The orbital diagram in which both the pauli's exclusion principal and Hund's rule are violated is :

Options

A.
B.
C.
D.

Answer

To solve the question regarding the orbital diagram that violates both Pauli's exclusion principle and Hund's rule, we will follow these steps:

### Step 1: Understand the Pauli Exclusion Principle
The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of all four quantum numbers. This means that if two electrons occupy the same orbital, they must have opposite spins.

**Hint:** Remember that the spins of electrons in the same orbital must be opposite.

### Step 2: Understand Hund's Rule
Hund's Rule states that electrons will fill degenerate orbitals (orbitals of the same energy) singly before pairing up. This means that each orbital in a subshell should have one electron before any orbital has two electrons.

**Hint:** Focus on how electrons fill orbitals; they must occupy each orbital singly before pairing.

### Step 3: Analyze the Options
Now, we will analyze the given options to identify which one violates both principles.

1. **Option 1:** Both electrons have opposite spins in the same orbital.
- This does not violate either principle.

2. **Option 2:** Electrons have opposite spins and are correctly distributed.
- This does not violate either principle.

3. **Option 3:** Electrons are paired before each orbital is singly occupied.
- This violates Hund's rule but not the Pauli exclusion principle.

4. **Option 4:** Electrons have the same spin in the same orbital.
- This violates both the Pauli exclusion principle (same spin in the same orbital) and Hund's rule (incorrect filling of orbitals).

### Step 4: Conclusion
Based on the analysis, **Option 4** is the correct answer as it violates both the Pauli exclusion principle and Hund's rule.

**Final Answer:** The orbital diagram in which both the Pauli's exclusion principle and Hund's rule are violated is **Option 4**.