Question

No two electrons in an atom can have the same set of quantum numbers. This is known as:

• A. Hund's rule
• B. Pauli's exclusion principle
• C. Aufbau principle
• D. Heisenberg's principle
• E. Fajan's rule

Hint:

Pauli's exclusion principle is fundamental in determining the electron configuration in atoms. It ensures that each electron in an atom has a unique quantum state.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept:
Quantum numbers act as a unique address for an electron within an atom, defined by principal (\(n\)), azimuthal (\(l\)), magnetic (\(m_{l}\)), and spin (\(m_{s}\)) numbers.
We need to identify the specific scientific principle that forbids two electrons from sharing all four numbers.
Step 2: Key Formula or Approach:
The approach involves identifying the standard definition of the quantum mechanical principles provided in the options.
No calculation is required.
Step 3: Detailed Explanation:
Let us review the definitions of the principles given.
Hund's rule dictates that electrons fill degenerate orbitals singly before pairing up.
The Aufbau principle states that electrons fill lower-energy atomic orbitals first.
Heisenberg's principle states that the exact position and momentum of an electron cannot be simultaneously determined.
Pauli's exclusion principle strictly states that no two electrons in a single atom can have an identical set of all four quantum numbers.
If two electrons occupy the exact same orbital (sharing \(n\), \(l\), and \(m_{l}\)), they must have opposite spins (different \(m_{s}\)).
Step 4: Final Answer:
The statement perfectly describes Pauli's exclusion principle.