Element X reacts with element Y to form an ionic compound containing \(\mathrm{X}^{4+}\) and \(\mathrm{Y}^{2-}\) ions. Write a formula for the compound and suggest in which periodic groups these elements are likely to be found. Name a representative compound.

Chemical bonding is the process by which atoms combine to form new substances. One of the most fundamental types of chemical bonds is the ionic bond, which occurs between metal and non-metal elements. In ionic bonding, one atom loses electrons and becomes positively charged, while the other gains electrons and becomes negatively charged. The atom that loses electrons is called a cation and the one that gains electrons is an anion. These opposite charges lead to a strong electrostatic attraction between the ions, resulting in the formation of an ionic compound.

For example, when element X loses four electrons, it becomes a positive cation with a 4+ charge, represented as \(\mathrm{X}^{4+}\). Conversely, when element Y gains two electrons, it becomes a negatively charged anion, represented as \(\mathrm{Y}^{2-}\). They combine in a ratio that balances their charges, creating an electrically neutral compound. This is why, to achieve neutrality, we need two \(\mathrm{Y}^{2-}\) anions to balance one \(\mathrm{X}^{4+}\) cation, resulting in the formula \(X(Y_2)\).

The periodic table is a tabular arrangement of elements organized by increasing atomic number and grouped by similar chemical properties. Groups, also known as families, are the columns of the periodic table and contain elements that share common characteristics, mainly due to their similar valence electron configurations.

For instance, elements in group 1 (alkali metals) have a single electron in their outermost shell and frequently form 1+ ions, while elements in group 17 (halogens) have seven electrons in their outer shell and often form 1- ions. As for our exercise, element X is likely in group 4 or 14, where elements typically have four electrons in their outer shell to lose, forming a 4+ ion. In contrast, element Y is predisposed to be in group 16, where elements generally have six valence electrons and are two electrons short of a full octet, leading to the formation of 2- ions when they gain those two missing electrons.

Ionic charges refer to the electrical charge an atom acquires when it loses or gains electrons to achieve a stable electron configuration. In forming ionic compounds, metals tend to lose electrons and non-metals tend to gain. This transfer of electrons is what gives ions their charge.

Metals, located on the left side of the periodic table, often form positive ions or cations. For example, in step 2 of our solution, element X loses four electrons, indicating the formation of a cation with a \(4+\) charge. On the other hand, non-metals, found on the right side of the periodic table, typically gain electrons and form negative ions, or anions. Element Y, in our exercise, gains two electrons leading to a \(2-\) charge. The charge on an ion dictates the ratio at which ions combine to form neutral compounds. In our case, to achieve electrical neutrality for the ionic compound, two \(\mathrm{Y}^{2-}\) ions combine with one \(\mathrm{X}^{4+}\) ion to create the compound \(X(Y_2)\). This is consistent with the principle that the total positive charge must equal the total negative charge in an ionic compound.