Give the electronic configurations of each of the following...

Give the electronic configurations of each of the following atoms and ions. Identify the valence electrons and valence orbitals in each.
(a) oxygen atom
(b) chloride ion, $\mathrm{Cl}^{-}$
(c) potassium ion, $\mathrm{K}^{+}$
(d) sodium atom

Key Concepts

Ionic Electronic Configurations

Ionic electronic configurations involve the changes in electron arrangements when an atom gains or loses electrons to form an ion. The loss of electrons (in cations) or gain of electrons (in anions) results in configurations that may alter an element's chemical reactivity and stability, often reflecting a transition to a more stable electron shell or achieving a noble gas configuration.

Valence Orbitals

Valence orbitals are the specific orbitals (such as the s and p orbitals in the outermost shell) where valence electrons reside. These orbitals are significant because they are the highest in energy and most exposed to interactions with other atoms, thus dictating the atom's or ion's chemical properties.

Electronic Configuration

Electronic configuration refers to the arrangement of electrons in an atom or ion according to a specific order (typically following the Aufbau principle, Hund's rule, and the Pauli exclusion principle). This configuration details how electrons populate various orbitals (s, p, d, f), providing insight into the element's chemical behavior and periodic properties.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that participate in chemical bonding and reactions. They determine the chemical reactivity and bonding patterns of an element; the number of valence electrons is often directly related to the element's group in the periodic table.

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