Discuss the similarities and differences between a 1s and 2s orbital.

Explanation

### Step-by-Step Solution

**Step 1: Similarities between 1s and 2s orbitals**
- **Shape**: Both 1s and 2s orbitals have a spherical shape. This means that the probability of finding an electron is distributed uniformly in all directions around the nucleus.
- **Orbital Angular Momentum**: The azimuthal quantum number (L) for both 1s and 2s orbitals is 0, as they belong to the s subshell. The formula for orbital angular momentum is given by \( \sqrt{L(L+1)} \frac{h}{2\pi} \). Since L = 0 for both orbitals, the orbital angular momentum is 0 for both 1s and 2s.

**Step 2: Differences between 1s and 2s orbitals**
- **Size**: The 2s orbital is larger than the 1s orbital. As the principal quantum number (n) increases, the size of the orbital also increases. Therefore, the 2s orbital has a greater radius compared to the 1s orbital.
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