Step 1: Understanding the Question:
Nodes are regions in space around the nucleus where the probability of finding an electron is zero. Step 2: Key Formula or Approach:
- Radial nodes = \( n - l - 1 \)
- Angular nodes = \( l \)
- Total nodes = \( n - 1 \)
Where \( n \) is the principal quantum number and \( l \) is the azimuthal quantum number. Step 3: Detailed Explanation:
For a \( 2s \) orbital:
- \( n = 2 \)
- For an s-orbital, \( l = 0 \)
Calculation:
Total nodes = \( 2 - 1 = 1 \).
(Specifically, this is one radial node). Step 4: Final Answer:
The number of nodes in the \( 2s \) orbital is 1.