Yes. Electromagnetic radiation can change the arrangement of electrons in an atom, as long as the radiation has the right amount of energy to move electrons between energy levels.

Core idea

  • Atoms have electrons arranged in quantized energy levels (shells and subshells), often called the electron configuration.
  • Electromagnetic radiation (from radio waves up to gamma rays) carries energy in photons. If a photon’s energy matches the gap between two electron energy levels, the atom can absorb or emit that photon, and an electron will move.

How radiation changes electron arrangement

  • Absorption (excitation):
    • When an atom absorbs electromagnetic radiation, an electron can “jump” from a lower energy level (closer to the nucleus) to a higher one (farther out), creating an excited state.
* This temporarily changes the electron arrangement from the ground-state configuration to an excited configuration.
  • Emission (relaxation):
    • Excited electrons are unstable and tend to fall back down to lower energy levels.
    • When they do, the atom emits electromagnetic radiation with energy equal to the difference between the two levels, producing line spectra characteristic of each element.

In simple terms: light in → electrons move up; light out → electrons fall back down.

Ground state vs excited state

  • Ground state:
    • This is the lowest-energy, most stable electron configuration of an atom.
    • It follows rules like “fill lowest energy orbitals first” and “spread electrons out in equal-energy orbitals” (Aufbau principle, Hund’s rule, Pauli exclusion principle).
  • Excited state:
    • When radiation is absorbed, electrons occupy higher-energy orbitals than they do in the ground state, so the electron configuration pattern is temporarily different.
* Once the electron drops back, the atom returns to its ground-state electron arrangement.

What kind of radiation is needed?

  • The energy gap between levels in atoms is typically matched by photons in the ultraviolet, visible, or infrared parts of the spectrum, depending on the atom and transition.
  • Very low-energy radiation (like many radio waves) usually cannot move bound electrons between atomic energy levels because each photon carries too little energy.
  • Very high-energy radiation (X‑rays, gamma rays) can do much more than just rearrange electrons; it can ionize atoms by knocking electrons completely out of the atom, or even damage nuclei at extreme energies.

Ionization vs simple rearrangement

  • Rearrangement (bound–bound transitions):
    • Electron stays in the atom but moves between levels.
    • This is responsible for atomic absorption and emission lines in spectra.
  • Ionization (bound–free transitions):
    • If a photon’s energy exceeds the binding energy of an electron, the electron can be completely removed from the atom.
    • This changes not just the arrangement but also the overall charge, turning the atom into an ion.

Why this matters (physics and “trending context”)

  • The way electromagnetic radiation shifts electron arrangements underpins:
    • Spectroscopy: Identifying elements in stars and galaxies by their emission/absorption lines, all tied to specific electron transitions.
* **Lasers and LEDs:** These rely on controlled excitation and de‑excitation of electrons.
* **Modern tech:** Solar cells, sensors, and even photoelectric devices exploit how metals and atoms eject or rearrange electrons under light.

TL;DR

  • Yes, electromagnetic radiation can change the electron arrangement of an atom by promoting electrons to higher energy levels (excitation) or letting them drop back down while emitting radiation.
  • If the photon energy is high enough, it can even eject electrons entirely, ionizing the atom.

Information gathered from public forums or data available on the internet and portrayed here.