Atomic Electron Distributions and Ions

Atomic Electron Distributions

• Iron (Fe): Atomic number 26, atomic mass 55.845. Its electron configuration shows electrons in 1s, 2s, 2p, 3s, 3p, and 3d orbitals.

Atomic Electron Distributions (continued)

• Nitrogen (N): Atomic number 7, atomic mass 14.007. Its electron configuration places electrons in 1s, 2s, and 2p orbitals.

Electron Distribution of Ions

• Nitrogen Ion (N⁺): The N⁺ ion has a single electron less than neutral nitrogen, so electron distribution in 1s and 2s remains the same, but the 2p orbital has one fewer electron-up arrow.
• Nitrogen Ion (N³⁺): The N³⁺ ion has three fewer electrons compared to neutral nitrogen. Electron distribution results in the removal of electrons from 2p before any other orbitals, leaving only electrons in the 1s orbital.
• Oxygen (O): Atomic number 8, atomic mass 15.999, has electrons in 1s, 2s and 2p orbitals.

Electron Distribution of Ions (continued)

• Oxygen Ion (O^2-): This ion has two extra electrons compared to neutral oxygen. The additional electrons fill the available spaces within the 2p orbitals.

Electron Distribution of Other Elements

• Chromium (Cr): Atomic number 24, atomic mass 51.996. Its electron configuration differs from the usual expected pattern due to the shifting of an electron from a 4s to a 3d orbital for stability. The 3d orbital has one more electron than the 4s orbital (following Hund's rule).
• Copper (Cu): Atomic Number 29, atomic mass 63.546. Similar to Chromium, copper's electron configuration deviates from expected convention as an electron is from the 4s orbital and into a 3d orbital for stability. The 3d orbital also has one more electron than the 4s orbital (following Hund's rule).
• Iron Ion (Fe²⁺): Iron's electron configuration changes accordingly after the oxidation, and electron distribution is adjusted to reflect a loss of two electrons from the neutral Fe atom's configuration.

This quiz explores the electron configurations of various elements, including Iron and Nitrogen, as well as their ionic forms. Understand how electron distributions change when atoms gain or lose electrons, particularly focusing on the N+ and N3+ ions. Test your knowledge on the fundamental principles of atomic structure and electron distribution.