Of the following set which one does not contain isoelectronic species? (a) \(\mathrm{CN}^{-}, \mathrm{N}_{2}, \mathrm{C}_{2}^{2}-\) (b) \(\mathrm{PO}_{4}{ }^{3}, \mathrm{SO}_{4}{ }^{2-}, \mathrm{ClO}_{4}^{-}\) (c) \(\mathrm{SO}_{3}^{2-} \cdot \mathrm{CO}_{3}^{2-} \cdot \mathrm{NO}_{3}^{-}\) (d) \(\mathrm{BO}_{3}{ }^{3-}, \mathrm{CO}_{3}{ }^{2-}, \mathrm{NO}_{3}^{-}\)

Chemical bonding is the fundamental concept that explains how atoms come together to form molecules and compounds. It involves the sharing or transfer of electrons between atoms to achieve stability, often resulting in the complete filling of their outermost electron shells or orbitals – a state inspired by the electron configuration of noble gases, which are inherently stable.

There are three primary types of chemical bonding: ionic, covalent, and metallic. Ionic bonding occurs when electrons are transferred from one atom to another, leading to the formation of positively and negatively charged ions. These ions then attract each other due to their opposing charges. Covalent bonding involves the sharing of electrons between atoms, often resulting in the formation of a molecule.

Understanding the concept of isoelectronic species fits into the broader context of chemical bonding because it relates to the number of electrons an atom, ion, or molecule has. Isoelectronicity is critical when considering the formation of ions, as gaining or losing electrons to become isoelectronic with a noble gas is a driving force for ionic bond formation.

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The geometry of a molecule plays a crucial role in determining its chemical and physical properties, including reactivity, polarity, and color.

The VSEPR (Valence Shell Electron Pair Repulsion) theory is often used to predict the geometry of a molecule. It's based on the idea that electron pairs around the central atom will assume a geometry that minimizes the repulsion between them. For example, electron pairs in a molecule with the formula AX2, where A is the central atom and X is a bonded atom, would be oriented 180 degrees apart, resulting in a linear shape.

In the context of isoelectronic species, although the species may have the same electron count, their molecular geometries can differ due to variations in the arrangement of electrons and the types of atoms involved in the molecule. This can lead to different physical and chemical characteristics despite being isoelectronic.

Ionic charges refer to the positive or negative electrical charge of an ion, which is an atom or molecule that has lost or gained one or more electrons. Cations are positively charged ions that occur when an atom loses electrons, while anions are negatively charged ions formed when an atom gains electrons.

The magnitude of the ionic charge is typically indicated by a superscript following the chemical symbol, such as Na+, which represents a sodium ion with a +1 charge. This charge is important because it determines the ionic bonding potential of the species. Ions tend to form ionic compounds by combining with ions of opposite charge in order to attain a full valence shell and achieve electrostatic stability.

In the exercise concerning isoelectronic species, the ionic charge is critical in calculating the total number of electrons. For example, a phosphate ion (PO4^3-) has three extra electrons due to its -3 charge, impacting its isoelectronic status. Correctly accounting for ionic charges is essential in identifying isoelectronic species and predicting the types of bonds they can form.