Electronic configuration Aufbau Pauli and Hund rules - Question Bank

1. Which subshell is filled immediately after the 4f subshell according to the Aufbau principle?
A) 5d
B) 6s
C) 5p
D) 4g
2. What is the electronic configuration of a neutral atom of Phosphorus (Z=15)?
A) 1s² 2s² 2p⁶ 3s² 3p³
B) 1s² 2s² 2p⁵ 3s² 3p³
C) 1s² 2s² 2p⁶ 3s³ 3p²
D) 1s² 2s² 2p⁶ 3s² 3d³
3. The electronic configuration of an atom cannot have two electrons in the same orbital with the same spin. This is the statement of:
A) Aufbau Principle
B) Hund's Rule
C) Pauli Exclusion Principle
D) Madelung Rule
4. Which of the following orbital filling sequences demonstrates the Aufbau principle correctly?
A) 1s, 3s, 2s, 2p
B) 1s, 2s, 3s, 2p
C) 1s, 2s, 2p, 3s
D) 1s, 2p, 2s, 3s
5. What is the total number of electrons in the 3rd shell (n=3) of an atom if its electronic configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹?
A) 8
B) 11
C) 13
D) 18
6. Hund's Rule is a consequence of:
A) electrostatic repulsion between electrons
B) exchange energy and spin alignment
C) the uncertainty principle
D) the quantization of energy levels
7. Which element has the electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p³?
A) Arsenic (As, Z=33)
B) Selenium (Se, Z=34)
C) Bromine (Br, Z=35)
D) Krypton (Kr, Z=36)
8. If an orbital contains two electrons, what must be true about their spins according to the Pauli Exclusion Principle?
A) They must have the same spin.
B) They must have opposite spins.
C) One must be spin up, the other spin down.
D) They can have either same or opposite spins.
9. The n+l rule is particularly useful for predicting the filling order of orbitals in:
A) the first 10 elements
B) the first transition series
C) elements with complex electronic structures
D) all elements
10. What is the electronic configuration of Scandium (Z=21)?
A) 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹ 4s²
B) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s³
D) 1s² 2s² 2p⁶ 3s² 3p⁵ 4s² 3d²
11. Which of the following statements about the electronic configuration of atoms is FALSE?
A) The Aufbau principle guides the filling of orbitals in order of increasing energy.
B) The Pauli Exclusion Principle limits the number of electrons in an orbital to two, with opposite spins.
C) Hund's Rule dictates that electrons pair up in degenerate orbitals as soon as possible.
D) The electronic configuration determines the chemical properties of an element.
12. According to the Aufbau principle, the order of filling for 3d and 4s subshells is:
A) 3d then 4s
B) 4s then 3d
C) Simultaneously
D) Depends on the element
13. The electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹ is characteristic of which element?
A) Manganese (Z=25)
B) Iron (Z=26)
C) Cobalt (Z=27)
D) Molybdenum (Z=42)
14. What is the electronic configuration of the ground state of the Oxygen ion (O²⁻)? (Atomic number of O is 8)
A) 1s² 2s² 2p²
B) 1s² 2s² 2p⁴
C) 1s² 2s² 2p⁶
D) 1s² 2s¹ 2p⁶
15. Which rule states that electrons will enter degenerate orbitals one by one with parallel spins before pairing up?
A) Aufbau Principle
B) Pauli Exclusion Principle
C) Hund's Rule
D) Laporte Rule
16. According to the Aufbau principle, which subshell is filled after 5s?
A) 5p
B) 4d
C) 5d
D) 4f
17. The electronic configuration of Argon (Z=18) is:
A) 1s² 2s² 2p⁶ 3s² 3p⁶
B) 1s² 2s² 2p⁶ 3s¹ 3p⁷
C) 1s² 2s² 2p⁵ 3s² 3p⁷
D) 1s² 2s² 2p⁶ 3s² 4s²
18. Which of the following represents a violation of Hund's Rule?
A) An orbital with two electrons and one with one electron.
B) Three orbitals each containing one electron with parallel spins.
C) An orbital with two electrons and two orbitals each with one electron.
D) An orbital with two electrons, another with two electrons, and one with one electron.
19. What is the correct order of filling orbitals according to the (n+l) rule for n=3 and n=4?
A) 3s, 3p, 3d, 4s
B) 4s, 3s, 3p, 3d
C) 3s, 3p, 4s, 3d
D) 3s, 4s, 3p, 3d
20. The electronic configuration of Copper (Z=29) is an exception to the Aufbau principle. Its actual configuration is:
A) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁹
B) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰
C) 1s² 2s² 2p⁶ 3s² 3p⁶ 4s⁰ 3d¹¹
D) 1s² 2s² 2p⁶ 3s² 3p⁶ 4p¹ 3d¹⁰
21. Which of the following electronic configurations violates the Pauli Exclusion Principle?
A) 1s²
B) 2s¹
C) 2p⁶
D) Two electrons in the same 1s orbital with opposite spins
22. How many electrons are there in the outermost shell of an atom with electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁴?
A) 2
B) 4
C) 6
D) 8
23. The Aufbau principle is based on the idea that:
A) electrons are arranged in specific orbits
B) electrons fill orbitals starting from the lowest energy levels
C) no two electrons can have identical quantum numbers
D) electrons in degenerate orbitals have parallel spins
24. The electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ represents which element?
A) Argon (Ar, Z=18)
B) Potassium (K, Z=19)
C) Calcium (Ca, Z=20)
D) Scandium (Sc, Z=21)
25. Which subshell is filled after 4p according to the Aufbau principle?
A) 4d
B) 5s
C) 4f
D) 5p
26. According to Hund's rule, the p-subshell can accommodate a maximum of how many unpaired electrons?
A) 1
B) 2
C) 3
D) 6
27. What is the electronic configuration of Fluorine (Z=9)?
A) 1s² 2s² 2p⁵
B) 1s² 2s¹ 2p⁶
C) 1s² 2s² 2p³ 3s²
D) 1s² 2p⁷
28. Which principle is violated if two electrons in the same orbital have the same spin direction?
A) Aufbau Principle
B) Hund's Rule
C) Pauli Exclusion Principle
D) Bohr's Postulate
29. The 'n+l' rule is a guideline for predicting the order of filling of orbitals. Which subshell has the lowest energy according to this rule?
A) 3d
B) 4s
C) 4p
D) 5s
30. What is the electronic configuration of the ground state of the Sodium ion (Na⁺)? (Atomic number of Na is 11)
A) 1s² 2s² 2p⁶ 3s¹
B) 1s² 2s² 2p⁵
C) 1s² 2s² 2p⁶
D) 1s² 2s¹ 2p⁶
31. Which of the following is an exception to the Aufbau principle due to the extra stability of a half-filled or fully-filled subshell?
A) Potassium (Z=19)
B) Calcium (Z=20)
C) Chromium (Z=24)
D) Iron (Z=26)
32. The electronic configuration of Oxygen (Z=8) is 1s² 2s² 2p⁴. According to Hund's rule, how are the electrons distributed in the 2p subshell?
A) Three electrons in one orbital, one in another.
B) Two electrons in one orbital, one in each of the other two.
C) One electron in each of the three orbitals, with two having parallel spins and one paired.
D) One electron in each of the three orbitals, all with parallel spins.
33. How many unpaired electrons are present in the ground state electronic configuration of Chromium (Z=24)?
A) 1
B) 5
C) 6
D) 0
34. For a given principal quantum number 'n', the order of filling of subshells is generally determined by:
A) n+l rule
B) Pauli Exclusion Principle
C) Hund's Rule
D) Diagonal rule
35. Which rule dictates that electrons will fill orbitals in such a way as to minimize the total energy of the atom?
A) Pauli Exclusion Principle
B) Hund's Rule
C) Aufbau Principle
D) Coulomb's Law
36. The electronic configuration of Helium (Z=2) is:
A) 1s¹
B) 1s²
C) 1s¹ 2s¹
D) 2s²
37. According to the Aufbau principle, which subshell is filled after 3d?
A) 4p
B) 4s
C) 5s
D) 3f
38. What is the maximum number of electrons that can be accommodated in the 'd' subshell?
A) 2
B) 6
C) 10
D) 14
39. When filling degenerate orbitals, electrons will occupy separate orbitals with parallel spins before pairing up. This is a statement of:
A) Aufbau Principle
B) Pauli Exclusion Principle
C) Hund's Rule
D) Bohr's Model
40. Which of the following sets of quantum numbers is NOT allowed for an electron in an atom, according to the Pauli Exclusion Principle?
A) n=1, l=0, ml=0, ms=+1/2
B) n=2, l=1, ml=0, ms=-1/2
C) n=2, l=0, ml=0, ms=+1/2
D) n=1, l=0, ml=0, ms=+1/2 and n=1, l=0, ml=0, ms=+1/2
41. The electronic configuration of an atom describes:
A) the number of neutrons in the nucleus
B) the arrangement of electrons in various atomic orbitals
C) the charge of the nucleus
D) the mass of the atom
42. What is the correct order of filling the 4th energy level's subshells according to the Aufbau principle?
A) 4s, 4p, 4d, 4f
B) 4s, 4d, 4p, 4f
C) 4s, 3d, 4p, 4f
D) 4s, 4f, 4d, 4p
43. Which element's ground state electronic configuration violates Hund's Rule?
A) Oxygen (Z=8)
B) Nitrogen (Z=7)
C) Carbon (Z=6)
D) Fluorine (Z=9)
44. How many electrons can a single 'p' orbital hold at maximum?
A) 1
B) 2
C) 3
D) 6
45. The Pauli Exclusion Principle is crucial for determining:
A) the shape of atomic orbitals
B) the maximum number of electrons in a subshell
C) the energy levels of electrons
D) the magnetic properties of atoms
46. Which of the following orbital filling orders is INCORRECT according to the Aufbau principle?
A) 1s, 2s, 2p, 3s, 3p, 4s, 3d
B) 1s, 2s, 2p, 3s, 3p, 3d, 4s
C) 1s, 2s, 2p, 3s, 4s, 3d, 4p
D) 1s, 2p, 2s, 3s, 3p, 4s
47. What is the electronic configuration of Nitrogen (Z=7)?
A) 1s² 2s² 2p³
B) 1s² 2s³ 2p²
C) 1s¹ 2s² 2p⁴
D) 1s² 2p⁵
48. Hund's Rule of Maximum Multiplicity states that electron pairing in degenerate orbitals begins only when:
A) all orbitals in a subshell are half-filled
B) all orbitals in a subshell are completely filled
C) all orbitals in a subshell are singly occupied
D) the subshell contains more than five electrons
49. According to the Aufbau principle, which subshell is filled after the 3p subshell?
A) 4s
B) 3d
C) 4p
D) 3s
50. Which principle states that in the ground state of an atom, no two electrons can have the same set of four quantum numbers?
A) Aufbau Principle
B) Pauli Exclusion Principle
C) Hund's Rule of Maximum Multiplicity
D) Heisenberg Uncertainty Principle
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