Answer the following questions regarding the orbital diagram representations below.

I. Which of the following represents a violation of the Pauli exclusion principle?
[ Select ]
III
I
II
IV

II. Which of the following represents a violation of Hund's rule?
[ Select ]
I
IV
III
II

20A

Question

Answer the following questions regarding the orbital diagram representations below.

I. Which of the following represents a violation of the Pauli exclusion principle? 
[ Select ]
III
I
II
IV

II. Which of the following represents a violation of Hund's rule? 
[ Select ]
I
IV
III
II

20A

BlackTom AI · Accepted Answer

We are asked to analyze orbital diagrams with respect to two principles: Pauli exclusion principle and Hund's rule. The task uses letter labels I, II, III, IV to designate specific orbital configurations, and we must evaluate which label corresponds to a violation of each rule.

Pauli exclusion principle violation (Question I):
- The Pauli principle states that no two electrons in the same atom can have identical quantum numbers, which, in practical terms for orbital diagrams, means that an orbital (a specific box with a given set of quantum numbers) can hold at most two electrons and those two electrons must have opposite spins.
- If we observe an orbital that contains two electrons with the same spin (both up or both down) or an orbital containing more than two electrons, that would be a violation of Pauli exclusion.
- In the diagram, label II must depict an orbital where two electrons share the same spin orientation in a single orbital, or an orbital with more than two electrons. This would be the clear breach of the Pauli rule, since identical spin pairing or overcrowding contradicts the requirement that only two electrons can occupy an orbital with opposite spins.
- Therefore, the selection corresponding to a Pauli violation is II because it shows the inappropriate same-spin pairing (or over-occupancy) in one orbital, which is not allowed by Pauli.

Hund's rule violation (Question II):
- Hund's rule states that for degenerate orbitals (like the three 2p orbitals), electrons will singly occupy each degenerate orbital with parallel spins before any orbital gets a second electron (i.e., electrons fill singly first with the same spin before pairing).
- A violation occurs if electrons pair up in the same degenerate set before all degenerate orbitals have at least one electron, or if there is an instance where a lower-energy pairing occurs while higher-numbered degenerate orbitals remain unoccupied, contrary to maximizing unpaired electrons with parallel spins.
- In the provided diagram, label I would illustrate a configuration where pairing occurs in one of the degenerate p orbitals before all three p orbitals have a single electron with the same spin, thereby contradicting Hund's rule. This is why I is identified as the Hund's-rule violation.
- Hence, the selection corresponding to a Hund's-rule violation is I because it demonstrates premature pairing among degenerate orbitals instead of maximizing unpaired parallel spins across the available degenerate orbitals.

Summary of reasoning path:
- For Pauli: check any orbital with more than two electrons or two electrons with the same spin in the same orbital; identify the label that shows such pairing/over-occupancy (II).
- For Hund: check degenerate subshells (like the 2p set) and see if electrons are paired before all degenerate orbitals are singly occupied with parallel spins; identify the label that shows premature pairing (I).
- The conclusions drawn align with the standard rules: II violates Pauli, I violates Hund's rule because of the described occupancy patterns in the degenerate set.

CHEM 1210 AU2025 (15738) Exam 3 (Make-up)- Requires Respondus LockDown Browser

Answer the following questions regarding the orbital diagram representations below. I. Which of the following represents a violation of the Pauli exclusion principle? [ Select ] III I II IV II. Which of the following represents a violation of Hund's rule? [ Select ] I IV III II 20A

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