Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? (a) from n = 3 to n = 2

Key Concepts

Energy Levels in Hydrogen

In hydrogen, electrons occupy discrete energy levels, denoted by quantum numbers (n). The energy associated with each level increases with n, meaning that higher levels (larger n) have more energy. When an electron transitions between these levels, it either absorbs or emits energy, depending on whether it moves to a higher or lower energy level.

Photon Emission and Absorption

When an electron transitions from a higher energy level to a lower one, it emits energy in the form of a photon. Conversely, when it moves from a lower to a higher energy level, it absorbs a photon. The energy of the emitted or absorbed photon corresponds to the difference in energy between the two levels involved in the transition.

Calculating Energy Changes

The energy change associated with an electronic transition can be calculated using the formula ΔE = E_final - E_initial, where E is the energy of the respective levels. For hydrogen, the energy of each level can be determined using the Rydberg formula, which allows for the calculation of the energy of the photon emitted or absorbed during the transition.