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Periodic Table of Elements – Structure and Significance

The periodic table organizes all known chemical elements by atomic number and electron configuration. It is a fundamental tool in chemistry, medicine, and pharmacy.

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Things worth knowing about "Periodic table"

The periodic table organizes all known chemical elements by atomic number and electron configuration. It is a fundamental tool in chemistry, medicine, and pharmacy.

What is the Periodic Table?

The periodic table of elements is a tabular arrangement of all known chemical elements, organized by their atomic number (number of protons in the nucleus), electron configuration, and recurring chemical properties. It was primarily developed by Dmitri Mendeleev in 1869 and remains the cornerstone of modern chemistry.

The periodic table currently contains 118 officially recognized elements, ranging from Hydrogen (H, atomic number 1) to Oganesson (Og, atomic number 118). The elements are arranged in 18 groups (columns) and 7 periods (rows).

Structure and Organization

The horizontal rows are called periods. Within a period, the atomic number increases from left to right. The vertical columns are called groups. Elements in the same group share similar chemical properties because they have the same number of valence (outer-shell) electrons.

Main groups (1, 2, 13–18): Contain the typical nonmetals, metalloids, and metals with characteristic properties.
Transition metals (groups 3–12): Occupy the central block of the table.
Lanthanides and Actinides: Displayed as separate rows below the main table.

Classification of Elements

Elements are classified according to their physical and chemical properties at room temperature:

Metals: Good electrical conductors, lustrous, malleable (e.g., iron, copper, gold)
Nonmetals: Poor electrical conductors (e.g., oxygen, nitrogen, sulfur)
Metalloids (Semimetals): Properties intermediate between metals and nonmetals (e.g., silicon, arsenic)
Noble gases: Highly unreactive, monoatomic gases (e.g., helium, neon, argon)
Halogens: Highly reactive, readily form salts (e.g., fluorine, chlorine, iodine)

Relevance to Medicine and Pharmacy

The periodic table has direct relevance to medicine and pharmacy. Many elements are essential to the human body or are used therapeutically:

Essential macroelements: Calcium (Ca), Phosphorus (P), Sodium (Na), Potassium (K), Magnesium (Mg) – vital for bone structure, muscle, and nerve function
Trace elements: Iron (Fe), Zinc (Zn), Selenium (Se), Iodine (I), Copper (Cu) – required in minute amounts for metabolic processes
Therapeutic elements: Lithium (Li) for bipolar disorder, Platinum (Pt) in cytostatic drugs (e.g., cisplatin), Gold (Au) in rheumatoid arthritis treatment
Contrast agents and diagnostics: Barium (Ba) in X-ray diagnostics, Gadolinium (Gd) as an MRI contrast agent
Radioactive elements: Technetium-99m (Tc) in nuclear medicine for scintigraphy imaging

Periodic Properties

A key feature of the periodic table is the periodicity of elemental properties. The following properties change systematically across periods and down groups:

Atomic radius: Decreases across a period from left to right; increases down a group.
Electronegativity: Increases across a period from left to right; decreases down a group.
Ionization energy: The energy required to remove an electron from an atom.
Metallic character: Decreases from left to right across a period.

Historical Development

The concept of a systematic ordering of elements was developed simultaneously by several scientists in the 19th century. Dmitri Mendeleev (1869) and Lothar Meyer are considered the most important pioneers. Mendeleev predicted the existence of then-unknown elements based on his system – a remarkable achievement that demonstrated the predictive power of the periodic table. The modern periodic table is based on Moseley's law (1913), which established atomic number as the fundamental ordering principle.

References

IUPAC (International Union of Pure and Applied Chemistry): Nomenclature of Inorganic Chemistry – IUPAC Recommendations 2005. RSC Publishing, 2005.
Atkins, P. & de Paula, J.: Physical Chemistry, 10th Edition. Oxford University Press, 2014.
National Institute of Standards and Technology (NIST): Atomic Weights and Isotopic Compositions. Available at: https://www.nist.gov

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