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    In chemistry, a nonmetal (or a non-metal) is a chemical element that generally lacks a predominance of metallic properties; they range from colorless gases (like hydrogen) to shiny solids (like carbon, as graphite). The electrons in nonmetals behave differently from those in metals. With some exceptions, those in nonmetals are fixed in place, resulting in nonmetals usually being poor conductors of heat and electricity and brittle or crumbly when solid.

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      A nonmetal is a chemical element that is not a metal or a...

  2. In chemistry, after nonmetallic elements such as silicon, chlorine, and helium are classed as either metalloids, halogens, or noble gases, the remaining unclassified elements are hydrogen, carbon, nitrogen, oxygen, phosphorus, sulfur and selenium. The nonmetallic elements are sometimes instead divided into two to six alternative classes or sets according to, for example, electronegativity; the relative homogeneity of the halogens; molecular structure; the peculiar nature of hydrogen; the corrosi

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  4. Nonmetals or non-metals are chemical elements which do not have the properties of a metal. They gain electrons when reacting with a metal. They are generally not lustrous and are bad conductors of heat and electricity. Some are gases including: hydrogen, helium, oxygen, nitrogen, fluorine, neon or radon and others.

    • Nonmetals on The Periodic Table
    • Properties of Nonmetals
    • Summary of Common Properties
    • Comparing The Metals and Nonmetals
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    The nonmetals are located on the upper right side of the periodic table. Nonmetals are separated from metals by a line that cuts diagonally through the region of the periodic table containing elements with partially filled p orbitals. The halogens and noble gases are nonmetals, but the nonmetal element groupusually consists of the following element...

    Nonmetals have high ionization energies and electronegativities. They are generally poor conductors of heat and electricity. Solid nonmetals are generally brittle, with little or no metallic luster. Most nonmetals have the ability to gain electrons easily. Nonmetals display a wide range of chemical properties and reactivities.

    Here is a summary of the properties of the nonmetals. 1. High ionization energies 2. High electronegativities 3. Poor thermal conductors 4. Poor electrical conductors 5. Brittle solids—not malleable or ductile 6. Little or no metallic luster 7. Gain electrons easily 8. Dull, not metallic-shiny, although they may be colorful 9. Lower melting points ...

    The chart below displays a comparison of the physical and chemical properties of the metals and nonmetals. These properties apply to the metals in general (alkali metals, alkaline earth, transition metals, basic metals, lanthanides, actinides) and nonmetals in general (nonmetals, halogens, noble gases).

    Atkins, P. A. (2001). The Periodic Kingdom: A Journey Into the Land of the Chemical Elements. London: Phoenix. ISBN 978-1-85799-449-0.
    Brady, J. E.; Senese, F. (2009).Chemistry: The Study of Matter and its Changes(5th ed.). New York: John Wiley & Sons. ISBN 978-0-470-57642-7.
    Challoner, J. (2014). The Elements: The New Guide to the Building Blocks of our Universe. Carlton Publishing Group. ISBN 978-0-233-00436-5.
    Oxtoby, D. W.; Gillis, H. P.; Butler, L. J. (2015). Principles of Modern Chemistry(8th ed.). Boston: Cengage Learning. ISBN 978-1-305-07911-3.
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  5. Feb 25, 2020 · There are 7 elements that belong to the nonmetals group: Hydrogen (sometimes considered an alkali metal) Carbon Nitrogen Oxygen Phosphorus Sulfur Selenium Although these are the elements in the group nonmetals, there are two additional element groups that could be included, since the halogens and noble gases also are types of nonmetals.

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  6. Non-metals are natural materials that do not produce heat or electricity and that are structurally brittle (can not be easily rolling, moulding, extruding or pressing). Hydrogen, carbon, nitrogen, oxygen, phosphorus, arsenic and selenium are the non-metallic elements in the periodic table.

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