The Organization of Elements on the Periodic Table

Since the inception of chemistry as a science, 118 elements have been discovered or synthesized. Each has its very own place in the periodic table of elements. This incredible scientific marvel celebrated its 150th anniversary in 2019, which was designated by the United Nations as the International Year of the Periodic Table (Cleave and Crans 2). Without this tool, scientists would be hard-pressed to perform valid, consistent scientific experiments, and the entire field would be something else entirely. Everything found on the table is there for a specific and exact reason in order to showcase periodic trends. Using groups, periods, atomic numbers, and elemental properties, a chemist is easily able to discern between elements and their properties using the periodic table. These properties of the periodic table are essential to a solid understanding of chemistry and are explained with scientific evidence throughout this paper.

Atomic numbers are the ground-level identifier of any element, and these numbers signify the number of protons in the nucleus of each element (Ross 4). Essentially, this number is the primary difference between one element and another and indicates many elemental properties. These are essential in any chemistry experiment because they identify the chemical and its properties made evident during experimentation. It is a good idea to have an understanding of what will happen before mixing any chemicals. The atomic numbers on the periodic table range from one to 118 and are essential in identifying an element's chemical properties.

The atomic number is only the beginning of the table's organization, however. Each element has its protons fill consecutive electron shells, or atomic orbitals. The outer shell populated by electrons can quickly be identified by observing which horizontal row, or period, the element sits in on the table (Ross 8). Each element in a row has outer electrons in the same atomic orbital. With metals on the left and nonmetals on the right, an element's period provides the reader with numerous elemental properties. These include its atomic radius, electronegativity, and energy of ionization, among others.

In contrast to these periods are the elemental groups, also known as families. These vertical columns provide even more information at a glance about any given element on the table, primarily the element's electron configuration of its outer valence shell (Ross 7). Typically, each element in a given group tends to display similar chemistry and elemental properties with their increasing atomic numbers. These groups are currently designated numerically from one, the alkali metals group, to eighteen, the noble gases family. Similar to periods, elements in the same groups also tend to share elemental patterns like atomic radius, ionization energy, and electronegativity as well.

The final basic level of periodic organization is aptly named blocks and indicates the sequence in which electrons populate the valence atomic orbitals. These are identified by grouping elements whose differentiating electron, the one distinguishing it from the next, is in the same atomic orbital (Ross 12). These blocks are named according to the subshell in which their last electron resides and are named after their characteristic orbital. This naming system creates the s-block, p-block, d-block, and f-block from left to right. The periodic table of elements is a complex structure for identifying the elemental properties of any element at a glance, and understanding it thoroughly is a crucial component for any successful chemist.

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