Consider a transition in which the electron of a hydrogen atom is excited from n = 1 to n = . (a) What is the end result of this transition?

Key Concepts

Quantum Energy Levels

In quantum mechanics, electrons in an atom occupy discrete energy levels, denoted by quantum numbers (n). For hydrogen, these levels are quantized, meaning an electron can only exist in specific states. The transition from a lower energy level (n=1) to a higher one (n=2, for example) involves the absorption of energy, typically in the form of a photon.

Photon Absorption

When an electron transitions from a lower to a higher energy level, it absorbs a photon whose energy matches the difference between the two levels. The energy of the photon is given by the equation E = hf, where E is energy, h is Planck's constant, and f is the frequency of the photon. This process is fundamental in understanding how atoms interact with light.

Excited State

An excited state refers to an electron configuration where an electron has absorbed energy and moved to a higher energy level than its ground state. In the case of hydrogen, when the electron transitions from n=1 to n=2, it is in an excited state. This state is typically unstable, and the electron will eventually return to the ground state, often releasing energy in the form of light.