Write the ground-state electron configurations of the...

Write the ground-state electron configurations of the following ions: (a) $\mathrm{Li}^{+},$ (b) $\mathrm{H}^{-}$, (c) $\mathrm{N}^{3-},$ (d) $\mathrm{F}^{-}$ (c) $S^{2-},\left(\text { (f) } A I^{3+},(g) S e^{2-},(h) B r^{-},(\text {i }) R b^{+},(j) S r^{2+}\right.$ (k) $\operatorname{Sn}^{2+},$ (l) $\operatorname{Te}^{2-},\left(\text { m) } \mathrm{Ba}^{2+}, \text { (n) } \mathrm{Pb}^{2+}, \text { (o) } \mathrm{In}^{3+}\right.$ (p) $\mathrm{T} 1^{+},$ (q) $\mathrm{T} 1^{3+}$

Key Concepts

Noble Gas Abbreviation (Shorthand Notation)

Noble gas shorthand is a method for writing electron configurations more concisely by using the electron configuration of a noble gas (such as [He], [Ne], or [Ar]) to represent core electrons. This simplifies the writing of configurations, especially for elements with many electrons, by avoiding the need to list all the inner orbitals.

Aufbau Principle

The Aufbau principle is the guideline that electrons fill lower-energy orbitals before occupying higher-energy orbitals. This rule is fundamental when writing ground-state electron configurations and helps predict the order in which orbitals are populated, including during ion formation.

Orbital Filling Order

This key concept deals with the sequential filling of atomic orbitals according to their energy levels. The arrangement follows a specific order (for example, 1s, 2s, 2p, 3s, etc.), which is crucial when determining how electrons are distributed in both neutral atoms and their corresponding ions.

Ground-State Electron Configuration

This concept refers to the arrangement of electrons in an atom or ion at its lowest energy level. For any species, electrons are distributed among orbitals in a way that minimizes energy, following specific rules and principles such as the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

Ion Formation and Electron Count

When atoms form ions, they either lose or gain electrons relative to the neutral atom, leading to a change in the overall electron configuration. Losing electrons typically occurs from the highest energy orbitals (often s or p orbitals), while gaining electrons fills the next available lower-energy orbitals, which alters configuration compared to the neutral state.

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