in a set of degenerate orbitals the electrons distribute themselves to retail similar spins as far as possible. This statement is attributed to

Options

A. Pauli's exclusion principle
B. hunds rule
C. Aufbau principle
D. slaters rule

Answer

To answer the question, we need to identify the principle that states that in a set of degenerate orbitals, electrons will fill these orbitals singly with the same spin before pairing up. This principle is known as Hund's Rule.

### Step-by-Step Solution:

1. **Understanding Degenerate Orbitals**: Degenerate orbitals are orbitals that have the same energy level. For example, the three p orbitals (px, py, pz) or the five d orbitals (dxy, dyz, dzx, dx2-y2, dz2) are considered degenerate.

2. **Electron Configuration**: When filling these degenerate orbitals with electrons, the electrons will first occupy each orbital singly. This is to minimize electron-electron repulsion.

3. **Similar Spins**: According to Hund's Rule, when electrons occupy degenerate orbitals, they will fill them with the same spin (either all spin-up or all spin-down) before pairing up. This means that if you have three degenerate orbitals and you are adding electrons, the first three electrons will each go into one of the three orbitals with the same spin.

4. **Filling Order**: After all degenerate orbitals have one electron, the next electrons will then start to pair up in the orbitals. For example, if you have three p orbitals and you are filling them with six electrons, the first three will have the same spin, and the next three will pair up with opposite spins.

5. **Conclusion**: The statement in the question is attributed to Hund's Rule, which emphasizes that electrons will occupy degenerate orbitals singly with the same spin before pairing up.

### Final Answer:
The statement is attributed to **Hund's Rule**.