Periodic table - Natural versus Synthetic Elements Overview

Natural Versus Synthetic Elements Introduction Elements in the periodic table fall into two categories: natural elements and synthetic elements. Natural elements occur in nature and can be extracted from Earth's materials. Synthetic elements, by contrast, do not exist naturally—they must be created artificially in laboratories. Understanding this distinction is crucial because it explains why certain elements have different properties and availability compared to more familiar elements. Synthetic Elements All 24 elements with atomic numbers 95 through 118 are synthetic elements. This means that every element from americium (Am, Z = 95) onward does not occur naturally on Earth and must be produced in controlled laboratory settings through nuclear reactions. Why Must They Be Produced in Laboratories? The key reason synthetic elements must be created artificially is radioactivity. All elements with atomic numbers 95–118 are radioactive, meaning their nuclei are unstable and spontaneously decay by emitting radiation and transforming into other elements. This instability is fundamental to their nature—they cannot exist for extended periods without breaking down. The periodic table above shows where these synthetic elements are located—in the actinide series (elements 89–103) and the subsequent period beyond lawrencium. Why Are Heavy Elements Radioactive? As atomic number increases, nuclei become larger and more difficult to hold together. The strong nuclear force, which binds protons and neutrons, can only reach a limited distance. In very heavy nuclei with many protons and neutrons, the repulsive electrical force between protons eventually becomes stronger than the binding force in certain regions of the nucleus. This creates instability, leading to radioactive decay. This is why synthetic elements cannot exist naturally in significant quantities—they decay too quickly. Creating them requires bombarding lighter elements with particles (such as neutrons or accelerated ions) in particle accelerators or nuclear reactors, forcing atomic nuclei to fuse together momentarily before they decay.