Electronic configuration Aufbau Pauli and Hund rules - One Line Questions
1.
How many electrons can a single 'p' orbital hold at maximum? —
2
2.
How many unpaired electrons are present in the ground state electronic configuration of Chromium (Z=24)? —
5
3.
According to Hund's rule, the p-subshell can accommodate a maximum of how many unpaired electrons? —
3
4.
Which of the following orbital filling orders is INCORRECT according to the Aufbau principle? —
1s, 2p, 2s, 3s, 3p, 4s
5.
Which of the following orbital filling sequences demonstrates the Aufbau principle correctly? —
1s, 2s, 2p, 3s
6.
The electronic configuration of Helium (Z=2) is: —
1s²
7.
Which of the following electronic configurations violates the Pauli Exclusion Principle? —
Two electrons in the same 1s orbital with opposite spins
8.
What is the electronic configuration of the ground state of the Oxygen ion (O²⁻)? (Atomic number of O is 8) —
1s² 2s² 2p⁶
9.
What is the electronic configuration of Nitrogen (Z=7)? —
1s² 2s² 2p³
10.
What is the electronic configuration of Fluorine (Z=9)? —
1s² 2s² 2p⁵
11.
What is the electronic configuration of the ground state of the Sodium ion (Na⁺)? (Atomic number of Na is 11) —
1s² 2s² 2p⁶
12.
What is the electronic configuration of a neutral atom of Phosphorus (Z=15)? —
1s² 2s² 2p⁶ 3s² 3p³
13.
The electronic configuration of Argon (Z=18) is: —
1s² 2s² 2p⁶ 3s² 3p⁶
14.
What is the electronic configuration of Scandium (Z=21)? —
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹
15.
The electronic configuration of Copper (Z=29) is an exception to the Aufbau principle. Its actual configuration is: —
1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰
16.
What is the maximum number of electrons that can be accommodated in the 'd' subshell? —
10
17.
How many electrons are there in the outermost shell of an atom with electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁴? —
6
18.
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? —
4s
19.
According to the Aufbau principle, the order of filling for 3d and 4s subshells is: —
4s then 3d
20.
What is the correct order of filling orbitals according to the (n+l) rule for n=3 and n=4? —
3s, 3p, 4s, 3d
21.
Which subshell is filled after 4p according to the Aufbau principle? —
5s
22.
According to the Aufbau principle, which subshell is filled after 3d? —
4s
23.
According to the Aufbau principle, which subshell is filled after the 3p subshell? —
4s
24.
What is the correct order of filling the 4th energy level's subshells according to the Aufbau principle? —
4s, 3d, 4p, 4f
25.
Which subshell is filled immediately after the 4f subshell according to the Aufbau principle? —
6s
26.
According to the Aufbau principle, which subshell is filled after 5s? —
4d
27.
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? —
13
28.
Hund's Rule of Maximum Multiplicity states that electron pairing in degenerate orbitals begins only when: —
all orbitals in a subshell are singly occupied
29.
Which of the following represents a violation of Hund's Rule? —
An orbital with two electrons, another with two electrons, and one with one electron.
30.
The electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ represents which element? —
Potassium (K, Z=19)
31.
Which element has the electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p³? —
Arsenic (As, Z=33)
32.
Which principle states that in the ground state of an atom, no two electrons can have the same set of four quantum numbers? —
Pauli Exclusion Principle
33.
When filling degenerate orbitals, electrons will occupy separate orbitals with parallel spins before pairing up. This is a statement of: —
Hund's Rule
34.
Which principle is violated if two electrons in the same orbital have the same spin direction? —
Pauli Exclusion Principle
35.
Which rule states that electrons will enter degenerate orbitals one by one with parallel spins before pairing up? —
Hund's Rule
36.
The electronic configuration of an atom cannot have two electrons in the same orbital with the same spin. This is the statement of: —
Pauli Exclusion Principle
37.
The Aufbau principle is based on the idea that: —
electrons fill orbitals starting from the lowest energy levels
38.
Hund's Rule is a consequence of: —
exchange energy and spin alignment
39.
The electronic configuration 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s¹ is characteristic of which element? —
Manganese (Z=25)
40.
For a given principal quantum number 'n', the order of filling of subshells is generally determined by: —
n+l rule
41.
Which of the following sets of quantum numbers is NOT allowed for an electron in an atom, according to the Pauli Exclusion Principle? —
n=1, l=0, ml=0, ms=+1/2 and n=1, l=0, ml=0, ms=+1/2
42.
Which element's ground state electronic configuration violates Hund's Rule? —
Oxygen (Z=8)
43.
Which rule dictates that electrons will fill orbitals in such a way as to minimize the total energy of the atom? —
Aufbau Principle
44.
Which of the following is an exception to the Aufbau principle due to the extra stability of a half-filled or fully-filled subshell? —
Chromium (Z=24)
45.
Which of the following statements about the electronic configuration of atoms is FALSE? —
Hund's Rule dictates that electrons pair up in degenerate orbitals as soon as possible.
46.
The n+l rule is particularly useful for predicting the filling order of orbitals in: —
elements with complex electronic structures
47.
The electronic configuration of an atom describes: —
the arrangement of electrons in various atomic orbitals
48.
The Pauli Exclusion Principle is crucial for determining: —
the maximum number of electrons in a subshell
49.
If an orbital contains two electrons, what must be true about their spins according to the Pauli Exclusion Principle? —
They must have opposite spins.
50.
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? —
One electron in each of the three orbitals, with two having parallel spins and one paired.