Bohr S Model For Hydrogen Atom

Bohr model assumes:

• electrons move in circular orbits,
• these orbits are stationary and non-radiating,
• angular momentum is quantized.

Bohr model works well only for: It does not successfully explain many-electron atoms. So the wrong statement is:

Step 1: Understanding the Concept:
In Bohr's highly successful model of the hydrogen atom, electrons occupy specific, discrete, and quantized circular orbits (energy levels).
The lowest possible energy level is correctly referred to as the ground state, while the higher energy levels above it are categorized sequentially as excited states.
Step 2: Key Formula or Approach:
The total energy of an electron orbiting in the principal quantum state of a hydrogen atom is calculated using the established formula:
Step 3: Detailed Explanation:
First, we must correctly identify the principal quantum number corresponding to the "3 excited state."
The ground state is inherently .
The excited state corresponds to .
The excited state corresponds to .
Therefore, the excited state strictly corresponds to .
Now, substitute directly into the quantized energy formula:
Executing the division yields the numerical value:
Step 4: Final Answer:
The energy of the electron in the excited state is .