INORGANIC CHEMISTRY
CLASS-XI
PERIODIC PROPERTIES
CONTENTS
EXERCISE-I.................................................. 2 - 6
EXERCISE-II ................................................ 7 - 8
EXERCISE-III ............................................. 9 - 26
EXERCISE-IV ........................................... 27 - 28
ANSWER KEY ........................................... 29 - 30
EXERCISE-II
1. The element with atomic number 57 belongs to :
(1) s-block (2) p-block (3) d-block (4) f-block
2. Element in periodic table with electronic configuration as [18Ar] 3d5 4s1 is placed in :
(1) 1st group, s-block (2) 2nd group, s-block
(3) 5th group, d-block (4) 6th group, d-block
3. Choose the incorrect option for the order of atomic radius :
(1) Au Ag < Cu (2) Li < Ne , Na < Ar
(3) O2– > O– >O> O+ (4) Sc < Y < La
4. Values of IE1, IE2 and IE3 of an element are 9.32, 18.21 and 553.83 eV. What informations do these data
convey ?
(1) The element has two electrons in the valence shell.
(2) The element has two p-electrons in the valence shell.
(3) (1) and (2) both.
(4) None of the two.
5. Which of the following order is correct
(1) S2– < Cl– < K+ : order of size (2) K < Na < Mg < Ne : order of ionisation energy
(3) Mg < Al < Si : order ionisation energy (4) Mg2+ < Al3+ < Na+ : order of size
6. The correct order of increasing atomic radius of the following elements is :
(1) S < O < Se < C (2) O < C < S < Se (3) O < S < Se < C (4) C < O < S < Se
7. Amongst the following elements, the highest ionisation energy is :
(1) [Ne] 3s2 3p1 (2) [Ne] 3s2 3p4 (3) [Ne] 3s2 3p3 (4) [Ne] 3s2 3p5
8. Which of the following statements are correct ?
(a) HF is a stronger acid than HCl.
(b) among halide ions, iodide is the most powerful reducing agent.
(c) Fluorine is the only halogen that does not show a variable oxidation state.
(d) HOCl is a stronger acid than HOBr.
(1) b and d (2) b and c (3) a, b and c (4) b, c, and d
9. If the same element is forming oxides in different oxidation states then :
(1) that oxide will be neutral in nature in which element will be in its highest oxidation state.
(2) that oxide will be highest acidic in nature in which element will be in its highest oxidation state.
(3) that oxide will be amphoteric in nature in which element will be in its highest oxidation state.
(4) that oxide will be highly basic in nature in which element will be in its highest oxidation state.
10. Elements with atomic number 58 to 71 are placed in :
(1) 5th period and 4th group (2) 6th period and 3th group
(3) 7th period and 3th group (4) 6th period and 4th group
[7]
11. Which of the following is not concerned to effective nuclear charge?
(1) Higher ionization potential of carbon than boron
(2) Higher ionization potential of magnesium than aluminium
(3) Higher values of successive ionization energy
(4) Higher electronegativity of Mn7+ than Mn4+
12. Which one of the following oxide have highest acidic character ?
(1) CO2 (2) ClO2 (3) SiO2 (4) SO2
13. Which is a true statement ?
(1) Larger is the value of ionisation energy easier is the formation of cation.
(2) Larger is the value of electron affinity easier is the formation of anion.
(3) Larger is the value of ionisation energy as well as electron affinity the smaller is the electronegativity of atom.
(4) Larger is the Zeff larger is the size of atom.
14. Electron gain enthalpy will be positive in
(1) O2– is formed from O–1 (2) O1– is formed from O
(3) S–1 is formed from S (4) Na– is formed from Na
15. The element which has highest electron affinity ?
(1) Oxygen (2) Sulphur (3) Nitrogen (4) Phosphorus
16. An atom with high electronegativity generally has a
(1) Low electron affinity (2) Small atomic number
(3) Large atomic radius (4) High ionisation potential
17. For electron affinity of halogens which of the following is correct ?
(1) Br > F (2) F > Cl (3) Br < Cl (4) F < l
18. The correct order of negative electron gain enthalpy is :
(1) Be < B < C < N (2) Be < N < B < C (3) N < Be < C < B (4) N < C < B < Be
19. Increasing order of second ionization enrgy is
(1) Ne < O < F < N < B < C < Be (2) Be < C < B < N < F < O < Ne
(3) Be < B < C < N < F < O < Ne (4) B < C < N < O < F < Be < Ne
20. The first ionisation potentials of Na, Mg, Al and Si are in the order
(1) Na < Mg > Al < Si (2) Na < Mg < Al > Si (3) Na > Mg > Al > Si (4) Na > Mg > Al < Si
21. Which of the following is wrong -
(1) NH3 < PH3 < AsH3 Acidic character
(2) Li < Be < B < C IE1
(3) Al2O 3 < MgO < Na2O < K2O Basic character
(4) Li+ < Na+ < K+ < Cs+ Ionic radius
22. Which of the following is correct order of increasing bond strength -
(1) HF < HCl < HBr < HI (2) HI < HBr < HF < HCl
(3) HI < HBr < HCl < HF (4) HCl < HBr < HF < HI
23. Density of sodium and potassium follows the order -
(1) K < Na (2) K > Na (3) Na K (4) None of these
24. The size of the species, Pb, Pb2+, Pb4+ decreases as -
(1) Pb4+ > Pb2+ > Pb (2) Pb > Pb2+ > Pb4+ (3) Pb > Pb4+ > Pb2+ (4) Pb4+ > Pb > Pb2+
[8]
EXERCISE-III
(Question asked in previous AIEEE/JEE-MAIN)
1. Which one of the following sets of ions represents a collection of isoelectronic species ? [AIEEE-2006]
(1) K+ , Cl–, Ca2+, Sc3+ (2) Ba2+, Sr2+, K+, S2–
(3) N3–, O2–, F–, S2– (4) Li+, Na+, Mg2+, Ca2+
2. The increasing order of the first ionization enthalpies of the elements B, P, S and F (lowest first) is
[AIEEE-2006]
(1) F < S < P < B (2) P < S < B < F (3) B < P < S < F (4) B < S < P < F
3. The charge/size ratio of a cation determines its polarizing power. When one of the following sequences
represents the increasing order of the polarizing order of the polarizing power of the catonic species, K+,
Ca2+, Mg2+, Be2+ ? [AIEEE-2007]
(1) Mg2+, Be2+, K+ , Ca2+ (2) Be2+, K+, Ca2+, Mg2+
(3) K+, Ca2+, Mg2+, Be2+ (4) Ca2+, Mg2+, Be2+, K+
4. In which of the following arrangements, the sequence is not strictly according to the property written against it ?
(1) NH3 < PH3 < As H3 < SbH3 : increasing basic strength [AIEEE-2009]
(2) B < C < O < N : increasing first ionization enthalpy
(3) CO2 < SiO2 < SnO2 < PbO2 : increasing oxidising power
(4) HF < HC < HBr < HI : increasing acid strength
5. The set representing the correct order of ionic radius is : [AIEEE-2009]
(1) Li+ > Na+ > Mg2+ > Be2+ (2) Mg2+ > Be2+ > Li+ > Na+
(3) Li+ > Be2+ > Na+ > Mg2+ (4) Na+ > Li+ > Mg2+ > Be2+
6. The correct sequence which shows decreasing order of the ionic radii of the elements is [AIEEE-2010]
(1) Na+ > F– > Mg2+ > O2– > Al3+ (2) O2– > F– > Na+ > Mg2+ > Al3+
(3) Al3+ > Mg2+ > Na+ > F– > O2– (4) Na+ > Mg2+ > Al3+ > O2– > F–
7. Which one of the following orders presents the correct sequence of the increasing basic nature of the given
oxides ? [AIEEE-2011]
(1) Al2O3 < MgO < Na2O < K2O (2) MgO < K2O < Al2O3 < Na2O
(3) Na2O < K2O < MgO < Al2O3 (4) K2O < Na2O < Al2O3 < MgO
8. The outer electron configuration of Gd (Atomic No : 64) is : [AIEEE-2011]
(1) 4f 3 5d5 6s2 (2) 4f 8 5d0 6s2 (3) 4f 4 5d4 6s2 (4) 4f 7 5d1 6s2
9. The increasing order of the ionic radii of the given isoelectronic species is : [AIEEE-2012]
(1) Cl–, Ca2+, K+, S2– (2) S2–, Cl– , Ca2+ , K+ (3) Ca2+, K+, Cl–, S2– (4) K+, S2–, Ca2+, Cl–1
10. Which among the following elements has the highest first ionization enthalpy?
[JEE Main Online-2012]
(1) Nitrogen (2) Boron (3) Carbon (4) Oxygen
[9]
11. Which of the following presents the correct order of second ionization enthalpies of C, N, O and F ?
[JEE Main Online-2012]
(1) F > O > N > C (2) O > N > F > C (3) C > N > O > F (4) O > F > N > C
12. Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se
and Ar ? [IIT-JEE Mains-2013]
(1) Ca < Ba < S < Se < Ar (2) Ca < S < Ba < Se < Ar
(3) S < Se < Ca < Ba < Ar (4) Ba < Ca < Se < S < Ar
13. Electron gain enthalpy with negative sign of fluorine is less than that of chlorine due to
[JEE Main Online-2013]
(1) Bigger size of 2p orbital of fluorine (2) High ionization enthalpy of fluorine
(3) Smaller size of fluorine atom (4) Smaller size of chlorine atom
14. Given [JEE Main Online-2013]
Reaction Energy Change (in kJ)
Li (s) Li (g) 161
Li (g) Li+ (g) 520
½ F2(g) F (g) 77
F (g) + e– F– (g) (Electron gain enthalpy)
Li+ (g) + F– (g) Li F (s) –1047
Li (s) + ½ F2 (g) Li F (s) –617
Based on data provided, the value of electron gain enthalpy of fluorine would be
(1) –228 kJ mol–1 (2) –300 kJ mol–1 (3) –350 kJ mol–1 (4) –328 kJ mol–1
15. The order of increasing sizes of atomic radii among the elements O, S, Se and As is
[JEE Main Online-2013]
(1) O < S < Se < As (2) As < S < O < Se (3) O < S < As < Se (4) Se < S < As < O
16. Which is the correct oder of second ionization potential of C, N, O and F in the following?
[JEE Main Online-2013]
(1) O > N > F > C (2) C > N > O > F (3) F > O > N > C (4) O > F > N > C
17. Which of the following series correctly represents relations between the elements from X to Y ?
XY [JEE Main Online-2014]
(1) 3Li 19K Ionization enthalpy increases.
(2) 9F 35Br Electron gain enthalpy with negative sign increases.
(3) 6C 32Ge Atomic radii increases.
(4) 18Ar 54Xe Noble character increases
18. Similarity in chemical properties of the atoms of elements in a group of the Periodic table is most closely
related to : [JEE Main Online-2014]
(1) Atomic numbers (2) Atomic masses
(3) Number of principal energy levels (4) Number of valence electrons
19. Which of the following arrangements represents the increasing order (smallest to largest) of ionic radii of the
given species [JEE Main Online-2014]
2– 2– 3–
O ,S ,N ,P ? 3–
(1) O2– < N3– < S2– < P3– (2) O2– < P3– < N3– < S2–
(3) N3– < O2– < P3– < S2– (4) N3– < S2– < O2– < P3–
[10]
20. Which one of the following has largest ionic radius ? [JEE Main Online-2014]
(1) Li+ (2) O2– (3) B3+ (4) F–
21. In the long form of the periodic table, the valence shell electronic configuration of 5s25p4 corresponds to the
element present in [JEE Main Online-2015]
(1) Group 16 and period 6 (2) Group 17 and period 5
(3) Group 16 and period 5 (4) Group 17 and period 6
22. The ionic radii (in Å) of N3–, O2– and F– are respectively [IIT-JEE Mains-2015]
(1) 1.71, 1.36 and 1.40 (2) 1.36, 1.40 and 1.71
(3) 1.36, 1.71 and 1.40 (4) 1.71, 1.40 and 1.36
23. Which of the following atoms has the highest first ionization energy ? [IIT-JEE Mains-2016]
(1) Rb (2) Na (3) K (4) Sc
24. Consider the following ionization enthalpies of two elements ‘A’ and ‘B’. [JEE Main Online-2017]
Element Ionization enthalpy (kJ/mol)
1st 2nd 3rd
A 899 1757 14847
B 737 1450 7731
Which of the following statements is correct ?
(1) Both ‘A’ and ‘B’ belong to group-1 where ‘B’ comes below ‘A’.
(2) Both ‘A’ and ‘B’ belong to group-2 where ‘B’ comes below ‘A’.
(3) Both ‘A’ and ‘B’ belong to group-1 where ‘A’ comes below ‘B’.
(4) Both ‘A’ and ‘B’ belong to group-2n where ‘A’ comes below ‘B’.
25. The electronic configuration with the highest ionization enthalpy is : [JEE Main Online-2017]
(1) [Ne] 3s2 3p1 (2) [Ne] 3s2 3p2
(3) [Ne] 3s2 3p3 (4) [Ar] 3d10 4s2 4p3
26. The group having isoelectronic species is [IIT-JEE Mains-2017]
(1) O–, F–, Na+, Mg2+ (2) O2–, F–, Na+, Mg2+ (3) O–, F–, Na, Mg2+ (4) O2–, F–, Na, Mg2+
27. For Na+, Mg2+, F– and O2– ; the correct order of increasing ionic radii is : [JEE Main Online-2018]
(1) O2– < F– < Na+ < Mg2+ (2) Na+ < Mg2+ < F– < O2–
(3) Mg2+ < Na+ < F– < O2– (4) Mg2+ < O2– < Na+ < F–
28. The correct order of spin-only magnetic moments among the following is : [JEE Main Online-2018]
(Atomic number : Mn = 25, Co = 27, Ni = 28, Zn = 30)
(1) [ZnCl4]2– > [NiCl4]2– > [CoCl4]2– > [MnCl4]2– (2) [CoCl4]2– > [MnCl4]2– > [NiCl4]2– > [ZnCl4]2–
2– 2– 2–
(3) [NiCl4] > [CoCl4] > [MnCl4] > [ZnCl4] 2– (4) [MnCl4]2– > [CoCl4]2– > [NiCl4]2– > [ZnCl4]2–
29. The correct order of electron affinity is : [JEE Main Online-2018]
(1) F > Cl > O (2) F > O > Cl (3) Cl > F > O (4) O > F > Cl
30. In general, the properties that decrease and increase down a group in the periodic table, respectively, are
(1) electron gain enthalpy and electronegativity [JEE-Main-Online 2019]
(2) electronegativity and atomic radius
(3) electronegativity and electron gain enthalpy
(4) atomic radius and electronegativity
[11]
EXERCISE-IV
(Question asked in previous IIT-JEE)
1. Moving from right to left in a periodic table, the atomic size is : [JEE 1995]
(1) increased (2) decreased
(3) remains constant (4) none of these
2. The increasing order of electronegativity in the following elements : [JEE 1995]
(1) C, N, Si, P (2) N, Si, C, P (3) Si, P, C, N (4) P, Si, N, C
3. One element has atomic weight 39. Its electronic configuration is 1s2, 2s2 2p6, 3s2 3p6 4s1. The true statement
for that element is : [JEE 1995]
(1) High value of IE (2) Transition element (3) Isotone with 18Ar38 (4) None
4. The number of paired electrons in oxygen is : [JEE 1995]
(1) 6 (2) 16 (3) 8 (4) 32
5. The decreasing size of K+, Ca2+, Cl– & S2– follows the order : [JEE 1995]
(1) K+ > Ca+2 > S–2 > Cl– (2) K+ > Ca+2 > Cl– > S–2
(3) Ca+2 > K+ > Cl– > S–2 (4) S–2 > Cl– > K+ > Ca+2
6. Which of the following oxide is neutral ? [JEE 1996]
(1) CO (2) SnO2 (3) ZnO (4) SiO2
7. Which of the following has the maximum number of unpaired electrons [JEE 1996]
(1) Mg2+ (2) Ti3+ (3) V3+ (4) Fe2+
8. The following acids have been arranged in the order of decreasing acid strength. Identify the correct order
ClOH(I) BrOH(II) IOH(III) [JEE 1996]
(1) I > II > III (2) II > I > III (3) III > II > I (4) I > III > II
9. The incorrect statement among the following is : [JEE 1997]
(1) the first ionisation potential of Al is less that the first ionisation potential of Mg
(2) the second ionisation potential of Mg is greater that the second ionisation potential of Na
(3) the first ionisation potential of Na is less than the first ionisation potential of Mg
(4) the third ionisation potential of Mg is greater than the third ionisation potential of Al
10. Assertion : F atom has a less negative electron gain enthalpy that Cl atom. [JEE 2000]
Reason : Additional electron is repelled more efficiently by 3p electron in Cl atom than by 2p electron in F
atom.
(1) If both assertion and reason are CORRECT, but reason is the CORRECT explanation of the assertion.
(2) If both assertion and reason are CORRECT, but reason is not the CORRECT explanation of the assertion.
(3) If asserton if CORRECT but reason in INCORRECT
(4) If assertion is INCORRECT reason in CORRECT.
[27]
11. Assertion : Al(OH)3 is amphoteric in nature. [JEE 2000]
Reason : Al –O and O – H bonds can be broken with equal case in Al(OH)3.
(1) If both assertion and reason are CORRECT, but reason is the CORRECT explanation of the assertion.
(2) If both assertion and reason are CORRECT, but reason is not the CORRECT explanation of the assertion.
(3) If asserton if CORRECT but reason in INCORRECT
(4) If assertion is INCORRECT reason in CORRECT.
12. The correct order of radii is : [JEE 2000]
(1) N < Be < B (2) F– , O2– , N3– (3) Na < Li < K (4) Fe3+ < Fe2+ < Fe4+
13. The correct order of acidic strength is [JEE 2000]
(1) Cl2O7 > SO3 > P4O10 (2) CO2 > N2O5 > SO3
(3) Na2O > MgO > Al2O3 (4) K2O > CaO > MgO
14. The set representing correct order of IP1 is [JEE 2001]
(1) K > Na > Li (2) Be > Mg > Ca (3) B > C > N (4) Fe > Si > C
15. Identify the least stable ion amongst the following : [JEE 2002]
(1) Li– (2) Be– (3) B– (4) C–
16. Identify the correct order of acidic strengths of CO2, CuO, CaO, H2O [JEE 2002]
(1) CaO < CuO < H2O < CO2 (2) H2O < CuO < CaO , CO2
(3) CaO < H2O < CuO < CO2 (4) H2O < CO2 < CaO < CuO
17. The increasing order of atomic radii of the following Group 13 elements is [JEE-Advanced 2016]
(1) Al < Ga < In < T (2) Ga < Al < In < Tl
(3) Al < In < Ga < Tl (4) Al < Ga < Tl < In
18. The 1st , 2nd, and 3rd ionization enthalpies, I1, I2 , I3 , of four atoms with atomic numbers n, n +1, n + 2 and
n + 3, where n < 10, are tabulated below. What is the value of n ? [JEE-Advanced 2020]
Atomic Ionization Enthalpy (kJ / mol)
number I1 I2 I3
n 1681 3374 6050
n+1 2081 3952 6122
n+2 496 4562 6910
n+3 738 1451 7733
[28]
ANSWER KEY
EXERCISE–I
1. 3 2. 4 3. 2 4. 2 5. 2 6. 2 7. 3
8. 1 9. 1 10. 4 11. 4 12. 1 13. 2 14. 3
15. 3 16. 4 17. 2 18. 2 19. 2 20. 3 21. 2
22. 1 23. 2 24. 2 25. 2 26. 3 27. 4 28. 3
29. 4 30. 3 31. 3 32. 2 33. 1 34. 1 35. 1
36. 3 37. 3 38. 2 39. 3 40. 3 41. 3 42. 4
43. 1 44. 4 45. 2 46. 3 47. 3 48. 4 49. 3
50. 2 51. 1 52. 1 53. 2 54. 4 55. 1 56. 4
57. 1 58. 1 59. 3 60. 2 61. 5.50 62. 5.50 63. 7
64. 5 65. 6 66. 5 67. 2 68. 2
EXERCISE–II
1. 3 2. 4 3. 1 4. 1 5. 2 6. 2 7. 4
8. 4 9. 2 10. 2 11. 2 12. 2 13. 2 14. 1
15. 2 16. 4 17. 3 18. 2 19. 2 20. 1 21. 2
22. 3 23. 1 24. 2
EXERCISE–III
1. 1 2. 4 3. 3 4. 1 5. 4 6. 2 7. 1
8. 4 9. 3 10. 1 11. 4 12. 4 13. 3 14. 4
15. 1 16. 4 17. 3 18. 4 19. 1 20. 2 21. 3
22. 4 23. 4 24. 2 25. 3 26. 2 27. 3 28. 4
29. 3 30. 2 31. 4 32. 3 33. 1 34. 2 35. 2
36. 1 37. 3 38. 3 39. 3 40. 2 41. 2 42. 4
43. 4 44. 2 45. 2 46. 4 47. 3 48. 4 49. 4
50. 3 51. 3 52. 3 53. 2 54. 1 55. 2 56. 2
57. 2 58. 2 59. 1 60. 1 61. 2 62. 3 63. 3
64. 2 65. 2 66. 1 67. 2 68. 3 69. 3 70. 2
71. 101.00 72. 1 73. 3 74. 4 75. 1 76. 2 77. 02.00
78. 2 79. 5576 kJ/mol 80. 1 81. 2 82. 4 83. 3
84. 1 85. 2 86. 1 87. 4 88. 2 89. 49 90. 4
91. 4 92. 2 93. 2 94. 3 95. 3 96. 3 97. 4
98. 4 99. 2 100. 0.00 101. 12.00 102. 4.00 103. 0.00 104. 10.00
105. 7.00 106. 1 107. 3 108. 1 109. 4 110. 1 111. 4
112. 4 113. 2 114. 2 115. 2 116. 4 117. 2.00 118. C
119. 3 120. 4 121. 3 122. 1 123. 03.00 124. 04.00 125. 2
126. 3 127. 2 128. 2 129. 1 130. 2 131. 3 132. 3
133. 1 134. 3 135. 3 136. 1 137. 1 138. 2.00 139. 2.00
140. 1 141. 1 142. 2 143. 1 144. 1 145. 4 146. 2
147. 3 148. 3 149. 3 150. 2 151. 2 152. 4 153. 4
154. 3 155. 3 156. 3 157. 3 158. 1 159. 2 160. 2
161. 2 162. 3 163. 16.00 164. 2.00 165. 11.00 166. 4.0
[29]
EXERCISE–IV
1. 1 2. 3 3. 3 4. 1 5. 4 6. 1 7. 4
8. 1 9. 2 10. 3 11. 3 12. 2 13. 1 14. 2
15. 2 16. 1 17. 2 18. 9
[30]
