A Five energy levels of the He atom are given in joules per...

A Five energy levels of the He atom are given in joules per atom above an arbitrary reference energy: (1) $6.000 \times 10^{-19}$ (2) $8.812 \times 10^{-19}$ (3) $9.381 \times 10^{-19}$ (4) $10.443 \times 10^{-19}$ (5) $10.934 \times 10^{-19}$. Construct an energy level diagram for He, and find the energy of the photon (a) absorbed for the electron transition from level 1 to level 5 and (b) emitted for the electron transition from level 4 to level 1 .

A Five energy levels of the He atom are given in joules per atom above an arbitrary reference energy:
(1) $6.000 \times 10^{-19}$
(2) $8.812 \times 10^{-19}$
(3) $9.381 \times 10^{-19}$
(4) $10.443 \times 10^{-19}$
(5) $10.934 \times 10^{-19}$.
Construct an energy level diagram for He, and find the energy of the photon (a) absorbed for the electron transition from level 1 to level 5 and (b) emitted for the electron transition from level 4 to level 1 .

Key Concepts

Energy Level Diagram

A diagram that visually represents the discrete energy levels available to electrons in an atom. It illustrates the relative positions of these levels, providing a framework to analyze transitions where electrons emit or absorb energy in the form of photons.

Electron Transitions

The process by which an electron moves between energy levels within an atom. Transitions to higher energy levels involve the absorption of energy, while transitions to lower energy levels result in the emission of energy. The energy change is precisely defined by the difference between the initial and final energy levels.

Photon Absorption and Emission

When an electron transitions, it either absorbs a photon (jumping to a higher energy level) or emits a photon (falling to a lower energy level). The energy of the photon corresponds exactly to the difference in energy between the initial and final states. This concept is fundamental in spectroscopy and helps explain how light interacts with matter.

Energy Difference Calculation

The method used to determine the energy of a photon involved in electronic transitions. By subtracting the energy of the initial level from the energy of the final level, one obtains the energy magnitude of the photon absorbed or emitted. This calculation underpins the quantitative analysis of spectral lines in atomic and molecular spectroscopy.

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