Write the ground-state electron configurations of the following ions, which play important roles in biochemical processes in our bodies: (a) \(\mathrm{Na}^{+}\), (b) \(\mathrm{Mg}^{2+},(\mathrm{c}) \mathrm{Cl}^{-},(\mathrm{d}) \mathrm{K}^{+},(\mathrm{e}) \mathrm{Ca}^{2+},(\mathrm{f}) \mathrm{Fe}^{2+},(\mathrm{g}) \mathrm{Cu}^{2+}\) (h) \(\mathrm{Zn}^{2+}\).

The periodic table is a comprehensive chart that organizes chemical elements based on their atomic number, electron configurations, and recurring chemical properties. Elements are arranged in order of increasing atomic number into rows called periods and columns called groups. The table facilitates a systematic way to explore the relationships between different elements and predict the properties of new compounds.

When dealing with ions, the periodic table becomes particularly useful in anticipating the loss or gain of electrons, guiding us through which orbital the electron would be removed from or added to. For instance, the elements in Group 1 are known to form +1 ions by losing an electron from their outermost shell, thus reducing to the configuration of a noble gas.

Atomic orbitals are the regions in an atom where electrons are most likely to be found. They are defined by the three quantum numbers: the principal (n), angular momentum (l), and magnetic (m_l). Each orbital can hold a maximum of two electrons with opposite spins, according to the Pauli exclusion principle.

The types of orbitals (s, p, d, f) have distinctive shapes and energy levels. In ions, the electron configuration can change, with electrons being added to or removed from these atomic orbitals. For example, when an atom forms a cation, electrons are usually removed from the orbitals with the highest principal quantum number (n), starting from the outermost orbitals.

Electron distribution refers to the arrangement of electrons in an atom's orbitals according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle. The Aufbau principle states that lower energy orbitals fill before higher energy orbitals. Hund's rule explains that electrons will fill degenerate orbitals (orbitals with the same energy level) singly before pairing up. Understanding the electron distribution is crucial when forming ions, as this determines how many electrons will be lost or gained and from which orbitals, to achieve the electron configuration of the nearest noble gas.

Chemical elements are pure substances consisting of only one type of atom, characterized by a specific number of protons in their nuclei, which determines the element's atomic number. The variations in the number of neutrons create different isotopes of an element. The distinct properties of each element are due to the differing number of protons, neutrons, and electrons, with the electrons playing a key role in chemical bonding and reactions.

When elements ionize to form cations or anions, they are transforming into ions by the gain or loss of electrons, which directly alters their chemical properties. This electron transfer leads to more stable electron configurations for the reacting atoms, typically resembling the stable configurations of noble gases.