Q40. Indicate whether or not the following orbital diagrams are possible and explain. When possible, indicate the element it represents.

Background

Topic: Electron Configuration and Orbital Diagrams

This question tests your understanding of how electrons fill atomic orbitals according to the Aufbau principle, Pauli exclusion principle, and Hund's rule. You are asked to determine if the given orbital diagrams are possible and, if so, to identify the element they represent.

Key Terms and Principles:

• Aufbau Principle: Electrons fill orbitals starting with the lowest energy levels first.

• Pauli Exclusion Principle: Each orbital can hold a maximum of two electrons with opposite spins.

• Hund's Rule: Electrons will fill degenerate orbitals (orbitals of the same energy) singly before pairing up.

• Orbital Box Diagram: A visual representation of electron configuration, showing electrons as arrows in boxes representing orbitals.

Step-by-Step Guidance

1. Examine each diagram and count the total number of electrons represented by the arrows. This will help you determine the atomic number and, therefore, the element.

2. Check if the electrons are filling the orbitals in the correct order (1s, 2s, 2p, 3s, 3p, 4s, 3d, etc.) according to the Aufbau principle.

3. Verify that no orbital contains more than two electrons and that paired electrons have opposite spins (Pauli exclusion principle).

4. For p and d orbitals, ensure that electrons are placed singly in each orbital before any pairing occurs (Hund's rule).

5. For each diagram, decide if the arrangement is possible. If it is, use the total electron count to identify the element. If not, explain which rule is violated.

Try solving on your own before revealing the answer!