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Quizzes > Science > Chemistry

Which Electron Configuration Violates Hund's Rule? Take the Quiz!

Test Your Skills on Hund's Rule, Pauli Exclusion & Aufbau - Dive In!

Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art style electron orbitals on dark blue background quiz inviting to spot Hunds Rule violation in configurations

Think you know Hund's rule inside out? Take our quiz to discover which electron configuration violates Hund's rule while reinforcing pauli exclusion aufbau hund rule essentials. Apply Hund's rule electron configuration concepts and tackle electron configuration Hund rule scenarios to separate correct setups from rule-breaking examples. Sharpen your skills with detailed electron configuration questions and delve into the excited state of electron configuration. Perfect for students eager to test their knowledge and boost confidence, this quick electron configuration quiz is your gateway to mastery. Ready to prove your expertise? Take the quiz now and see if you can spot the rule-breaker!

Which of the following orbital assignments for two electrons in p orbitals violates Hund's rule?
px^1 py^1 pz^0
px^2 py^0 pz^0
px^0 py^1 pz^1
px^1 py^0 pz^1
Hund's rule states that electrons occupy separate orbitals within a subshell before pairing. In the px^2 py^0 pz^0 assignment, both electrons are in the same p orbital although there are empty degenerate orbitals available, which violates Hund's rule. The correct distribution places one electron into two distinct p orbitals before any pairing occurs. For more details, see Hund's Rule.
Which of the following scenarios violates Hund's rule?
Electrons fill lower energy orbitals completely before higher ones.
Two electrons are paired in one 3p orbital while another 3p orbital remains empty.
Electrons remain unpaired in f orbitals as much as possible.
No two electrons in an atom share all four quantum numbers.
Hund's rule requires that degenerate orbitals are occupied singly before any pairing occurs. Pairing two electrons into the same 3p orbital while leaving an empty 3p orbital violates this rule. The other scenarios describe the Aufbau principle, the Pauli exclusion principle, and the proper application of Hund's rule to f orbitals respectively. See Chemistry LibreTexts for more information.
Which of the following 2p electron distributions for an oxygen atom violates Hund's rule?
px^1 py^1 pz^2
px^2 py^1 pz^1
px^2 py^2 pz^0
px^1 py^2 pz^1
Oxygen has four electrons in its 2p subshell and by Hund's rule, each 2p orbital should receive one electron before any orbital gets a second. The px^2 py^2 pz^0 distribution pairs electrons in two orbitals while leaving one orbital empty, which violates Hund's rule. The correct configuration is px^2 py^1 pz^1 after each orbital is singly occupied. More on Hund's rule and p orbital filling can be found at Wikipedia.
Which of the following complete electron configurations explicitly shows a violation of Hund's rule?
1s2 2s2 2p1
1s2 2s2 2p4
1s2 2s2 2p3
1s2 2s2 2px2 2py0 2pz0
The notation 1s2 2s2 2px2 2py0 2pz0 shows two electrons paired in one p orbital before the other two degenerate p orbitals receive any electrons, violating Hund's rule. The other configurations either follow Hund's rule or do not specify an explicit violation. Hund's rule applies to the filling of degenerate orbitals where maximum multiplicity is favored. For more, see Chemistry LibreTexts.
Which of the following d2 orbital diagrams violates Hund's rule?
0 ? 0 ? 0
? ? 0 0 0
?? 0 0 0 0
? 0 ? 0 0
In a d2 configuration, Hund's rule requires that the two electrons occupy separate degenerate orbitals with parallel spins. The diagram ?? 0 0 0 0 shows both electrons paired in the same orbital while three degenerate orbitals remain empty, violating Hund's rule. The other diagrams distribute the electrons singly across different d orbitals, which is consistent with Hund's rule. See Hund's Rules for further details.
Which orbital diagram for a d5 configuration violates Hund's rule?
? ? 0 ? ?
? ? ? ? ?
? 0 ? 0 ?
?? ? ? ? 0
A d5 configuration should have one unpaired electron in each of the five degenerate d orbitals according to Hund's rule. The diagram ?? ? ? ? 0 pairs two electrons in one orbital before the fifth electron occupies the last empty orbital, violating Hund's rule. The other diagrams correctly place one electron in each orbital. More on this is available at Chemistry LibreTexts.
Which of the following subshells cannot exhibit a violation of Hund's rule due to having only one orbital?
d subshell
f subshell
p subshell
1s or any s subshell
Hund's rule applies to degenerate orbitals within a subshell. An s subshell contains only one orbital, so there are no degenerate orbitals to distribute electrons among, and thus no possibility of a Hund's rule violation. In contrast, p, d, and f subshells have multiple degenerate orbitals where violations can occur. For more details, see Chemistry LibreTexts.
Which of the following f orbital distributions for an f2 configuration violates Hund's rule?
0 ? ? 0 0 0 0
? 0 ? 0 0 0 0
? ? 0 0 0 0 0
?? 0 0 0 0 0
Hund's rule requires that each electron occupies a separate degenerate orbital with parallel spins before any pairing occurs. The configuration ?? 0 0 0 0 0 has both electrons paired in the same f orbital while other degenerate f orbitals remain empty, which violates Hund's rule. The other distributions correctly place the two electrons in separate orbitals. Visit Wikipedia for more information.
Which of the following scenarios is an example of a violation of Hund's rule?
Maximal unpaired electrons in the 3d subshell
Electrons in the 1s orbital being paired
Pairing two electrons in a 3p orbital while another 3p orbital is empty
Electrons occupying lower energy orbitals before higher ones
Hund's rule dictates that electrons fill degenerate orbitals singly before any orbital receives a second electron. Pairing two electrons in one 3p orbital while leaving another 3p orbital empty clearly violates this rule. Filling lower-energy orbitals first follows the Aufbau principle, and pairing in the 1s orbital is mandated by the Pauli exclusion principle since there is only one 1s orbital. Maximizing unpaired electrons in the 3d subshell exemplifies correct application of Hund's rule. See Hund's Rules.
Which of the following orbital diagrams for a 3d4 configuration violates Hund's rule?
? ? ? ? 0
?? ? ? 0 0
? ? 0 ? 0
? 0 ? ? 0
For a 3d4 configuration, Hund's rule requires four electrons to occupy separate orbitals with parallel spins before any pairing occurs. The diagram ?? ? ? 0 0 pairs two electrons in one orbital while a degenerate orbital remains empty, violating Hund's rule. The other diagrams correctly distribute electrons singly across distinct orbitals. More information is available at Chemistry LibreTexts.
Which of the following f orbital distributions for an f6 configuration violates Hund's rule while respecting the Pauli exclusion principle?
?? ? ? ? ? 0
0 ? ? ? ? ? ?
? ? 0 ? ? ? 0
? ? ? ? ? ? 0
In an f6 configuration, Hund's rule demands one electron in each of the first six degenerate f orbitals with parallel spins before any orbital is paired. The configuration ?? ? ? ? ? 0 pairs two electrons in one orbital while another orbital stays singly occupied, satisfying the Pauli exclusion principle but violating Hund's rule. The other distributions respect the requirement of maximizing unpaired electrons. See Hund's Rules for more information.
Which of the following ground-state electron configurations is often mistaken as a violation of Hund's rule but is actually explained by exchange energy stabilization?
[Ar] 4s2 3d4
[Ar] 4s2 3d5 (Manganese)
[Ar] 4s1 3d5 (Chromium)
[Ar] 4s1 3d4
Chromium's ground-state configuration [Ar] 4s1 3d5 appears to break the simple aufbau order but does not violate Hund's rule, as the 3d subshell still maximizes unpaired electrons. The exception is due to extra exchange energy gained by having a half-filled d subshell, not a violation of Hund's rule. The configurations [Ar]4s2 3d4 and [Ar]4s2 3d5 or 4s1 3d4 either follow normal filling or do not represent chromium. More details can be found at Chromium Electron Configuration.
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Study Outcomes

  1. Identify Hund's Rule Violations -

    Pinpoint which electron configurations violate Hund's rule by recognizing uneven spin distributions in degenerate orbitals.

  2. Apply the Pauli Exclusion Principle -

    Use the Pauli exclusion principle to ensure no two electrons in the same orbital share identical quantum numbers.

  3. Implement the Aufbau Principle -

    Arrange electrons in orbitals correctly by following the Aufbau filling order from lowest to highest energy levels.

  4. Analyze Spin Pairing -

    Evaluate how electrons pair in orbitals and distinguish between allowed and disallowed spin configurations.

  5. Reinforce Core Concepts -

    Review and solidify the interplay between Hund's rule, the Pauli exclusion principle, and the Aufbau principle through targeted quiz questions.

Cheat Sheet

  1. Hund's Rule Fundamentals -

    Hund's rule electron configuration teaches that electrons occupy degenerate orbitals singly before pairing to minimize repulsion. For example, in the 2p subshell of carbon (1s2 2s2 2p2), both electrons occupy separate orbitals with parallel spins. A handy mnemonic is "fill seats on the bus one by one before doubling up."

  2. Pauli Exclusion Principle Insights -

    The pauli exclusion aufbau hund rule dictates that no two electrons in an atom can share the same four quantum numbers. This means each orbital can hold a max of two electrons with opposite spins (↑↓). Understanding this prevents errors like assigning three electrons to a single orbital in an electron configuration quiz.

  3. Aufbau Principle in Action -

    The Aufbau principle specifies filling orbitals from lowest to highest energy, following the n+l rule and diagonal guide. For instance, 4s fills before 3d, yielding 1s2 2s2 2p6 3s2 3p6 4s2. Mastering this order helps you spot when an electron configuration violates Hund's rule by also mixing up energy levels.

  4. Identifying Hund's Rule Violations -

    Which electron configuration violates Hund's rule? Look for subshells where electrons pair prematurely, such as writing 2p4 as (↑↓)(↑↓)( ) instead of the correct (↑↓)(↑)(↑) diagram. Such mistakes show paired electrons in lower orbitals before all are half-filled and indicate a conceptual slip.

  5. Quiz-Based Reinforcement -

    Engage with an electron configuration Hund rule quiz to reinforce these principles under exam conditions. Timing yourself while filling out configurations like Fe (1s2 2s2 2p6 3s2 3p6 4s2 3d6) can boost recall speed and accuracy. Frequent quizzing is one of the best ways to ensure you never mix up Aufbau, Hund's rule, and the pauli exclusion aufbau hund rule again!

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