Write electron configurations for a. the cations Mg^2+, K^+, and Al^3+. b. the anions N^3-, O^2-

step 1 Problem 49 says to get the electron configurations for the following. So A, you have the cations

Write electron configurations for a. the cations Mg^2+, K^+,...

Write electron configurations for
a. the cations $\mathrm{Mg}^{2+}, \mathrm{K}^{+}$, and $\mathrm{Al}^{3+}$.
b. the anions $\mathrm{N}^{3-}, \mathrm{O}^{2-}, \mathrm{F}^{-}$, and $\mathrm{Te}^{2-}$.

Key Concepts

Electron Configuration

Electron configuration is the systematic method of describing the arrangement of electrons in the atomic orbitals of an atom or ion. It involves placing electrons in orbitals in an order dictated by increasing energy, typically following the guidelines of the Aufbau principle, which prioritizes lower energy levels before higher ones.

Ion Formation

Ions are charged species that arise from the loss or gain of electrons. Cations are formed by the removal of electrons and have a positive charge, whereas anions are created by the addition of electrons resulting in a negative charge. Understanding electron configurations for ions requires adjusting the number of electrons compared to the neutral atom in accordance with the type of ion formed.

Aufbau Principle

The Aufbau principle is a rule used to determine the electron configuration of an atom or ion by filling atomic orbitals in order of increasing energy. This principle ensures that electrons occupy the lowest available energy states before moving to higher ones, thereby determining the sequence in which orbitals are populated.

Electron Removal and Addition Order

When forming cations, electrons are typically removed from the highest energy orbitals first (often the outermost shell), which may not always be the same as the orbital order in the neutral atom. Conversely, anions are formed by adding electrons into the available orbitals, filling them according to standard orbital energy levels while obeying the Pauli Exclusion Principle and Hund’s Rule.

Orbital Notation and Noble Gas Shorthand

Orbital notation is a concise method of representing electron configurations by using symbols for orbitals and superscripts for the number of electrons in each orbital. The noble gas shorthand further simplifies electron configurations by representing the core electrons with the symbol of the nearest noble gas, allowing focus on the valence electrons which are most relevant in chemical reactivity and ion formation.

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