Fundamental Particles 1. Where are protons located in an atom? (A) Around the nucleus (B) Inside the nucleus (C) Both (A) & (B) (D) None of these 2. Which of the following statements is true ? (A) A ‘p’ is 1837 times heavier than an ‘e’. (B) A ‘p’ is 1/1837 times heavier than an ‘e’. (C) A ‘p’ is 1837 times lighter than an ‘e’ (D) ‘p’ has the same mass as an ‘e’. 3. Isotopes of an elements have – (A) different chemical properties (B) different atomic (C) The same physical properties (D) Different number of neutrons 4. Nucleus consist of (A) Proton and electron (B) Proton and neutron (C) Neutron and electron (D) Only neutron 5. Mass number of element is - (A) Number of protons in its nucleus (B) Number of electrons and protons in the atom (C) Number of neutrons and protons in the nucleus (D) Number of neutrons in the nucleus 6. According to the Dalton's atomic theory (A) Electrons, proton and neutron are found in atom (B) Atom is indivisible (C) Atom of various element have same properties (D) Atoms are destroyed in the chemical reaction 7. Neutron is a fundamental particle which have (A) +1-unit charge and 1 unit mass (B) No charge and 1 unit mass (C) Have no charge and no mass (D) Have-1 unit charge and I unit mass 8. Atomic number of any element (A) Atomic weight divided by two (B) Number of neutron in nucleus (C) Nucleus weight (D) Nuclear charge 9. Lightest particle is (A) n (B) e (C) p (D) None of these 10. Fundamental particle of atomic nucleus is (A) p. e - (B) p. n. e (C) p. n (D) n, e 11. Isotopes of an element are the atom which have - (A) The same number of neutrons in their nuclei (B) The same mass number (C) Different number of electrons in their orbit (D) The same number of proton in their nuclei 12. Cl !" #$ and Cl !" #" differ from other in number of (A) ‘e’ (B) ‘p’ (C) ‘n’ (D) A & C 13. Ar !% &’ and Ca (’ &’ have the same number of (A) ‘e’ (B) ‘p’ (C) ‘n’ (D p+n 14. The total number of neutrons in zinc (z= 30) with mass number 70 is (A) 40 (B) 20 (C) 36 (D) 38
Transcript
Fundamental Particles 1. Where are protons located in an atom? (A) Around the nucleus (B) Inside the nucleus (C) Both (A) & (B) (D) None of these 2. Which of the following statements is true ? (A) A ‘p’ is 1837 times heavier than an ‘e’. (B) A ‘p’ is 1/1837 times heavier than an ‘e’. (C) A ‘p’ is 1837 times lighter than an ‘e’ (D) ‘p’ has the same mass as an ‘e’. 3. Isotopes of an elements have – (A) different chemical properties (B) different atomic (C) The same physical properties (D) Different number of neutrons 4. Nucleus consist of (A) Proton and electron (B) Proton and neutron (C) Neutron and electron (D) Only neutron 5. Mass number of element is - (A) Number of protons in its nucleus (B) Number of electrons and protons in the atom (C) Number of neutrons and protons in the nucleus (D) Number of neutrons in the nucleus 6. According to the Dalton's atomic theory (A) Electrons, proton and neutron are found in atom (B) Atom is indivisible (C) Atom of various element have same properties (D) Atoms are destroyed in the chemical reaction 7. Neutron is a fundamental particle which have (A) +1-unit charge and 1 unit mass (B) No charge and 1 unit mass (C) Have no charge and no mass (D) Have-1 unit charge and I unit mass 8. Atomic number of any element (A) Atomic weight divided by two (B) Number of neutron in nucleus (C) Nucleus weight (D) Nuclear charge 9. Lightest particle is (A) n (B) e (C) p (D) None of these 10. Fundamental particle of atomic nucleus is (A) p. e- (B) p. n. e (C) p. n (D) n, e 11. Isotopes of an element are the atom which have - (A) The same number of neutrons in their nuclei (B) The same mass number (C) Different number of electrons in their orbit (D) The same number of proton in their nuclei 12. Cl!"
#$ and Cl!"#" differ from other in number of
(A) ‘e’ (B) ‘p’ (C) ‘n’ (D) A & C 13. Ar!%
&' and Ca('&' have the same number of
(A) ‘e’ (B) ‘p’ (C) ‘n’ (D p+n 14. The total number of neutrons in zinc (z= 30) with mass number 70 is (A) 40 (B) 20 (C) 36 (D) 38
15. The sum of number of neutron and protons in one of the isotopes of hydrogen is (A) 3 (B) 2 (C) 5 (D) 6 16. Difference between Cl atom and CI- ion of (A) ‘e’ (B) ‘p’ (C) ‘n’ (D) A & B 17. 8Ar40, 19K40, 20Ca40 (A) Isotopes (B) Isobars (C) A & B both (D) None 18. Neutron is present in all atom except (A) Protium (B) Deuterium (C) Tritium (D) Helium 19. A monovalent anions has 10 electrons and 10 neutrons The atomic number and mass number of the element are respectively (A) 10, 20 (B) 9, 18 (C) 10,20 (D) 9, 19 20. A trivalent cation of an element contains 10 electrons. The atomic number of the element is (A) 10 (B) 7 (C) 13 (D) None of these 21. Select correct statement (A) Isobars have the same mass number (B) Isotopes have same mass but different atomic number having in elements (C) mass number is negative charged particle (D) isotone have same p-n 22. Mg+2 and F- ions differ in which of the following fundamental particle? (A) Electrons, protons and neutrons (B) Protons and neutrons (C) Only protons (D) Neutrons and electrons 23. The charge carried by an electron is (A) 1.602 x 1019 coulombs (B) 1.602 x 10-19 coulombs (C) 1.609 coulombs (D) 6.02 x 1019 coulombs 24. The mass of a proton is: (A) 1.609 g (B) 1.6 x 1024 g (C) 1.6 × 10-23 g (D) 1.6 × 10-24 g 25. Which of the following is false? (A) Neutron has highest mass among fundamental particles (B) The mass of an electron is negligible (C) e/m is highest for a proton (D) Charge of neutron is zero 26. Species 'X' contains 9 protons, 10 electrons and 11 neutrons. It is : (A) A neutral atom (B) An isotope (C) A cation (D) An anion 27. If three neutrons are added to the nuclei of 92U235, atomic number of new nucleus is : (A) 89 (B) 95 (C) 90 (D) 92 28. Oxygen atom and oxide ion have : (A) Same size (B) Same electron number (C) Same electronic configuration (D) Same proton number
29. Which of the following statement is true ? (A) F- has more electrons than Na+ (B) F- has less electrons than Na+ (C) Na+ and F- has equal electrons (D) None of the above 30. Isotopes differ in : (A) Physical properties (B) Chemical properties (C) Number of protons (D) None of these 31. 5B10+ ₂He4 → X+ 0n¹ 'X' in the above reaction is (A) 7N¹2 (B) 7N13 (C) 6B13 (D) None of these 32. An atom has 12 protons and 12 neutrons, its mass and atomic numbers are: (A) Mass number 12, atomic number 12 (B) Mass number 24, atomic number 12 (C) Mass number 12, atomic number 0 (D) None of these 33. The number of electrons and neutrons in tritium (₁T³) respectively is : (A) 3, 1 (B) 1, 3 (C) 1, 2 (D) None of the above 34. Which of the following triad represents isotones? (A) 6C¹2, 6C13, 6C14 (B) 18Ar40, 20Ca42, 21Sc43 (C) 18Ar40, 20Ca40, 21Sc41 (D) 7N14, 8O16, 9F19 35. An atom with atomic number 18 and mass number 40, has the following arrangement. (A) 18p, 18e, 22n (B) 18p, 18e, 40n (C) 22p, 18e, 18n (D) 22p,22e, 18n 36. Which of the following statements is correct? (A) 7N¹4 and 6C¹3 are isotones (B) 7N¹4 and 6C¹4 are isotopes (C) 7N¹4 and 6C¹2 are isobars (D) 7N¹4 and 6C¹5 are isotones 37. An anion has (A) more electrons than protons (B) more protons than electrons (C) more neutrons than protons (D) more protons than neutrons 38. The number of quantum numbers required to describe an electron in an atom completely is (A) 1 (B) 2 (C) 3 (D) 4 39. Which of the following statement are wrong? (A) An atom is electrically neutral (B) An atom & its ion have an unequal number of protons (C) The size of a cation is smaller than that of corresponding atom (D) An atom & its corresponding anion have equal number of electrons 40. A proton is identical to (A) the nucleus of helium (B) the nucleus of a hydrogen atom (C) a molecule of a hydrogen (D) an atom of hydrogen 41. The e/m ratio of an electron for all type of substances is (A) constant (B) less than one (C) greater than one (D) zero 42. Mass of electron is (A) 9.1083 × 10-31 kg (B) 9.1083 x 10-24 kg (C) 9.1083 × 10-28 kg (D) 1.67 × 10-24 kg 43. Total number of neutrons in dipositive Zinc ion (Zn²+) with mass number 70 is (Z=30) (A) 30 (B) 40 (C) 50 (D) 20
44. An atom which has a mass number of 14 and has 8 neutrons is an (A) isotope of oxygen (B) isobar of oxygen (C) isotope of carbon (D) isobar of carbon 45. An atom of an element has 26 electrons and has a mass number 56. The nucleus of this atom contains ......... neutrons. (A) 26 (B) 36 (C) 30 (D) 56 46 Which of the following statements is not correct? (A) 11Na23 and 12Mg24 are isotones (B) 18Ar40 and 20Ca40 are isobars (C) N–3 and P–3 are isoelectronic species (D) 92U235 and 92U238 are isotopes 47. The quantum number which specifies the location of an electron as well as energy is (A) Principal quantum number (B) Azimuthal quantum number (C) Spin quantum number (D) Magnetic quantum number 48.The electrons of the same orbitals can be distinguished by (A) principal quantum number (B) azimuthal quantum number (C) spin quantum number (D) magnetic quantum number. 49. Principal, azimuthal and magnetic quantum numbers are respectively related to (A) Size, shape, and orientation (B) Shape, size,and orientation (C) Size, orientation, and shape (D) None of the above 50.Principal quantum number of an atom represents. (A) Size of the orbital (B) Spin angular momentum (C) Orbital angular momentum (D) Space orientation of the orbital 51. Two electrons occupying the same orbital are distinguished by : (A) Spin quantum number (B) Principal quantum number (C) Magnetic quantum number (D) Azimuthal quantum number 52. Which quantum number will determine the shape of the subshell (A) Principal quantum number (B) Azimuthal quantum number (C) Magnetic quantum number (D) Spin quantum number 53. The orientation of an atomic orbital is governed by : (A) azimuthal quantum number (B) spin quantum number (C) magnetic quantum number (D) principal quantum number
Principal Quantum Number 54 The principal quantum number ‘n’ can have integral values ranging from : (A) 0 to 10 (B) 1 to ¥ (C) 1 to (n – 1) (D) 1 to 50 55. The total number of orbitals in an energy level designated by principal quantum number n is equal to (A) 2n (B) 2n2 (C) n (D) n2
56. The number of orbitals in a shell with principal quantum number ‘n’ is : (A) 2n (B) 2n2 (C) n2 (D) n + 1
57. The total number of atomic orbitals in fourth energy level of an atom are : (A) 8 (B) 16 (C) 32 (D) 4 58. How many electrons can fit into the orbitals that comprise the 3rd quantum shell n = 3 (A) 2 (B) 8 (C) 18 (D) 32 59. The maximum number of electrons that can be accommodated in fifth energy level is (A) 10 (B) 25 (C) 50 (D) 32 60. The number of sub-shells in the fifth energy level is (A) 4 (B) 11 (C) 9 (D) 5 61.The maximum number of electrons that can be accommodated in the Mth shell is (A) 2 (B) 8 (C) 18 (D) 32 62.For n = 3 energy level, the number of possible orbitals are (A) 1 (B) 3 (C) 4 (D) 9 63. For the n=2 energy level, how many orbitals of all kinds are possible (A) 2 (B) 3 (C) 4 (D) 5 64. The number of quantum numbers required to describe an electron in an atom completely is (A) 1 (B) 2 (C) 3 (D) 4 65. What is the maximum number of electrons which can be accommodated in an atom in which the highest principal quantum number value is 2 (A)10 (B)18 (C) 32 (D) 54 66. Maximum number of electrons present in 'N' shell is (A)18 (B) 32 (C) 2 (D) 8 67. An electron has principal quantum number 3. The number of its (i) sub-shells and (ii) orbitals would be respectively (A) 3 and 5 (B) 3 and 7 (C) 3 and 9 (D) 2 and 5 68. The number of electrons which can be accommodated in an orbital is (A) One (B) Two (C) Three (D) Four 69. Principal quantum number can be used to explain (A) energy (B) size (C) both of them (D) none of these 70.The maximum energy is present in any electron at (A) Nucleus (B) Ground state (C) First excited state (D) Infinite distance from the nucleus 71. The principal quantum number represents (A) Shape of an orbital (B) Distance of electron from nucleus (C) Number of electrons in an orbit (D) Number of orbitals in an orbit 72 For an atom the energy of electron increases with increase in 'n' and the energy difference between successive energy levels (A) Increases (B) Decreases (C) Remains constant (D) Cannot be found
Azimuthal Quantum Numbers
73. The maximum number of electrons which each sub-shell can occupy is (A) 2n2 (B) 2n (C) 2(2l + 1) (D) (2l + 1) 74. The maximum number of electrons in a subshell is given by the expression. (A) 4l – 2 (B) 4l + 2 (C) 2l + 2 (D) 2n2 75. Maximum numbers of electrons in a subshell is given by - (A) (2l+1) (B) 2(2l+1) (C) (2l+1)2 (D) 2(2l+1)2 76. If n and l are respectively the principal and azimuthal quantum numbers, then the expression for calculating the total number of electrons in any orbit is –
(A) (B) (C) (D) 77. The total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is : (A) 2 (B) 4 (C) 6 (D) 8 78. For (n = 3), the possible values of azimuthal quantum number (l) is (A) 0, 1, 2, 3 (B) 0, 1, 2 (C) –2, – 1, 0, 1, 2 (D) 1, 2, 3 79. If n = 3, then the value of 'l' which is incorrect (A) 0 (B)1 (C) 2 (D) 3 80. The maximum number of electrons in a subshell for which l = 3 is: (A) 14 (B) 10 (C) 8 (D) 4 81. For a shell of principal quantum number n = 4, which is incorrect: (A) 16 orbitals (B) maximum 32 electrons (C) 4 subshells (D) l = 0, 1, 2, 3, 4 82. For an orbital with azimuthal quantum number l = 3, the maximum number of electrons will be: (A) 2 (B) 6 (C) zero (D) 1 83. How many electrons can fit in the orbital for which n = 3 and l = 1? (A) 14 (B) 2 (C) 6 (D) 10 84. For azimuthal quantum number l = 3, the maximum number of electrons will be (A) 2 (B) 6 (C) 0 (D) 14 85. A sub-shell with n = 6, l = 2 can accommodate a maximum of (A) 12 electrons (B) 36 electrons (C) 10 electrons (D) 72 electrons 86. Maximum number of electrons in a subshell having n = 4 and l = 3 are: (A) 14 (B) 16 (C) 10 (D) 12 87. How many electrons can be accommodated in a sub-shell for which n = 3, l = 1 (A) 8 (B) 6 (C) 18 (D) 32
n
12 (2 1)
=
=
+å!
!
!
n 1
12 (2 1)
= -
=
+å!
!
!
n 1
02(2 1)
= +
=
+å!
!
!
n 1
02(2 1)
= -
=
+å!
!
!
88. The total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is (A) 2 (B) 4 (C) 6 (D) 8 89. 2p orbitals have (A) 𝑛 = 1, 𝑙 = 2 (B) 𝑛 = 1, 𝑙 = 0 (C) 𝑛 = 2, 𝑙 = 1 (D) 𝑛 = 2, 𝑙 =0 90. The maximum number of electrons present in an suborbit l = 3, is (A) 6 (B) 8 (C) 10 (D) 14 91. If n = 3, then the value of 'l' which is incorrect (A) 0 (B) 1 (C) 2 (D) 3 92. Which of the following orbital is not possible (A) 3 f (B) 4 f (C) 5 f (D) 6 f
Shape Of Orbitals
93.The quantum number which may be designated by s,p,d and f instead of number is (A) n (B) l (C) 𝑚) (D) 𝑚* 94. The shape of an orbital is given by the quantum number (A) n (B) l (C) m (D) s 95. When the azimuthal quantum number has a value of l = 0, the shape of the orbital is (A) Rectangular (B) Spherical (C) Dumbbell (D) Unsymmetrical 96. The shape of s-orbital is (A) Pyramidal (B) Spherical (C) Tetrahedral (D) Dumbbell shaped 97. The azimuthal quantum number is related to (A) Size (B) Shape (C) Orientation (D) Spin 98. The shape of p-orbital is (A) Elliptical (B) Spherical (C) Dumb-bell (D) Complex geometrical 99. When the azimuthal quantum number has a value of l = 1, the shape of the orbital is (A) Unsymmetrical (B) Spherically symmetrical (C) Dumb-bell (D) Complicated 100.Which is not permissible subshell? (A) 2d (B) 4f (C) 6p (D) 3s 101.Which orbital is non-directional (A) s (B) p (C) d (D) All 102.For the dumb-bell shaped orbital, the value of l is (A) 3 (B) 1 (C) 0 (D) 2 103.An orbital with l = 0 is symmetrical about the (A) x-axis only (B) y-axis only (C) z-axis only (D) All 104.Which orbital is dumb-bell shaped ? (A) 1s (B) 2p (C) 3s (D) 3d
105. The value of Azimuthal quantum number for all electrons presents in 5p orbitals is (A) 4 (B) 5 (C) 2 (D) 1 106. If n + l = 6, then total possible number of subshells would be (A) 3 (B) 4 (C) 2 (D) 5 107. The number of orbitals in 3p sub-shell is. (A) 6 (B) 2 (C) 3 (D) 4 108. The number of orbitals in d sub-shell is. (A) 1 (B) 3 (C) 5 (D) 7 109.A sub-shell l = 2 can take how many electrons (A) 3 (B) 10 (C) 5 (D) 6 110.For d electrons, the azimuthal quantum number is (A) 0 (B) 1 (C) 2 (D) 3 111.The quantum numbers n = 2, l = 1 represent (A) 1s orbital (B) 2sorbital (C) 2p orbital (D) 3d orbital 112. Azimuthal quantum number defines (A) e/m ratio of electron (B) Spin of electron (C) Angular momentum of electron (D) Magnetic momentum of electron 113. Number of orbitals in h sub-shell is (A) 11 (B) 15 (C) 17 (D) 19 114. For principal quantum number n = 4 the total number of orbitals having l = 3 (A) 3 (B) 7 (C) 5 (D) 9 115. The maximum number of electrons that can be accommodated in 'ƒ' sub shell is (A) 2 (B) 8 (C) 32 (D) 14 116. The maximum number of electrons accommodated in 5ƒ orbitals are (A) 5 (B) 10 (C) 14 (D) 18 117. The maximum number of electrons in an atom with l = 2 and n = 3 is (A) 2 (B) 6 (C) 12 (D) 10 118. Energy of atomic orbitals in a particular shell is in the order (A) 𝑠 < 𝑝 < 𝑑 < 𝑓 (B) 𝑠 > 𝑝 > 𝑑 > 𝑓 (C) 𝑝 < 𝑑 < 𝑓 < 𝑠 (D)𝑓 > 𝑑 >𝑠 > 𝑝 119. Which of the sub-shell is circular (A) 4s (B) 4f (C) 4p (D) 4d 120. There is no difference between a 2p and a 3p orbital regarding (A) Shape (B) Size (C) Energy (D) Value of 𝑛
Angular Momentum
121.For a d-electron, the orbital angular momentum is (A) √6ℏ (B) √2ℏ (C) ℏ (D) 2ℏ 122.The orbital angular momentum of an electron in 2s-orbital is - (A) ℎ
&+ (B) zero (C) ℎ
(+ (D) ℎ
(+
123.The orbital angular momentum of a p-electron is given as :
(A) ℎ√(+
(B) √3 ℎ(+
(C) 8#(ℎ+ (D) √6. ℎ(+
124.The orbital angular momentum of an electron in 3s-orbital is : (A) +!
(ℎ(+
(B) zero (C) ℎ(+
(D) √2 ℎ(+
125.The orbital with zero angular momentum is - (A) s (B) p (C) d (D) f 126. The orbital angular momentum of an electron in the orbitals 1s, 3s, 3d and 2p is respectively (A) 0, 0, ℎ
(+√6, ℎ(+√2 (B) 1, 1, ℎ
(+√4, ℎ(+√2
(C) 0, 1, ℎ(+√6, ℎ
(+√3 (D) 0, 0, ℎ(+√20, ℎ
(+√6 127.In which of the following sets of orbitals, electrons have equal orbital angular momentum? (A) 1s and 2s (B) 2s and 2p (C) 2p and 3p (D) 3p and 3d
Magnetic Quantum Numbers
128. For a given value of quantum number 𝑙, the number of allowed values of 𝑚 is given by (A) l + 2 (B) 2l + 2 (C) 2l + 1 (D) l + 1 129. Which statement is not correct for n = 5, m = 3 (A) l = 4 (B) 𝑙 = 0,1,3; 𝑠 = + !
( (C) l = 3 (D) All are
correct 130. An e– has magnetic quantum number as –3, what is its principal quantum number (A) 1 (B) 2 (C) 3 (D) 4 131. When the value of azimuthal quantum number is 3, magnetic quantum number can have value (A) + 1, 0, – 1 (B) + 2, + 1, 0, – 1, – 2 (C) – 3, – 2, – 1, – 0, + 1, + 2, + 3 (D) + 1, – 1 132. The total magnetic quantum numbers for d-orbital is given by (A) 2 (B) 0, ± 1, ± 2 (C) 0, 1, 2 (D) 5
2
133. The quantum number ‘m’ of a free gaseous atom is associated with (A) The effective volume of the orbital (B) The shape of the orbital (C) The spatial orientation of the orbital (D) The energy of the orbital in the absence of a magnetic field 134.The maximum number of electrons in p-orbital with n = 5, m = 1 is (A) 6 (B) 2 (C) 14 (D) 10 135. The number of electrons that can be accommodated in dz2 orbital is (A) 10 (B) 1 (C) 4 (D) 2 136. Maximum electrons in a d-orbital are (A) 2 (B) 10 (C) 6 (D) 14 137. The energy of an electron of 2py orbital is (A) Greater than that of 2px orbital (B) Less than that of 2px orbital (C) Equal to that of 2s orbital (D) Same as that of 2pz orbital 138. What is the maximum number of orbitals that can be identified with the following quantum number n = 3, l = 1, m = 0 (A) 1 (B) 2 (C) 3 (D) 4 139. The maximum value of m for an electron in fourth energy level is: (A) +4 (B) +3 (C) +5 (D) +9 140. The orbital angular momentum corresponding to n = 4 and m = –3 is :
(A) 0 (B) (C) (D)
141. Which is not correct for an electron having n = 5, m = 2 : (A) l = 4 (B) l = 0, 1, 2, 3 (C) l = 3 (D) l = 2, 3, 4 142. Which of the following orbital quantum number value is not possible for an electron present in 4d subshell: (A) n = 4 (B) l = 1 (C) m = 1 (D) m = 2 143. Maximum number of orbitals in an atom having quantum numbers n = 3, l = 2, m = + 2 are (A) 1 (B) 2 (C) 3 (D) 4 144. Match List-I with List-II and select the correct answer using the codes given below the lists
List-I List-II (P) Number of value of l for an energy level (1) 0, 1, 2, ............. (n - 1) (Q) Value of l for a particular type of orbital (2) +l to –l through zero (R) Number of values of m for l = 2 (3) 5 (S) Value of 'm' for a particular type of orbital (4) n Code : P Q R S P Q R S (A) 4 1 2 3 (B) 4 1 3 2 (C) 1 4 2 3 (D) 1 4 3 2
p2h
p2h6
ph3
145. Which of the following statements is/are correct for an electron of quantum numbers n = 4 and m = 2 ? (A) The value of l may be 2. (B) The value of l may be 3. (C) The value of l may be +1/2. (D) The value of l may be 0, 1, 2, 3. 146. Which quantum number will determine the shape of the subshell (A) Principal quantum number (B) Azimuthal quantum number (C) Magnetic quantum number (D) Spin quantum number 147. A given orbital is labelled by the magnetic quantum number m = –1. This can not be - (A) s-orbital (B) d-orbital (C) p-orbital (D) f-orbital 148. For an electron, magnetic quantum number m = +2. The electron may be present in (A) 5s-sub-shell (B) 5d-sub-shell (C) 5p-sub-shell (D) 5f-sub-shell 149. If magnetic quantum number of a given atom represented by –3, then what will be its principal quantum number (A) 2 (B) 3 (C) 4 (D) 5 150. The magnetic quantum number for an electron when the value of principal quantum number is 2 can have (A) 3 values (B) 2 values (C) 9 values (D) 6 values 151. The magnetic quantum number specifies (A) Size of orbitals (B) Shape of orbitals (C) Orientation of orbitals (D) Nuclear stability 152. If value of azimuthal quantum number 𝑙 is 2, then total possible values of magnetic quantum number will be (A) 7 (B) 5 (C) 3 (D) 2 153. For p-orbital, the magnetic quantum number has value (A) 2 (B) 4, – 4 (C) – 1, 0, +1 (D) 0 154. If the value of azimuthal quantum number is 3, the possible values of magnetic quantum number would be (A) 0, 1, 2, 3 (B) 0, – 1, – 2, – 3 (C) 0, ±1, ±2, ± 3 (D) ±1, ±2, ±3
Orientation of Orbitals
155. The maximum probability of finding electron in the dxy orbital is – (A) Along the x-axis (B) Along the y-axis (C) At an angle of 45º from the x and y-axis (D) At an angle of 90º from the x and y-axis 156. Which d - orbital has different shape from rest of all d - orbitals ? (A) 𝑑-! (B) dxy (C) dxz (D) dyz 157. 3py orbital has..........nodal plane : (A) XY (B) YZ (C) ZX (D) All of these
158. In case of 𝑑.!/0! orbital (A) Probability of finding the electron along x-axis is zero. (B) Probability of finding the electron along y-axis is zero. (C) Probability of finding the electron is maximum along x and y-axis. (D) Probability of finding the electron is zero in x-y plane 159. Which d-orbital does not have four lobes (A) 𝑑.!/0! (B) dxy (C) 𝑑-! (D) dxz 160. Which of the following d-orbitals has dough-nut shape ? (A) dxy (B) dyz (C) 𝑑.!/0! (D) 𝑑-! 161. Magnetic quantum number specifies - (A) Size of orbitals (B) Shape of orbitals (C) Orientation of orbitals (D) Nuclear stability 162. A p-orbital can accommodate (A) 4 electrons (B) 6 electrons (C) 2 electrons with parallel spins (D) 2 electrons with opposite spins 163. A given orbital is labeled by the magnetic quantum number m = –1. This could not be (A) s - orbital (B) p-orbital (C) d-orbital (D) f-orbital 164. Non-directional orbital is : (A) 3s (B) 4f (C) 4d (D) 4p 165. Which of the following pairs of d-orbitals will have electron density along the axis ? (A) 𝑑.0,𝑑.!–0! (B) 𝑑-!, 𝑑.- (C) 𝑑.-, 𝑑0- (D) 𝑑-!, 𝑑.!–0! 166. The probability of finding an electron residing in a px orbital is not zero : (A) In the yz plane (B) In the xy plane (C) In the y direction (D) In the z direction 167. The shape of dxy orbital will be (A) Circular (B) Dumb-bell (C) Double dumb-bell (D) Trigonal
Nodes 168. For an electron, with n = 3 has only one radial node. The orbital angular momentum of the electron will be (A) 0 (B) 2
(+ (C) 2
(+ (D) 3 = 2
(+>
169. Number of nodal centers for 2s orbital (A) 1 (B) 0 (C) 4 (D) 3 170. The number of nodal planes in a px orbital is : (A) 1 (B) 2 (C) 3 (D) zero 171. The number of radial nodes in 3s and 2p respectively are: (A) 2 and 0 (B) 1 and 2 (C) 0 and 2 (D) 2 and 1
6 2
172. Which of the following orbitals has (have) one spherical node? (A) 1s (B) 2s (C) 2p (D) 3p 173. The number of nodal planes in a px orbital is (A) one (B) two (C) three (D) Zero 174. The sum of angular nodes and radial nodes of 4dxy atomic orbital are (A) 1 (B) 2 (C) 3 (D) 4 175. Which of the following pair of orbitals posses two nodal planes (A) 𝑝. , 𝑑.!/0! (B) 𝑑.0 , 𝑑-. (C) 𝑝.0 , 𝑑-. (D) 𝑑-! , 𝑑.!/0!
176. The number of radial nodes of 3s and 2p orbitals are respectively. (A) 2, 0 (B) 0, 2 (C) 1, 2 (D) 2, 1 177. The electron density between 1s and 2s orbital is (A) High (B) Low (C) Zero (D) None of these 178. A 3p orbital has (A) Two spherical nodes (B) Two non-spherical nodes (C) One spherical and one non-spherical nodes (D) One spherical and two non-spherical nodes
Spin Quantum Number
179.An electron has spin quantum number, ms = + 1/2 and magnetic quantum number, ml = +1. It cannot be present in (A) s-orbital (B) p-orbital (C) d-orbital (D) f-orbital 180.The maximum number of electrons with clockwise spin that can be accommodated in a f-sub-shell is (A) 14 (B) 7 (C) 5 (D) 10 181.The quantum numbers + 1/2 and – 1/2 for the electron spin represent: (A) Rotation of the electron in clockwise and anticlockwise direction, respectively. (B) Rotation of the electron in anticlockwise and clockwise direction, respectively. (C) Magnetic moment of the electron pointing up and down respectively, (D) Two quantum mechanical spin states which have no classical analogue. 182.The maximum number of 3d-electrons that can have s = –1/2, are (A) 10 (B) 3 (C) 5 (D) 7 183.Spin angular momentum for an electron is given as : (A) ?𝑠(𝑠 + 1) ∗ 2
(+ (B) ?2𝑠(𝑠 + 1) ∗ 2
(+ (C) ?𝑠(𝑠 + 2) ∗ 2
(+ (D) None
184.For a given subshell let maximum number of electrons with same spin be x and number of possible ml values be y. (A) x = 2y (B) x = y (C) .
( = y (D) x = 0
(
185.Assertion: Spin quantum number can have two values, +1/2 and –1/2 Reason: + and – signs signify the positive and negative wave functions. (A) If both assertion and reason are true and reason is the correct explanation of assertion. (B) If both assertion and reason are true but reason is not the correct explanation of assertion. (C) If Assertion is true but reason is false. (D) If both assertion and reason are false. 186.The electrons occupying the same orbital have always ________ spin. (A) parallel (B) antiparallel (C) both (A) and (B) (D) none of these 187. Which of the following rules limits the maximum number of electrons in an orbital to two (A) Aufbau principle (B) Pauli's exclusion principle (C) Hund's rule of maximum multiplicity (D) Heisenberg's uncertainty principle 188. In a given atom no two electrons can have the same values for all the four quantum numbers. This is called (A) Hund's rule (B) Aufbau's principle (C) Uncertainty principle (D) Pauli's exclusion principle 189. The number of 2p electrons having spin quantum number s = –1/2 are (A) 6 (B) 0 (C) 2 (D) 3
Set Of Quantum Numbers
190. Which set of quantum numbers for an electron of an atom is not possible (A) 𝑛 = 1, 𝑙 = 0,𝑚 = 0, 𝑠 = +1/2 (B) 𝑛 = 1, 𝑙 = 1,𝑚 = 1, 𝑠 = +1/2 (C) 𝑛 = 1, 𝑙 = 0,𝑚 = 0, 𝑠 = −1/2 (D) 𝑛 = 2, 𝑙 = 1,𝑚 = −1, 𝑠 = +1/2 191.. Which of the following sets of quantum number is not possible? (A) n = 3; l = 0 + 2, ml = 0, ms = + 1/2 (B) n = 3; l = 0, ml = 0, ms = – 1/2 (C) n = 3; l = 0, ml = –1, ms = +1/2 (D) n = 3; l = 1, ml = 0, ms = –1/2 192. Which of the following sets of the quantum numbers is permitted? (A) n = 4, l = 2, ml = +3, ms = + 1/2 (B) n = 3, l = 3, ml = +3, ms = + 1/2 (C) n = 4, l = 0, ml = 0, ms = + 1/2 (D) n = 4, l = 3, ml = +1, ms = 0
193.Which of the following statements concerning the four quantum numbers is false - (A) n gives idea of the size of an orbital (B) l gives the shape of an orbital (C) ms gives the energy of the electron in the orbital in absence of magnetic field (D) ms gives the direction of spin angular momentum of the electron in an orbital 194. The set of quantum numbers not applicable for an electron in an atom is - (A) n = 1, l = 1, m = 1, s = + 1/2 (B) n = 1, l = 0, m = 0, s = + 1/2 (C) n = 1, l = 0, m = 0, s = – 1/2 (D) n = 2, l = 0, m = 0, s = + 1/2
195. Which one of the following represents an impossible arrangement ? n l m s n l m s (A) 3 2 –2 -½ (B) 4 0 0 +½ (C) 3 2 –3 +½ (D) 5 3 0 -½ 196. What is the correct orbital designation for the electron with the quantum numbers,
n = 4, l = 3, m = – 2, s = +1/2 (A) 3 s (B) 4 f (C) 5 p (D) 6 s 197. For principal quantum number n = 4, the total number of orbitals having l = 3 is (A) 3 (B) 7 (C) 5 (D) 9 198. Principal quantum number of an atom represents (A) Size of the orbital (B) Spin angular momentum (C) Orbital angular momentum (D) Space orientation of the orbital 199. Which of the following set of quantum numbers is not valid. (A) n = 3, l = 2, m = 2, s = +1/2 (B) n = 2, l = 0, m = 0, s = +1/2 (C) n = 4, l = 2, m = –1, s = +1/2 (D) n = 4, l = 3, m = 4, s = +1/2 200. Which of the following combinations of quantum numbers is allowed ? n l m ms n l m ms (A) 3 2 1 0 (B) 2 0 0 +1/2 (C) 3 -3 -2 +1/2 (D) 1 0 1 +1/2 201. An orbital containing electron having quantum number n = 4, l = 3, m = 0 and s = +1/2 is called (A) 3s orbital (B) 3p orbital (C) 4d orbital (D) 4f orbital 202. Which of the following represents the correct set of quantum numbers of a 4d electron ? (A) 4, 3, 2, + !
( (B) 4, 2, 1, 0 (C) 4, 3, – 2, + !
( (D) 4, 2, 1, – !
(
203. Maximum number of electrons that can have n = 3, l = 2, m = +2, s = +1/2 in an atom are : (A) 18 (B) 6 (C) 24 (D) 1 204. Which of the following sets of quantum number are correct ? (A) n = 3, l = 2, m = + 1, s = +1/2 (B) n = 3, l = 3, m = + 3, s = +1/2 (C) n = 4, l = 0, m = 0, s = +1/2 (D) n = 5, l = 2, m = + 4, s = +1/2 205. From the given sets of quantum numbers the one that is inconsistent with the theory is (A) 𝑛 = 3; 𝑙 = 2;𝑚 = −3; 𝑠 = +1/2 (B) 𝑛 = 4; 𝑙 = 3;𝑚 = 3; 𝑠 = +1/2 (C) 𝑛 = 2; 𝑙 = 1;𝑚 = 0; 𝑠 = −1/2 (D) 𝑛 = 4; 𝑙 = 3;𝑚 = 2; 𝑠 = +1/2 206. Which of the following set of quantum numbers is permitted (A) n = 3, l = 2, m = – 2, s = +1/2 (B) n = 3, l = 2, m = – 1, s = 0 (C) n = 2, l = 2, m = +1, s = – 1/2 (D) n = 2, l = 2, m = +1, s = – ½
207. Consider the following sets of quantum numbers : n l m s n l m s
(i) 3 0 0 +1/2 (ii) 2 2 1 +1/2 (iii) 4 3 –2 –1/2 (iv) 1 0 –1 –1/2 (v) 3 2 3 +1/2 Which of the following sets of quantum numbers is not possible ? (A) (i) and (iii) (B) (ii), (iii) and (iv) (C) (i), (ii), (iii) and (iv) (D) (ii), (iv) and (v) 208. The following quantum number are possible for how many orbitals? n = 3, l = 2, m = +2 (A) 3 (B) 2 (C) 1 (D) 4 209. Which of the following sets of the quantum numbers is not possible? (A) n = 2, l = 1, m = –1, s = +1/2 (B) n = 2, l = 0, m = 0, s = + 1/2 (C) n = 3, l = 2, m = –2, s = +1/2 (D) n = 3, l = 2, ml = –3, s = +1/2 210. Which of the following sets of quantum number is(are) correct: (A) n = 5, l = 4, m = 0, s = + 1/2 (B) n = 3, l = 3, m = +3, s = +1/2 (C) n = 6, l = 0, m = +1, s = – 1/2 (D) n = 4, l = 2, m = +2, s = 0 211. Which of the following sets of quantum number is/are incorrect? (A) n = 3, l = 3, m = 0, s = +1/2 (B) n = 3, l = 2, m = 2, s = –1/2 (C) n = 3, l = 1, m = 2, s = –1/2 (D) n = 3, l = 0, m = 0, s = +1/2 212. Number of two electron can have the same values of …… quantum numbers (A) One (B) Two (C) Three (D) Four 213. Which of the following sets of quantum numbers is correct for an electron in 4ƒ orbital (A) 𝑛 = 4, 𝑙 = 3,𝑚 = +1, 𝑠 = +1/2 (B) 𝑛 = 4, 𝑙 = 4,𝑚 = −4, 𝑠 = +1/2 (C) 𝑛 = 4, 𝑙 = 3,𝑚 = +4, 𝑠 = +1/2 (D) 𝑛 = 3, 𝑙 = 2,𝑚 = −2, 𝑠 = +1/2 214.Which of the following sets is possible for quantum numbers (A) 𝑛 = 4, 𝑙 = 3,𝑚 = −2, 𝑠 = 0 (B) 𝑛 = 4, 𝑙 = 4,𝑚 = +2, 𝑠 = +1/2 (C) 𝑛 = 4, 𝑙 = 4,𝑚 = −2, 𝑠 = +1/2 (D) 𝑛 = 4, 𝑙 = 3,𝑚 = −2, 𝑠 =+1/2 215. Which set of quantum numbers for an electron of an atom is not possible (A) 𝑛 = 1, 𝑙 = 0,𝑚 = 0, 𝑠 = +1/2 (B) 𝑛 = 1, 𝑙 = 1,𝑚 = 1, 𝑠 = +1/2 (C) 𝑛 = 1, 𝑙 = 0,𝑚 = 0, 𝑠 = −1/2 (D) 𝑛 = 2, 𝑙 = 1,𝑚 = −1, 𝑠 = +1/2 216. Which one of the following set of quantum numbers is not possible for 4p electron (A) 𝑛 = 4, 𝑙 = 1,𝑚 = −1, 𝑠 = +1/2 (B) 𝑛 = 4, 𝑙 = 1,𝑚 = 0, 𝑠 = +1/2 (C) 𝑛 = 4, 𝑙 = 1,𝑚 = 2, 𝑠 = +1/2 (D) 𝑛 = 4, 𝑙 = 1,𝑚 = −1, 𝑠 = +1/2 217. Which of the following sets of quantum numbers is not allowed
218. An electron having the quantum numbers 𝑛 = 4, 𝑙 = 3,𝑚 = 0, 𝑠 = − !( would be in the
orbital (A) 3s (B)3p (C) 4d (D) 4f 219. The number of possible spatial orientations of an electron in an atom is given by its (A) Spin quantum number (B) Spin angular momentum (C) Magnetic quantum number (D) Orbital angular momentum 220. All electrons on the 4p sub-shell must be characterized by the quantum number(s) (A) 𝑛 = 4,𝑚 = 0, 𝑠 = ± !
( (B) l = 1 (C) 𝑙 = 0, 𝑠 = ± !
( (D) 𝑠 = ± !
(
221. Which of the following represents the correct sets of the four quantum numbers of a 4d electron.
(A) 4,3,2, !( (B) 4, 2, 1, 0 (C) 4,3, −2,+ !
( (D) 4,2,1, − !
(
222. Which of the following statements is not correct for an electron that has the quantum numbers 𝑛 = 4 and 𝑚 = 2
(A)The electron may have the quantum number 𝑠 = + !(
(B)The electron may have the quantum number l = 2 (C) The electron may have the quantum number l = 3 (D) The electron may have the quantum number l = 0,1,2,3 223. The set of quantum numbers not applicable for an electron in an atom is (A) 𝑛 = 1, 𝑙 = 1,𝑚) = 1,𝑚* = +1/2 (B) 𝑛 = 1, 𝑙 = 0,𝑚) = 0,𝑚* = +1/2 (C) 𝑛 = 1, 𝑙 = 0,𝑚) = 0,𝑚* = −1/2 (D) 𝑛 = 2, 𝑙 = 0,𝑚) = 0,𝑚* = +1/2
224. If an electron has spin quantum number of + !( and a magnetic quantum number of –1, it
cannot be presented in an (A) d-orbital (B) f-orbital (C) p-orbital (D) s-orbital
Aufbau Principle 225. In hydrogen atom, which is incorrect order of their energies. (A) 1s < 2p (B) 2p = 2s (C) 2p > 2s (D) 2p < 3s 226. Which of the following sets of orbitals may degenerate (A) 2𝑠, 2𝑝. , 2𝑝0 (B) 3𝑠, 3𝑝. , 3𝑑.0 (C) 1𝑠, 2𝑠, 3𝑠 (D) 2𝑝. , 2𝑝0 , 2𝑝- 227. If n = 6, the correct sequence for filling of electrons will be : (A) ns ® (n – 2)f ® (n – 1)d ® np (B) ns ® (n – 1)d ® (n – 2)f ® np (C) ns ® (n – 2)f ® np ® (n – 1)d (D) ns ® np(n – 1)d ® (n – 2)f 228. 4d, 5p, 5f and 6p orbitals are arranged in the order of decreasing energy. The correct option is (A) 5f > 6p > 4d > 5p (B) 5f > 6p > 5p > 4d (C) 6p > 5f > 5p > 4d (D) 6p > 5f > 4d > 5p
229. Which of the following has the least energy (A) 2p (B) 3p (C) 2s (D) 4d 230. The correct order of increasing energy of atomic orbitals is (A) 5𝑝 < 4𝑓 < 6𝑠 < 5𝑑 (B) 5𝑝 < 6𝑠 < 4𝑓 < 5𝑑 (C) 4𝑓 < 5𝑝 < 5𝑑 < 6𝑠 (D) 5𝑝 < 5𝑑 < 4𝑓 < 6𝑠 231. The orbital with maximum energy is (A) 3d (B) 5p (C) 4s (D) 6d 232. Which of the following sequence is correct as per Aufbau principle (A) 3𝑠 < 3𝑑 < 4𝑠 < 4𝑝 (B) 1𝑠 < 2𝑝 < 4𝑠 < 3𝑑 (C) 2𝑠 < 5𝑠 < 4𝑝 < 5𝑑 (D) 2𝑠 < 2𝑝 < 3𝑑 < 3𝑝 233. Which of the following set of quantum numbers represents the highest energy of an atom ? (A) n = 3, l = 0, m = 0, s = +!
( (B) n = 3, l = 1, m =1, s = +!
(
(C) n = 3, l = 2, m = 1, s = +!( (D) n = 4, l = 0, m = 0, s = +!
(
234. The electrons identified by quantum numbers n and l : (1) n = 4, l = 1 (2) n = 4, l = 0 (3) n = 3, l = 2 (4) n = 3, l = 1 can be placed in the order of increasing energy as : (A) 3 > 4 < 2 < 1 (B) 4 < 2 < 3 < 1 (C) 2 < 4 < 1 3 (D) 1 < 3 2 < 4 235. In any atom which sub-shell will have the highest energy in the following (A) 3p (B) 3d (C) 4s (D) 3s 236. Which of the following set of quantum numbers belong to highest energy
237. n and l for some electrons are given. Which of the following is expected to have least energy? (A) n = 3, l = 2 (B) n = 3, l = 0 (C) n = 2, l = 1 (D) n = 4, l = 0 238. The electrons, identified by quantum numbers n and l (i) n = 4, l = 1 (ii) n= 4, l = 0 (iii) n = 3, l = 2 (iv) n = 3, l = 1 can be placed in order of increasing energy, from the lowest to highest, as (A) (iv) < (ii) < (iii) < (i) (B) (ii) < (iv) < (v) < (iii) (C) (i) < (iii) < (ii) < (iv) (D) (iii) < (i) < (iv) < (ii) 239. The atomic orbitals are progressively filled in order of increasing energy. This principle is called as (A) Hund’s rule (B) Aufbau principle (C) Exclusion principle (D) de-Broglie rule 240. The electron should be filled in the orbital in accordance with the increasing order of their energy. This statement is related with – (A) Aufbau principle (B) Pauli principle (C) Hund's principle (D) Plank's rules
241. According to Aufbau's principle, which of the three 4d, 5p and 5s will be filled with electrons first (A) 4d (B) 5p (C) 5s (D) 4d and 5s will be filled simultaneously 242. The order of filling of electrons in the orbitals of an atom will be (A) 3𝑑, 4𝑠, 4𝑝, 4𝑑, 5𝑠 (B) 4𝑠, 3𝑑, 4𝑝, 5𝑠, 4𝑑 (C) 5𝑠, 4𝑝, 3𝑑, 4𝑑, 5𝑠 (D) 3𝑑, 4𝑝, 4𝑠, 4𝑑, 5𝑠 243. Which of the following transition neither shows absorption nor emission of energy in case of Hydrogen atom: (A) 3px, 3s (B) 3dxy, 3dyz (C) 3s, 3dxy (D) All the above 244. Aufbau principle is obeyed in which of the following electronic configurations (A) 1𝑠(2𝑠(2𝑝3 (B) 1𝑠(3𝑝#3𝑠( (C) 1𝑠(3𝑠(3𝑝3 (D) 1𝑠(2𝑠(3𝑠( 245. The orbital diagram in which the Aufbau’s principle is violated is 2s 2𝑝. 2𝑝0 2𝑝- 2s 2𝑝. 2𝑝0 2𝑝- (A) ↑↓ ↑↓ ↑ (B) ↑ ↑↓ ↑ ↑ (C) ↑↓ ↑ ↑ ↑ (D) ↑↓ ↑↓ ↑↓ ↑ 246. Which electronic configuration is not observing the (n + 1) rule (A) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑!, 4𝑠( (B)1𝑠(, 2𝑠(𝑠𝑝3, 3𝑠(3𝑝33𝑑", 4𝑠( (C) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑$, 4𝑠! (D) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑%, 4𝑠( 247. The 19th electron of chromium has which of the following sets of quantum numbers?
n l m ms n l m ms (A) 3 0 0 –1/2 (B) 3 2 –2 –1/2 (C) 4 0 0 –1/2 (D) 4 1 –1 – 1/2 248. In a multi-electron atom, which of the following orbitals described by the three quantum members will have the same energy in the absence of magnetic and electric fields (a) 𝑛 = 1, 𝑙 = 0,𝑚 = 0 (b) 𝑛 = 2, 𝑙 = 0,𝑚 = 0 (c) 𝑛 = 2, 𝑙 = 1,𝑚 = 1 (d) 𝑛 = 3, 𝑙 = 2,𝑚 = 0 (e) 𝑛 = 3, 𝑙 = 2,𝑚 = 0 (A) (a) and (b) (B) (b) and (c) (C) (c) and (d) (D) (d) and (e) 249. When 3d orbital is complete, the new electron will enter the (A) 4p-orbital (B) 4f-orbital (C) 4s-orbital (D) 4d-orbital 250. In a potassium atom, electronic energy levels are in the following order (A) 4s > 3d (B) 4s > 4p (C) 4s < 3d (D) 4s < 3p 251. Electronic configuration of deuterium atom is (A) 1s1 (B) 2s2 (C) 2s1 (D) 1s2
252. The configuration [Ar] 3d10 4s2 4p4 is similar to that of (A) boron (B) nitrogen (C) Sulphur (D) aluminum
253. The type of orbitals present in Fe is (A) s (B) s and p (C) s, p and d (D) s,p,d and f 254. Which of the following electronic configuration is not possible (A) 1𝑠(2𝑠( (B) 1𝑠(, 2𝑠(2𝑝3 (C) [𝐴𝑟]3𝑑!', 4𝑠(4𝑝( (D) 1𝑠(, 2𝑠(2𝑝(, 3𝑠! 255. Fe (atomic number = 26) atom has the electronic arrangement (A) 2, 8, 8, 8 (B) 2, 8, 16 (C) 2, 8,14, 2 (D) 2, 8, 12, 4 256. The electronic configuration of an element with atomic number 17 is (A) 1𝑠(, 2𝑠(2𝑝3, 3𝑠!3𝑝3 (B) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝&, 4𝑠! (C) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝$ (D) 1𝑠(, 2𝑠(2𝑝3, 3𝑠!3𝑝&, 4𝑠( 257. The total number of electrons present in all the s-orbitals, all the p-orbitals and all the d-orbitals of cesium ion are respectively (A) 8, 26, 10 (B) 10, 24, 20 (C) 8, 22, 24 (D) 12, 20, 22 258. After np orbitals are filled, the next orbital filled will be : (A) (n + 1) s (B) (n + 2) p (C) (n + 1) d (D) (n + 2) s 259. Which element is represented by the following electronic configuration
2𝑝 2𝑠 ↑↓ ↑↓ ↑
1𝑠 ↑↓ ↑↓
(A) Nitrogen (B) Oxygen (C) Fluorine (D) Neon 260. Given is the electronic configuration of element X : K L M N 2 8 11 2 The number of electrons present with l = 2 in an atom of element X is : (A) 3 (B) 6 (C) 5 (D) 4 261. The four quantum numbers of the outermost orbital of K (atomic no. =19) are
262. Azimuthal quantum number for last electron of Na atom is (A) 1 (B) 2 (C) 3 (D) 0 263. The number of electrons in the M-shell of the element with atomic number 24 are : (A) 24 (B) 12 (C) 8 (D) 13 264. Krypton (36Kr) has the electronic configuration (18Ar) 4𝑠(, 3𝑑!', 4𝑝3. The 37th electron will go into which one of the following sub-levels (A) 4f (B) 4d (C) 3p (D)5s
265. Electronic configuration of C is (A) 1𝑠(, 2𝑠(2𝑝( (B) 1𝑠(, 2𝑠(2𝑝# (C) 1𝑠(, 2𝑠( (D) 1𝑠(, 2𝑠(2𝑝3 266. The correct electronic configuration of 𝑇𝑖(𝑍 = 22) atom is (A) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠(3𝑑( (B) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝33𝑑& (C) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝33𝑑& (D) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠!3𝑑# 267. Which of the following configuration is correct for iron (A) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝33𝑑$ (B) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠(3𝑑$ (C) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠(3𝑑" (D) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠(3𝑑3 268. An atom has 2 electrons in K shell, 8 electrons in L shell and 6 electrons in M shell. The number of s-electrons present in that element is (A) 6 (B)5 (C) 7 (D) 10 269. The total number of electrons present in all the p-orbitals of bromine are (A) Five. (B) Eighteen. (C) Seventeen (D) Thirty five 270. Be's 4th electron will have four quantum numbers n l m s n l m s (A) 1 0 0 +1/2 (B) 1 1 +1 +1/2 (C) 2 0 0 – ½ (D) 2 1 0 +1/2 271. Electronic configuration of Sc21 is (A) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠(3𝑑! (B) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠!3𝑑( (C) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝34𝑠'3𝑑# (D) 1𝑠(2𝑠(2𝑝33𝑠(3𝑝(4𝑠(3𝑑( 272. Which of the following electronic configurations is not possible. (A) 1𝑠(2𝑠( (B) 1𝑠(2𝑠(2𝑝3 (C) 3𝑑!'4𝑠(4𝑝( (D) 1𝑠(2𝑠(2𝑝(3𝑠! 273. Values of the four quantum numbers for the last electron in the atom are 𝑛 = 4, 𝑙 = 1,𝑚 = +1 and 𝑠 = −1/2. Atomic number of the atom can’t be (A) 22 (B) 32 (C) 33 (D)36
Hund’s Rule of Maximum Multiplicity 274. Nitrogen has the electronic configuration 1s(, 2s(2p4!2p5!2p6! and not 1s(, 2s(2p4(2p5!2p6' which is determined by (A) Aufbau's principle (B) Pauli's exclusion principle (C) Hund's rule (D) Uncertainty principle 275. Which one of the following configurations represents a noble gas (A) 1s(, 2s(2p3, 3s( (B) 1s(, 2s(2p3, 3s! (C) 1s(, 2s(2p3 (D) 1s(, 2s(sp3, 3s(3p3, 4s(
276. The electronic configuration of silver atom in ground state is (A) [Kr]3d!'4s! (B) [Xe]4f!&5d!'6s! (C) [Kr]4d!'5s! (D) [Kr]4d75s( 277. The correct ground state electronic configuration of chromium atom is (A) [Ar]3d$4s! (B) [Ar]3d&4s( (C) [Ar]3d34s' (D) [Ar]4d$4s! 278. The total number of unpaired electrons in d-orbitals of atoms of element of atomic number 29 is (A) 10 (B) 1 (C) 0 (D) 5 279. Chromium has the electronic configuration 4s!3d$ rather than 4s(3d& because (A) 4s and 3d have the same energy (B) 4s has a higher energy than 3d (C) 4s1 is more stable than 4s2 (D) 4s!3d$ half-filled is more stable than 4s(3d& 280. The two electrons in K sub-shell will differ in (A) Principal quantum number (B) Azimuthal quantum number (C) Magnetic quantum number (D) Spin quantum number 281. The explanation for the presence of three unpaired electrons in the nitrogen atom can be given by (A) Pauli's exclusion principle (B) Hund's rule (C) Aufbau's principle (D) Uncertainty principle 282. Which electronic configuration for oxygen is correct according to Hund's rule of multiplicity (A) 1s(, 2s(2p4(2p5!2p6! (B) 1s(, 2s(2p4(2p5(2p6' (C) 1s(, 2s(2p4#2p5!2p6' (D) None of these 283. The electronic configuration of copper ((7Cu) is (A) 1s(, 2s(2p3, 3s(3p33d7, 4s( (B) 1s(, 2s(2p3, 3s(3p33d!', 4s! (C) 1s(. 2s(2p3, 3s(3p3, 4s(4p3 (D) 1s(, 2s(2p3, 3s(3p33d!' 284.The electronic configuration of an element with atomic number 7 i.e. nitrogen atom is (A) 1s(, 2s!, 2p4# (B) 1s(, 2s(2p4(2p5! (C) 1s(, 2s(2p4!2p5!2p6! (D) 1s(, 2s(2p4!2p5( 285. The electronic configuration of chromium is (A) [Ne]3s(3p33d&, 4s( (B) [Ne]3s(3p33d$, 4s! (C) [Ne]3s(3p3, 4s(4p& (D) [Ne]3s(3p33d!, 4s(4p# 286. The electronic configuration of the element of atomic number 27 is (A) 1s(, 2s(2p3, 3s(3p3, 4s(↑↓)4p(↑↓)(↑↓)(↑↓) 5s (↑) (B) 1s(, 2s(2p3, 3s(3p33d (↑↓)(↑↓)(↑↓),4s (↑↓) 4p (↑) (C) 1s(, 2s(2p3, 3s(3p3, 3d (↑↓)(↑↓)(↑↓)(↑↓), 4s (↑) (D) 1s(, 2s(2p3, 3s(3p3, 3d (↑↓)(↑↓)(↑)(↑)(↑) 4s(↑↓)
287. The electronic configuration of gadolinium (atomic no. 64) is (A) [Xe]4s%5d76s( (B) [Xe]4f "5d!6s( (C) [Xe]4s#5d$6s( (D) [Xe]4f 35d(6s( 288. The electronic configuration 1s(2s(2p4!2p5!2p6! (A) Oxygen (B) Nitrogen (C) Hydrogen (D) Fluorine 289. The electronic configuration of an element is 1s(2s(2p33s(3p33d34s(. This represents its (A) Excited state (B) Ground state (C) Cationic form (D) Anionic form 290. The outer electronic structure 3s(3p$ is possessed by (A) Cl (B) O (C) Ar (D) Br 291. Correct statement is (A) K = 4s!, Cr = 3d&4s(, Cu = 3d!'4s( (B) K = 4s(, Cr = 3d&4s(, Cu = 3d!'4s( (C) K = 4s(, Cr = 3d$4s!, Cu = 3d!'4s( (D) K = 4s!, Cr = 3d$4s!, Cu = 3d!'4s! 292. Consider the ground state of (Z = 24). The numbers of electrons with the azimuthal quantum numbers, l = 1 and 2 are, respectively (A)16 and 4 (B)12 and 5 (C)12 and 4 (D)16 and 5 293. Which of the following electronic configuration is not possible according to Hund’s rule (A) 1s(2s( (B) 1s(2s! (C)1s(2s(2p4!2p5!2p4! (D) 1s(2s(2p4( 294. For sodium atom the number of electrons with m = 0 will be (A) 2 (B) 7 (C) 9 (D) 8 295. Number of unpaired electrons in 1s(2s(2p# is (A) 2 (B) 0 (C) 3 (D) 1 296. The electronic configuration of element with atomic number 24 is (A) 1s(, 2s(2p3, 3s(3p33d&, 4s( (B) 1s(, 2s(2p3, 3s(3p33d!' (C) 1s(, 2s(2p3, 3s(3p33d3 (D) 1s(, 2s(2p3, 3s(3p33d$4s! 297. Total number of unpaired electrons in an atom of atomic number 29 is (A) 1 (B) 3 (C) 4 (D) 2 298. The number of unpaired electrons in 1s(, 2s(2p& is (A) 4 (B) 2 (C) 0 (D)1 299. Number of unpaired electrons in the ground state of beryllium atom is (A) 2 (B) 1 (C) 0 (D) All the above 300. The maximum number of unpaired electron can be present in d subshell are (A) 1 (B)3 (C) 5 (D) 7 301. The atom of the element having atomic number 14 should have (A)One unpaired electron (B)Two unpaired electrons (C)Three unpaired electrons (D)Four unpaired electrons 302. How many unpaired electrons are present in cobalt [Co] metal
(A) 2 (B) 3 (C) 4 (D)7 303. The number of unpaired electrons in nitrogen is (A) 1 (B)3 (C) 2 (D) None of these 304. Which of the following explains the sequence of filling the electrons in different shells (A) Hund's rule (B) Octet rule (C) Aufbau principle (D) All of these 305. Which element contains six unpaired electron (A) Fe (B) Co (C) Ni (D) Cr 306. Electron enters the sub-shell for which (n + l) value is minimum. This is enunciated as (A) Hund’s rule (B) Aufbau principle (C) Heisenberg uncertainty principle (D) Pauli’s exclusion principle 307 For sodium atom the number of electrons with m = 0 will be : (A) 2 (B) 7 (C) 9 (D) 8 308. Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers, l = 1 and 2 are, respectively : (A) 16 and 5 (B) 12 and 5 (C) 16 and 4 (D) 12 and 4 309. The total spin resulting from a d7 configuration is : (A) 1 (B) 2 (C) 5/2 (D) 3/2 310. A neutral atom of an element has 2K, 8L, 9M and 2N electrons. Which of the following is/are incorrectly matched : (A) Total number of s electrons - 8 (B) Total number of p electrons - 12 (C) Total number of d electrons -1 (D) Number of unpaired electrons in element - 3 311. Calculate the minimum and maximum number of electrons which may have magnetic quantum number, m = +1 and spin quantum number, s = –!
( in chromium (Cr) :
(A) 0, 1 (B) 1, 2 (C) 4, 6 (D) 2, 3 312. Which of the following has the maximum number of unpaired electrons ? (A) Mn (B) Ti (C) V (D) Al 313. Aufbau principle is not satisfied by (A) Cr and Cl (B) Cu and Ag (C) Cr and Mg (D) Cu and Na 314. The total spin resulting from a d7 configuration is : (A) 1 (B) 2 (C) 5/2 (D) 3/2 315. Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers, l = 1 and 2 are, respective (A) 16 and 5 (B) 12 and 5 (C) 16 and 4 (D) 12 and 4 316. The correct set of quantum numbers for the unpaired electron of chlorine atom is n l m n l m n l m n l m (A) 2 1 0 (B) 2 1 1 (C) 3 1 1 (D) 3 0 0 317. Number of electrons having l = 1 and m=0 in P-atom in its ground state : (A) 3 (B) 1 (C) 2 (D) 0
318. The atomic number of an element is 17. The number of orbitals containing electron pairs in the valency shell in its ground state are is : (A) 8 (B) 2 (C) 3 (D) 6 319. Which electronic configuration does not follow the Pauli’s exclusion principle (A) 1s2, 2s2 2p4 (B) 1s2, 2s2 2p4 3s2 (C) 1s2, 2p4 (D) 1s2, 2s2 2p6 3s3
320. Pauli's exclusion principle states that (A) Nucleus of an atom contains no negative charge (B) Electrons move in circular orbits around the nucleus (C) Electrons occupy orbitals of lowest energy (D) All the four quantum numbers of two electrons in an atom cannot be equal 321. The statements (i) In filling a group of orbitals of equal energy, it is energetically preferable to assign electrons to empty orbitals rather than pair them into a particular orbital. (ii) When two electrons are placed in two different orbitals, energy is lower if the spins are parallel. are valid for (A) Aufbau principle (B) Pauli's exclusion principle (C) Hund's rule of maximum multiplicity (D) Heisenberg's uncertainty principle 322 The electrons would go to lower energy levels first and then to higher energy levels according to which of the following (A) Aufbau principle (B) Pauli's exclusion principle (C) Hund's rule of maximum multiplicity (D) Heisenberg's uncertainty principle
Effective Nuclear Charge
323. Effective nuclear charge of an atom depends on: (A) The atomic number of the atom (B) The charge on the ion (C) The shielding effect (D) Both the actual nuclear charge and the shielding effect 324.The screening effect of d-electrons is (A) equal to the p-electrons (B) more than p-electrons (C) same as f-electrons (D) less than p-electrons 325.In a given energy level, the order penetration effect of different orbitals is (A) f < d < p < s (B) s = p = d = f (C) s < p < d < f (D) p > s > d > f 326.Which one of the following group of atoms or ions is not isoelectronic?
(A) He, H–, Li+ (B) Na+, Mg2+, Al3+ (C) F–, O2–, N3– (D) K+, Ca2+, Ne 327 The size of isoelectronic species F–, Ne and Na+ is affected by : (A) nuclear charge (Z)
(B) valence principal quantum number (n) (C) electron-electron interaction in the outer orbitals (D) none of the factors because their size is the same. 328. Screening effect is not observed in : (A) He+ (B) Li2+ (C) Be3+ (D) In all cases 329. Which one of the following sets of ions represents a collection of isoelectronic species?
330. Which statement is false:- (A) Screening effect increases down the group (B) Zeff increases down the group (C) Zeff. increases in a period (D) None 331. The formula for effective nuclear charge is (if s is screening constant)
(A) Z - s (B) Z + s (C) Z s -1 (D) Z s 332. Effective nuclear charge in group generally (A) Increases down the group (B) Decreases down the group (C) Remains constant (D) First increases than decreases 333. In sodium atom the screening is due to :-
(A) 3s2, 3p6 (B) 2s1 (C) 1s2, 2s2, 2p6 (D) 1s2, 2s2 334.The screening effect of d- electrons is :- (A) Equal to the p - electrons (B) Much more than p - electrons (C) Same as f - electrons (D) Less than p – electrons
335. K+, Ar, Ca2+ and S2– contains _ (A) Same electronic configuration and atomic volume (B) Different electronic configuration but same IP. (C) Same electronic configuration but different atomic volume (D) None 336.Which of the following is not different for an atom and its corresponding ion :- (A) Number of electrons (B) Nuclear charge (C) Ionization energy (D) Size 337.Which of the following is not isoelectronic series :-
(A) Cl— , P3-, Ar (B) N3-, Ne, Mg+2 (C) B+3, He, Li+ (D) N3-, S2-, Cl— 338.The screening effect of s orbital electron is :- (A) Greater than p but lesser than d and f electrons (B) Less than p, d and f electrons (C) Greater than p, d and f electrons (D) Is equal to p , d and f electrons
339. Which one of the following groups represent a collection of isoelectronic species ?
(A) N3–, F–, Na+ (B) Be, Al3+, Cl– (C) Ca2+, Cs+, Br (D) Na+, Ca2+, Mg2+ 340.Which statement is false : (A) Screening effect increases down the group (B) Zeff increases down the group (C) Zeff. increases in a period (D) none 341.The best reason to account for the general tendency of atomic diameters to decrease as the atomic numbers increase within a period of the periodic table is the fact that (A) Outer electrons repel inner electron (B) Closer packing among the nuclear particles is achieved (C) The number of neutrons increases (D) The increasing nuclear charge exerts a greater attractive force on the electrons 342. Incorrect statement is (A) Atomic size ∝ Zeff (B) Atomic size ∝ negative charge
(C) Atomic size ∝ (D) Atomic size ∝ Screening effect 343. Which of the following is generally true regarding effective nuclear charge (Zeff) : (A) It increases on moving left to right in a period. (B) It remains almost constant on moving top to bottom in a group. (C) For isoelectronic species, as Z increases, Zeff decreases. (D) Both (A) and (B). 344 Among following species which of them have maximum Zeff. (A) Sn (B) Sn4+ (C) In (D) In+ 345 From the given set of species, point out the species from each set having highest Zeff (A) O2–, F–, Na+ (B) Li, Be, Na (C) He, Li+, H–
a b c a b c (A) Na+ Be Li+ (B) O2– Li H– (C) F– Na He (D) Na+ Be He
346 The group having isoelectronic species is: (A) O2–, F– , Na+ Mg2+ (B) O–, F–, Na+, Mg2+ (C) O2–, F– , Na+, Mg2+ (D) O–, F–, Na+ Mg+2
347.Which of the following have higher Zeff than Fluorine. (A) Cl (B) O (C) F– (D) none of these 348. Maximum size of first member of a period is due to (A) Maximum number of shells (B) Maximum screening effect (C) Minimum Zeff (D) All
Ions
349.Electronic configuration of H– is
(A) 1s0 (B)1s1 (C) 1s2 (D) 1s12s1
350.The electronic configuration of calcium ion (𝐶𝑎(8) is (A) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝3, 4𝑠( (B) 1𝑠(, 2𝑠(𝑠𝑝3, 3𝑠(3𝑝3, 4𝑠! (C) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑( (D) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝3, 4𝑠' 351.Which of the following ions is not having the configuration of neon (A) F– (B)Mg+2 (C) Na+ (D) Cl–
352.Ions which have the same electronic configuration are those of (A) Lithium and sodium (B) Sodium and potassium
(C) Potassium and calcium (D) Oxygen and chlorine
353.Cu2+ will have the following electronic configuration
(A) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑!' (B) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑7, 4𝑠! (C) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑7 (D) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑!', 4𝑠! 354.Which one is the electronic configuration of Fe+2 (A) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑3 (B) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑&, 4𝑠( (C) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑$, 4𝑠! (D) None of these 355.The electronic configuration (outermost) of Mn+2 ion (atomic number of Mn = 25) in its ground state is (A) 3d5, 4s0 (B) 3𝑑&, 4𝑠! (C) 3𝑑#, 4𝑠( (D) 3𝑑(, 4𝑠(4𝑝( 356.An ion has 18 electrons in the outermost shell, it is (A) Cu+ (B) Th4+ (C) Cs+ (D) K+
357.Correct configuration of Fe+3 [26] is (A) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑$ (B) 1𝑠(, 2𝑠(𝑠𝑝3, 3𝑠(3𝑝33𝑑#, 4𝑠( (C) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑3, 4𝑠( (D) 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝33𝑑$, 4𝑠! 358.What is the electronic configuration of Cu2+(Z = 29) of least position (A) [𝐴𝑟]4𝑠!3𝑑% (B) [𝐴𝑟]4𝑠(3𝑑!'4𝑝! (C) [𝐴𝑟]4𝑠!3𝑑!' (D) [𝐴𝑟]3𝑑7 359.Electronic configuration of ferric ion is (A) [𝐴𝑟]3𝑑$ (B) [𝐴𝑟]3𝑑" (C) [𝐴𝑟]3𝑑# (D) [𝐴𝑟]3𝑑% 360.Which one pair of atoms or ions will have same configuration (A) 𝐹8 and Ne (B) Li+ and He– (C) Cl– and Ar (D) Na and K 361.3𝑑!'4𝑠' electronic configuration exhibits by (A) Zn++ (B) Cu++ (C) Cd++ (D) Hg++
362.The number of d electrons in Fe+2 (atomic number of Fe = 26) is not equal to that of the (A) p-electrons in Ne (B) s-electrons in Mg (C) d-electrons in Fe (D) p-electrons in Cl– 363.A transition metal X has a configuration [𝐴𝑟]3𝑑& in its +3 oxidation state. Its atomic number is (A) 25 (B) 26 (C) 22 (D) 19
364.Which set has the same number of s-electrons (A) C, Cu2+, Zn (B) Cu2+ , Fe2+,Ni2+ (C) S2– , Ni2+,Zn (D) None of these 365.Among the following transition metal ions, the one set where all the metal ions have 3d2 electronic configuration is [At Nos. Ti = 22, V = 23, Cr = 24, Mn = 25 (A) Ti3+, V2+, Cr3+, Mn4+ (B) Ti4+, V4+, Cr+6, Mn7+ (C) Ti4+, V3+, Cr2+, Mn3+ (D) Ti2+, V3+, Cr4+, Mn5+ 366.The number of d-electrons in Fe2+ (Z=26) is not equal to the number of electrons in which one of the following? (A) p - electrons in Cl (Z=17) (B) d-electrons in Fe (Z=26) (C) p-electrons in Ne (Z=10) (D) s-electrons in Mg (Z=12) 367 Which of the following ion has inert gas configuration and having complete octet. (A) B+3 (B) Al+3 (C) Ga+3 (D) All of these 368 Which of the following set of species is not isoelectronic ? (A) Cu+, Zn2+, Ga3+ (B) N3–, Ne, Mg2+ (C) N3–, S2–, Cl– (D) He, Li+, H– 369. Which one of the following ion have 2 electrons in outermost shell and 18 electron in penultimate shell ? (A) Fe2+ (B) Sn2+ (C) Zn2+ (D) Mg2+ 370. Z/e ratio for N3–, O2– and F– respectively will be -
(A) 0.7, 0.8 and 0.9 (B) 0.9, 0.8 and 0.7 (C) 7, 8 and 9 (D) 9, 8 and 7
Magnetic moment
371. How many unpaired electrons are present in Ni2+ cation (atomic number = 28) (A) 0 (B) 2 (C) 4 (D) 6 372. The number of unpaired electrons in a chromic ion Cr3+ (atomic number = 24) is (A) 6 (B) 4 (C) 3 (D) 1 373. Which of the following metal ions will have maximum number of unpaired electrons (A) Fe+2 (B) Co+2 (C) Ni+2 (D) Mn+2
374. Which of the metal ion will have highest number of unpaired electrons (A) Cu+ (B) Fe2+ (C) Fe3+ (D) Co2+
374. Which of the following has the maximum number of unpaired electrons (A) Mg2+ (B) Ti3+ (C) V3+ (D) Fe2+ 376. Which of the following has more unpaired d-electrons (A) Zn+ (B) Fe2+ (C) N3+ (D) Cu+
377. The number of unpaired electrons in Fe3+ (Z = 26) are (A) 5 (B) 6 (C) 3 (D) 4 378 Number of unpaired electrons in Mn4+ is
(A) 3 (B) 5 (C) 6 (D) 4 379. Which of the following ions has the maximum number of unpaired d-electrons? (A) Zn2+ (B) Fe2+ (C) Ni3+ (D) Cu+ 380. Ratio of number of unpaired electrons in Fe2+ to that of Ti is (A) 1.2 (B) 3 (C) 2 (D) 4 381. Magnetic moment of Xn+ (Z = 26) is √24 B.M. Hence number of unpaired electrons and value of n respectively are : (A) 4, 2 (B) 2, 4 (C) 3, 1 (D) 0, 2 382. A compound of Vanadium has a spin magnetic moment 1.73 BM. Work out the electronic configuration of the Vanadium ion in the compound : (A)1s22s22p63s23p64s1 (B) 1s22s22p63s23p63d2 (C) 1s22s22p63s23p63d1 (D) nothing can be said with certainty 383. Magnetic moment 2.84 B.M. is given by (At. nos, Ni =28, Ti= 22, Cr =24, Co = 27 ) (A) Ti3+ (B) Cr2+ (C) Co2+ (D) Ni2+ 384. A compound of metal ion MX+ ( Z= 24) has a spin only magnetic moment of √15 Bohr Magnetons. The number of unpaired electrons in the compound are (A) 2 (B) 4 (C) 5 (D) 3 385. A gas metal in bivalent state have approximately 23e– what is spin magnetic moment in elemental state (A) 2.87 (B) 5.5 (C) 5.9 (D) 4.9 386. What is the total spin value in case of 26Fe3+ ion. (A) +1 or –1 (B) +2 or –2 (C) + 2.5 or – 2.5 (D) +3 or –3 387. A compound of vanadium has a magnetic moment of 1.73 BM. What will be the electronic configurations: (A) 1s2 2s2 2p6 3s2 3p6 3d1 (B) 1s2 2s2 2p6 3s2 3p6 3d2
388. Which of the following is electronic configuration of Cu2+ (Z = 29) ? (A) [Ar]4s1 3d8 (B) [Ar]4s2 3d10 4p1 (C) [Ar]4s1 3d10 (D) [Ar] 3d9 389. Spin magnetic moment of Xn+ (Z = 26) is √24 B.M. Hence number of unpaired electrons and value of n respectively are : (A) 4, 2 (B) 2, 4 (C) 3, 1 (D) 0, 2 390. Which of the following ions has the maximum number of unpaired d-electrons? (A) Zn2+ (B) Fe2+ (C) Ni3+ (D) Cu+ 391. The possible value of l and m for the last electron in the Cl– ion are : (A) 1 and 2 (B) 2 and +1 (C) 3 and –1 (D) 1 and –1 392. Which of the following has maximum number of paired electrons. (A) Cu+ (B) Fe2+ (C) Zr+ (D) Sc+ 393. A correct set of four quantum numbers for unpaired electron in Cl-atom :
n l m s n l m s (A) 3 2 0 +½ (B) 3 1 0 +½ (C) 3 1 +1 0 (D) 3 0 –1 +½ 394. The value of the spin magnetic moment of a particular ion is 2.83 Bohr magneton. The ion is : (A) Fe2+ (B) Ni2+ (C) Mn2+ (D) Co3+ 395. If element 25X+Y has spin magnetic moment 1.732 B.M then (A) number of unpaired electron = 1 (B) number of unpaired electron = 2 (C) Y = 4 (D) Y = 6 396. Which of the following statement(s) is incorrect? (A) The electronic configuration of Cr is [Ar] (3d)5(4s)1. (Atomic number of Cr = 24) (B) The magnetic quantum number may have negative values. (C) In silver atom, 23 electrons have a spin of one type and 24 of the opposite type (D) None of these 397. Number of unpaired electrons in Mn4+ is (A) 3 (B)5 (C) 6 (D) 4
398. No. of unpaired electron in 1s2,2s2,2p4 (A) 4 (B) 2 (C) 0 (D) 1 399The correct set of quantum numbers for the unpaired electron of Xenon (single positive) ion
is n l m n l m
(A) 6 1 0 (B) 4 1 1 (C) 5 1 1 (D) 3 0 0 400 the species not having same number of d-electron in last possible filled d-subshell as in Zn. (A) Ga (B) Pd (C) Cd (D) Pt 401 Which of the following elements will have the same total number of electrons in 's' as well as 'd' subshells in the ground state electronic configuration? (A) Zn (B) Ni (C) Cr (D) Cu 401 Which of the following has maximum number of unpaired electrons : (A) Fe2+ (B) Fe3+. (C) Sc3+ (D) Cu2+
Valence Electron 403. An element has the electronic configuration 1𝑠(, 2𝑠(2𝑝3, 3𝑠(3𝑝(. Its valency electrons are
(A) 6 (B) 2 (C) 3 (D) 4 404. The following has zero valency (A) Sodium (B) Beryllium (C) Aluminum (D) Krypton 405. The number of electrons in the valence shell of calcium is (A) 6 (B) 8 (C) 2 (D) 4 406. The valence electron in the carbon atom are (A) 0 (B) 2 (C) 4 (D) 6 407. The structure of external most shell of inert gases is (A) 𝑠(𝑝# (B)𝑠(𝑝3 (C) 𝑠!𝑝( (D) 𝑑!'𝑠( 408. The four-quantum number for the valence shell electron or last electron of sodium (Z = 11) is (A)𝑛 = 2, 𝑙 = 1,𝑚 = −1, 𝑠 = − !
409. The magnetic quantum number for valency electrons of sodium is (A) 3 (B) 2 (C) 1 (D) 0 410. The four quantum numbers of the valence electron of potassium are
