The electrons are more likely to be found:

🧠 Finding the Dense Regions Wave mechanics tells us that electrons don't just "sit" in a circle. They exist in regions of probability. The radial probability distribution ($4\pi r^2 \psi^2$) specifically maps where you are most likely to find an electron at a certain distance ($r$) from the nucleus.

🗺️ Reading the Peaks and Valleys For a 2s orbital:

• Radial Nodes: $n - l - 1 = 2 - 0 - 1 = 1$. There is exactly one point where the probability drops to zero.
• Regions on Graph:
  • Region a (Peak 1): The "inner" probability density. Small, but very close to the nucleus (penetration effect).
  • Region b (Valley): The radial node. Probability $= 0$.
  • Region c (Peak 2): The "outer" probability density. Large and broad, representing where the valence electron spends most of its time.

Electrons inhabit the high-probability zones, which are the peaks. Thus, they are most likely found in a and c.

⚡ The Node-Counter Shortcut Any "s" orbital has $n$ regions of electron density (peaks) separated by $n-1$ nodes. For 2s, that's $2$ regions and $1$ node. Identifying the peaks on any probability graph is as simple as counting the "bumps."

⚠️ Common Traps Don't confuse probability density ($\psi^2$) with radial probability ($4\pi r^2 \psi^2$). The density $\psi^2$ is maximum at the nucleus for s-orbitals, but the volume element ($\propto r^2$) makes the radial probability zero at $r=0$. Always check if the graph starts at the origin!

$\boxed{\text{Answer: (c)}}$