Which of the following electronic transitions in a hydrogen atom will require the largest amount of energy?

Question

Question

This question was previously asked in

HPSC Assistant Professor 2018 Chemistry (Official Paper)

Answer 1

CONCEPT:

Electronic Transitions in Hydrogen Atom

In a hydrogen atom, electronic transitions involve the movement of an electron between energy levels (n).
The energy required for a transition is given by the difference in energy between the two levels, according to the formula: eV, where is the final state and is the initial state.
The energy difference between lower energy levels (e.g., n=1 to n=2) is larger than between higher energy levels (e.g., n=3 to n=4).

EXPLANATION:

Option 1: From n=0 to n=1 is not a valid transition since the ground state of a hydrogen atom starts from n=1, so this option is irrelevant.
Option 2: From n=1 to n=2 requires energy, and it involves a transition from the first energy level to the second. This is a significant energy transition.
Option 3: From n=2 to n=1 releases energy as the electron moves to a lower energy state. Although significant, this is not the largest energy transition.
Option 4: From n=3 to n=4 requires less energy compared to the transition from n=1 to n=2 because the energy levels are closer together at higher n values.

The correct answer is: From n=1 to n=2

Download Solution PDF