Assertion Reason) (3, -1 Marks) (A) If A is true but R is false. (B) If A is false but R is true. S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

7 (C) If both A and R are true and R is correct explanation of A. (D) If both A and R are true but R is not the correct explanation of A. Q49. (A) Each d-block series contains ten elements. (R) The maximum capacity of d-orbitals is of ten electrons as in each series d- orbitals are gradually filled up. (c) Q50. (A) Electron affinity of oxygen is less than that of fluorine but greater than that of nitrogen. (R) Ionisation potential is as follows: N > O > F Section C (Comprehension) (3,-1 Marks) Passage-1: (Prize for this Passage) First and second ionisation energies of Mg(g) are 740 and 1450 kj mol -1. If 1g of absorbs 50 kj of energy than write the answer of the following questions. (Solution for Q. 51, 52, 53) Mg(g) No. of moles of Mg vapours present in 1g 24 1 =.0417 Energy absorbed in ionisation of.0417 mole of Mg 1 mole of Mg requires 740 kj Mg + I. E., = 740 kj/mol moles of Mg requires kj = kj to be converted to Mg + Energy left unused which will be utilized to convert Mg + to Mg 2+ Energy unused = = kj Step II Moles of Mg moles of Mg 2 formed Mg 2 I.E kj/mol 1450 kj is required for 1 mol of Mg + Mg kj is required for mole 1450 No. of moles of Mg left as Mg + = =.0285 Q51. Q1. Calculate the percentage of Mg + (a) (c) % of Mg + = % Q52. Q2. Calculate the percentage of Mg 2+ ion (a) (c) (a) % of Mg 2+ = = or % of Mg 2+ = 100 = %.0417 Q53. Q3. Calculate the moles of Mg atom: (a) (c) S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

8 (c) 1 =.0417 moles 24 Passage-2: The minimum amount of energy required to remove the most loosely bound electron from an isolated atom in the gaseous state is known as ionisation energy or first ionisation energy or ionisation enthalpy (IE 1 ) of the element. The energy required to remove the second electron from the monovalent cation is called second ionisation enthalpy (IE 2 ). Similarly, we have third, fourth. Ionisation enthalpies. The values of ionisation energy depends on a number of factors such as (i) size of the atom (ii) screening effect (iii) nuclear charge (iv) half filled and fully filled orbitals (v) shape of orbital. In a group, the ionisation energy decreases from top to bottom. In a period, the value of ionisation energy increases from left to right with breaks where atoms have somewhat stable configurations. Q54. In a period, the ionisation energy is lowest for the (a) noble gases halogens (c) alkaline earth metals alkali metals Q55. The electronic configurations of some neutral elements are given below: (A) 1s 2, 2s 2 ; (B) 1s 2, 2s 2 2p 1 ; (C) 1s 2, 2s 2 2p 4 ; (D) 1s 2, 2s 2 2p 3 which of these electronic configurations would be expected to have highest second ionisation energy (IE 2 )? (a) A B (c) C D (c) after losing 1 electron it aquires stable half filled configuration Q56. The first (IE 1 ) and second (IE 2 ) ionisation energies (kjmol -1 ) of a few elements are shown below: IE 1 IE 2 IE 1 IE 2 (A) (B) (C) (D) Which of the above elements is likely to be a noble gas? (a) A B (c) C D (a) Whose both I. E. are high Q57. In above question which of the elements is likely to be a non-metal? (a) A B (c) C D Q58. Which of the order for ionisation energy is correct? (a) Be > B > C > N > O (c) B < Be < C < N < O B < Be < C < O < N B < Be < N < C < O Exception Be > B N > O Q59. The first ionisation energy of Mg, Al, P and S follows the order: (a) Mg < Al < P < S (c) Al < Mg < S < P Al < Mg < P < S Mg < Al < S < P (c) Al < Mg < S < P same reason as above S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

9 Section D (Single Integer Answer (3, Marks) The section contains 5 questions. The answer to each of the questions is a single digit integer, ranging from 0 to 9. Q60. How many groups are occupied by p-block elements in long form of periodic table? (6) Max. occupancy of p orbital is 6 Q61. If for an element (X), the values of successive ionisation energies I 1, I 2, I 3, I 4 and I 5 are 800, 2427, 3658, 25024, kj mol -1 respectively, then the number of valence electrons present are: (3) after losing 3 e I. E 4 is very high Q62. The ionisation energy of lithium is 500 kj mol -1. The amount of energy required to convert 70 mg of lithium atoms in gaseous state into Li + ions is: (5) For 1 mole energy required is 500 kj For mole energy required is 500 = Section E (Match the following) (8 1 = 8 Marks) Q63. Column I lists the main type of elements in the periodic table. Column II mentions atomic numbers of some of the elements. Match correctly each entry in column I with those given in column II. Column I Column II (a) s-block element (p) 63 p-block element (q) 57 (c) d-block element (r) 38 f-block element (s) 50 a r b u, s (t) 48 (u) 51 c t, q d p Q64. Column I includes atomic numbers of some of the elements and column II lists the locations of these elements in the periodic table. Identify the correct choice from column II for each entry of column I Column I Column II (a) 41 (p) 6 th period Group 8 76 (q) 6 th period group 15 (c) 83 (r) 5 th period and group (s) 7 th period and group 3 b p c q S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

10 d s S.C.O. 208 II floor, Sec-36 D Chandigarh, Ph , Mb

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