Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. (a) CI⁻, (b) Sc³⁺, (c) Fe²⁺, (d) Zn²⁺, (e) Sn⁴⁺.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons. Understanding electron configuration is crucial for determining how ions form and how they compare to their neutral atoms, as it directly influences chemical properties and reactivity.

Ionic Charge and Electron Count

The ionic charge of an atom indicates the number of electrons lost or gained compared to its neutral state. For example, a cation like Sc³⁺ has lost three electrons, while an anion like Cl⁻ has gained one. Identifying the neutral atom corresponding to an ion involves adjusting the electron count based on its charge, which is essential for comparing electron configurations.

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons and, consequently, the same electron configuration. This concept is important for understanding how different ions can exhibit similar chemical behavior despite being different elements. Recognizing isoelectronic relationships helps in predicting properties and reactivity of ions in various chemical contexts.