The graph shown below represents the variation of probability density, \( \Psi(r) \), with distance \( r \) of the electron from the nucleus. This represents:
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The shape of the probability density function is crucial in identifying atomic orbitals:
- 1s orbital: A single peak.
- 2s orbital: A peak, a node (zero probability at some radius), and then another peak.
- 3s orbital: Multiple peaks and nodes.
Step 1: Analyze the graph showing the variation of probability density \( \Psi(r) \) with distance \( r \). The graph shows a single peak, followed by a monotonic decrease, and then no further peaks. This is characteristic of a 2s orbital, where the probability density function first increases, reaches a peak, and then decreases after crossing a node (zero probability at some distance from the nucleus). Step 2: In contrast, a 1s orbital would have only a single peak and no node, while a 3s orbital would have multiple peaks and nodes. Therefore, the graph represents a 2s orbital.
