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 In the Periodic Table a group(also known as a family) is a vertical column of the chemical elements. There are 18 groups in the standard Periodic Table. The modern explanation of the pattern of the table is that the elements in a group have similar configurations of the outer most electron shells of their atoms: as most chemical probertiea qre dominated by the orbital location of the outermost electron.

 In the periodic table of the elements, elements are arranged in a series of rows (or periods) so that those with similar properties appear in vertical columns. Elements of the same period have the same number of electron shells; with each group across a period, the elements have one more proton and electron and become less metallic. This arrangement reflects the periodic recurrence of similar properties as the atomic number increases. For example, the alkaline metals lie in one group (group 1) and share similar properties, such as high reactivity and the tendency to lose one electron to arrive at a noble-gas electronic configuration.

 A metal is a chemical element that is a good conductor of both electricity and heat and forms cations and ionic bonds with non-metals. In chemistry, a metal is an element, compound, or alloy characterized by high electrical conductivity. In a metal, atoms readily lose electrons to form positive ions. Metal is also know for its high tensile strength and malleability.

 Non-metals are the elements in groups of the periodic table. Non-metals are not able to conduct electricity or heat very well. As opposed to metals, non-metallic elements are very brittle, and cannot be rolled into wires or pounded into sheets. The non-metals exist in two of the three states of matter at room temperature: gases (such as oxygen) and solids (such as carbon). The non- metals have no metallic luster, and do not reflect light.  The Non-Metal elements are:  Hydrogen  Carbon  Nitrogen  Oxygen  Phosphorus  Sulfur  Selenium

 Metalloids have properties of both metals and non-metals. Some of the metalloids, such as silicon and germanium, are useful in semi-conductors. This property makes metalloids useful in electronic componets. Mettalloids are located in a stair-step shape between the meatals and non- metals. This line is drawn from between Boron and Aluminum to the border between Polonium and Astatine.

 The lanthanide elements are the group of elements with atomic number increasing from 58 (cerium) to 71 (lutetium). They are termed lanthanide because the lighter elements in the series are chemically similar to lanthanum. Strictly speaking lanthanum is a group 3 element and the ion La^3+ has no f electrons. However this element is often included in any general discussion of the chemistry of the lanthanide elements.

 The Actinides are a collection of 14 radioactive elements named after the element actinium. They also have no stable isotopes. Actinides share the following common properties:  All are radioactive.  Actinides are highly electropositive.  The metals tarnish readily in air.  Actinides are very dense metals with distinctive structures. Numerous allotropes may be formed (plutonium has at least 6 allotropes!).  They react with boiling water or dilute acid to release hydrogen gas.  Actinides combine directly with most nonmetals.

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 The six noble gases are found in group 18 of the periodic table. These elements were considered to be inert gases until the 1960's, because their oxidation number of 0 prevents the noble gases from forming compounds readily. All noble gases have the maximum number of electrons possible in their outer shell (2 for Helium, 8 for all others), making them stable.  Helium  Neon  Argon  Krypton  Xenon  Radon

Metals:left and center Non Metals:right side Noble Gases:right side, except for hydrogen Metalloids:stair-step shape between metals and non-matals Lanthanides/Actinides:at the bottom(57-71,89-103)

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