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This document provides an introduction to the periodic table. It discusses the organization of the periodic table into groups and periods and lists some of the key groups including alkali metals, alkaline earth metals, halogens, and noble gases. It also provides brief descriptions of some of the elements in these groups and discusses important properties like atomic number and mass. Overall, the document serves as a high-level overview of the periodic table and how it organizes the elements.

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The periodic table arranges the known chemical elements in order of their atomic number, with elements in the same group (vertical column) having similar properties. Elements are classified into periods (horizontal rows) and groups based on their atomic structure and electron configuration, with elements in the same group having the same number of electrons in their outer shell and exhibiting similar chemical behaviors. The periodic table summarizes periodic trends in properties of the elements and how an element's position determines its chemical properties.

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This document summarizes key concepts from a chemistry textbook chapter on the periodic table. It discusses how elements are organized in the periodic table based on their atomic structure and properties. Early sections describe the historical development of periodic tables and how elements are classified into groups based on electron configuration. Later sections summarize periodic trends in atomic size, ionization energy, and ion size based on an element's position in the periodic table and how its electron configuration is filled.

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The halogens are a group of non-metals that all have seven electrons in their outer shell, making them highly reactive as they only need one more electron to fill their outer shell. The halogens featured are fluorine, chlorine, bromine, iodine, and astatine. Fluorine is used in toothpaste as fluoride. Chlorine is mostly used to kill bacteria or as a bleach. Bromine is a main ingredient in camera film as silver bromide. Iodine dissolved in water can be used as an antiseptic or starch test.

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Nucleic acids are polymers made of nucleotides joined by phosphodiester bonds. The nucleotides contain nitrogenous bases (purines or pyrimidines) attached to a sugar-phosphate backbone. DNA contains the sugars deoxyribose and the bases adenine, guanine, cytosine, and thymine. RNA contains the sugar ribose and replaces thymine with uracil. Nucleic acids form double-stranded helical structures stabilized by base pairing between adenine-thymine and guanine-cytosine in DNA or adenine-uracil and guanine-cytosine in RNA.

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The document summarizes key periodic trends in the properties of elements as they relate to their position in the periodic table, including: 1) Atomic radius generally increases down a group and decreases across a period as more protons are added to the same principal energy level. 2) Ionization energy decreases down a group as atoms gain principal energy levels but increases across a period as more protons are added. 3) Positive ion size decreases and negative ion size increases relative to their parent atoms. Ion sizes also increase down a group. 4) Electronegativity decreases down a group but increases across a period toward the nonmetals.

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Alchemists in the Middle Ages first introduced symbols for elements, which influenced modern chemists' use of symbols for convenience. Jons Jacob Berzelius invented the current system of chemical symbols. Elements' symbols are derived from their names in Latin, English, or the scientists who discovered them. Henry Moseley's work with X-ray spectra showed that atomic number, not mass, determines an element's position in the periodic table. This led to restating the periodic law in terms of atomic number and the modern form of the periodic table.

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This document summarizes the history of the periodic table, beginning with Aristotle's theory of four elements in 330 BC. It then discusses key contributors such as Lavoisier, Berzelius, Dobereiner, Newlands, Meyer, and Mendeleev who developed early classifications and periodic tables of the elements in the 17th-19th centuries. The modern periodic table took shape in the early 20th century with discoveries like the noble gases, determination of atomic numbers, and transuranium elements. Many scientists collectively contributed to developing the systematic arrangement of elements now known as the periodic table.

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