Metals Non-Metals and Metalloids

11 Key excerpts on "Metals Non-Metals and Metalloids"

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  Phase Transformations and Heat Treatments of Steels

  • Bankim Chandra Ray, Rajesh Kumar Prusty, Deepak Nayak(Authors)
  • 2020(Publication Date)
  • CRC Press

    (Publisher)

  Based on the broad physical and mechanical properties of elements, they are categorized into three groups, i.e., (i) metals, (ii) metalloids, and (iii) nonmetals. Typically, metals are of shiny lustrous appearance, when prepared fresh or fractured. They are good conductors of heat and electricity. Metals can be plastically deformed and are normally malleable (can be made to thin sheets) and ductile (can be drawn into wires). Except mercury, all other metals remain in their solid state at normal room temperature and exhibit crystalline arrangement of atoms. Around 91 out of 118 elements in the periodic table are metal. However, the exact number is not available, as the boundaries between metals, nonmetals, and metalloids fluctuate due to lack of globally accepted basis of categorization. Metals constitute around 25% of the earth’s crust and are inseparable from the present era of civilization. To a large extent, the development of civilization is driven by development in the field of metals and associated products. In the same line, a nonmetal is defined as an element that lacks in the metallic properties. Low density, boiling temperature, and melting temperature are some key physical properties of nonmetals. Most of the nonmetals are gases at room temperature and usually poor conductors of heat and electricity. Some nonmetals are brittle solids at room temperature but good conductors of electricity and heat, e.g., carbon. Metalloids exhibit properties that are in between metals and nonmetals or a mixture of metals and nonmetals. Boron, silicon, germanium, arsenic, antimony, and tellurium are the well-accepted metalloids. They usually have metal-like lustrous appearance but are only moderate conductors of heat and electricity.

  1.2     Types of Bonding between Atoms

  In general, materials in their solid state exhibit a well-arranged array of atoms forming a regular geometric pattern to reduce their free energy. However, solids such as glass, wax, and paraffin do not follow this trend, and the arrangement of atoms is similar to that of the liquid state and thus termed as amorphous solids. The next important point now is to consider the types of forces responsible to have bonds between adjacent atoms in order to complete the structure of the solid. Generally, there exist four types of interatomic bonding.

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  Chemistry

  The Molecular Nature of Matter

  • Neil D. Jespersen, Alison Hyslop(Authors)
  • 2018(Publication Date)
  • Wiley

    (Publisher)

  Figure 2.3 .) About 75% of the elements are metals, approximately 20 are nonmetals, and only a handful are metalloids.

  Periodic table: Metals, nonmetals, and metalloids

  Figure 2.3 Distribution of metals, nonmetals, and metalloids among the elements in the periodic table.

  Metals

  You probably know a metal when you see one, and you are familiar with their physical properties. Metals tend to have a shine so unique that it’s called a metallic luster. For example, the silvery sheen of the surface of potassium in Figure 2.4 would most likely lead you to identify potassium as a metal even if you had never seen or heard of it before. We also know that metals conduct electricity. Few of us would hold an iron nail in our hand and poke it into an electrical outlet. In addition, we know that metals conduct heat very well. On a cool day, metals always feel colder to the touch than do neighboring nonmetallic objects because metals conduct heat away from your hand very rapidly. Nonmetals seem less cold because they can’t conduct heat away as quickly and so their surfaces warm up faster.

  Figure 2.4 Potassium is a metal. Potassium reacts quickly with moisture and oxygen to form a white coating. Due to its high reactivity, it is stored under oil to prevent water and oxygen from reacting with it.

  Other properties that metals possess, to varying degrees, are malleability —the ability to be hammered or rolled into thin sheets—and ductility —the ability to be drawn into wire. The ability of gold to be hammered into foils a few atoms thick depends on the malleability of gold (Figure 2.5 ), and the manufacture of electrical wire is based on the ductility of copper.

  Figure 2.5 Malleability of gold. Pure gold is not usually used in jewelry because it is too malleable. It is used decoratively to cover domes since it can be hammered into very thin sheets called gold leaf.

  Hardness is another physical property that can be used to descibe metals. Some, such as chromium or iron, are indeed quite hard; but others, including copper and lead, are rather soft. The alkali metals such as potassium (Figure 2.4

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  Types of Solid Materials and Their Scientific Applications

  • (Author)
  • 2014(Publication Date)
  • Learning Press

    (Publisher)

  Elements to the lower left of this division line are called metals, while elements to the upper right of the division line are called non-metals. An alternative definition of metal refers to the band theory. If one fills the energy bands of a material with available electrons and ends up with a top band partly filled then the material is a metal. This definition opens up the category for metallic polymers and other organic metals, which have been made by researchers and employed in high-tech devices. These synthetic materials often have the characteristic silvery gray reflectiveness (luster) of elemental metals. Astronomy In the specialized usage of astronomy and astrophysics, the term metal is often used to refer collectively to all elements other than hydrogen or helium, including substances as chemically non-metallic as neon, fluorine, and oxygen. Nearly all the hydrogen and helium in the Universe was created in Big Bang nucleosynthesis, whereas all the metals were produced by nucleosynthesis in stars or supernovae. The Sun and the Milky Way Galaxy are composed of roughly 74% hydrogen, 24% helium, and 2% metals (the rest of the elements; atomic numbers 3-118) by mass. The concept of a metal in the usual chemical sense is irrelevant in stars, as the chemical bonds that give elements their properties cannot exist at stellar temperatures. ____________________ WORLD TECHNOLOGIES ____________________ Properties Chemical Metals are usually inclined to form cations through electron loss, reacting with oxygen in the air to form oxides over changing timescales (iron rusts over years, while potassium burns in seconds). Examples: 4 Na + O 2 → 2 Na 2 O (sodium oxide) 2 Ca + O 2 → 2 CaO (calcium oxide) 4 Al + 3 O 2 → 2 Al 2 O 3 (aluminium oxide) The transition metals (such as iron, copper, zinc, and nickel) take much longer to oxidize. Others, like palladium, platinum and gold, do not react with the atmosphere at all.

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  Chemistry: Atoms First 2e

  • Edward J. Neth, Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson(Authors)
  • 2019(Publication Date)
  • Openstax

    (Publisher)

  There are 20 nonradioactive representative metals in groups 1, 2, 3, 12, 13, 14, and 15 of the periodic table (the elements shaded in yellow in Figure 18.2). The radioactive elements copernicium, flerovium, polonium, and livermorium are also metals but are beyond the scope of this chapter. In addition to the representative metals, some of the representative elements are metalloids. A metalloid is an element that has properties that are between those of metals and nonmetals; these elements are typically semiconductors. The remaining representative elements are nonmetals. Unlike metals, which typically form cations and ionic compounds (containing ionic bonds), nonmetals tend to form anions or molecular compounds. In general, the combination of a metal and a nonmetal produces a salt. A salt is an ionic compound consisting of cations and anions. 862 18 • Representative Metals, Metalloids, and Nonmetals Access for free at openstax.org FIGURE 18.2 The location of the representative metals is shown in the periodic table. Nonmetals are shown in green, metalloids in purple, and the transition metals and inner transition metals in blue. Most of the representative metals do not occur naturally in an uncombined state because they readily react with water and oxygen in the air. However, it is possible to isolate elemental beryllium, magnesium, zinc, cadmium, mercury, aluminum, tin, and lead from their naturally occurring minerals and use them because they react very slowly with air. Part of the reason why these elements react slowly is that these elements react with air to form a protective coating. The formation of this protective coating is passivation. The coating is a nonreactive film of oxide or some other compound. Elemental magnesium, aluminum, zinc, and tin are important in the fabrication of many familiar items, including wire, cookware, foil, and many household and personal objects.

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  Chemistry: Atoms First

  • William R. Robinson, Edward J. Neth, Paul Flowers, Klaus Theopold, Richard Langley(Authors)
  • 2016(Publication Date)
  • Openstax

    (Publisher)

  There are 20 nonradioactive representative metals in groups 1, 2, 3, 12, 13, 14, and 15 of the periodic table (the elements shaded in yellow in Figure 18.2). The radioactive elements copernicium, flerovium, polonium, and livermorium are also metals but are beyond the scope of this chapter. In addition to the representative metals, some of the representative elements are metalloids. A metalloid is an element that has properties that are between those of metals and nonmetals; these elements are typically semiconductors. The remaining representative elements are nonmetals. Unlike metals, which typically form cations and ionic compounds (containing ionic bonds), nonmetals tend to form anions or molecular compounds. In general, the combination of a metal and a nonmetal produces a salt. A salt is an ionic compound consisting of cations and anions. 966 Chapter 18 | Representative Metals, Metalloids, and Nonmetals This OpenStax book is available for free at http://cnx.org/content/col12012/1.7 Figure 18.2 The location of the representative metals is shown in the periodic table. Nonmetals are shown in green, metalloids in purple, and the transition metals and inner transition metals in blue. Most of the representative metals do not occur naturally in an uncombined state because they readily react with water and oxygen in the air. However, it is possible to isolate elemental beryllium, magnesium, zinc, cadmium, mercury, aluminum, tin, and lead from their naturally occurring minerals and use them because they react very slowly with air. Part of the reason why these elements react slowly is that these elements react with air to form a protective coating. The formation of this protective coating is passivation. The coating is a nonreactive film of oxide or some other compound. Elemental magnesium, aluminum, zinc, and tin are important in the fabrication of many familiar items, including wire, cookware, foil, and many household and personal objects.

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  Chemistry 2e

  • Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson(Authors)
  • 2019(Publication Date)
  • Openstax

    (Publisher)

  There are 20 nonradioactive representative metals in groups 1, 2, 3, 12, 13, 14, and 15 of the periodic table (the elements shaded in yellow in Figure 18.2). The radioactive elements copernicium, flerovium, polonium, and livermorium are also metals but are beyond the scope of this chapter. In addition to the representative metals, some of the representative elements are metalloids. A metalloid is an element that has properties that are between those of metals and nonmetals; these elements are typically semiconductors. The remaining representative elements are nonmetals. Unlike metals, which typically form cations and ionic compounds (containing ionic bonds), nonmetals tend to form anions or molecular compounds. In general, the combination of a metal and a nonmetal produces a salt. A salt is an ionic compound consisting of cations and anions. 858 18 • Representative Metals, Metalloids, and Nonmetals Access for free at openstax.org FIGURE 18.2 The location of the representative metals is shown in the periodic table. Nonmetals are shown in green, metalloids in purple, and the transition metals and inner transition metals in blue. Most of the representative metals do not occur naturally in an uncombined state because they readily react with water and oxygen in the air. However, it is possible to isolate elemental beryllium, magnesium, zinc, cadmium, mercury, aluminum, tin, and lead from their naturally occurring minerals and use them because they react very slowly with air. Part of the reason why these elements react slowly is that these elements react with air to form a protective coating. The formation of this protective coating is passivation. The coating is a nonreactive film of oxide or some other compound. Elemental magnesium, aluminum, zinc, and tin are important in the fabrication of many familiar items, including wire, cookware, foil, and many household and personal objects.

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  Chemistry

  • Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson(Authors)
  • 2015(Publication Date)
  • Openstax

    (Publisher)

  Their properties and behavior are quite different from those of metals on the left side. Under normal conditions, more than half of the nonmetals are gases, one is a liquid, and the rest include some of the softest and hardest of solids. The nonmetals exhibit a rich variety of chemical behaviors. They include the most reactive and least reactive of elements, and they form many different ionic and covalent compounds. This section presents an overview of the properties and chemical behaviors of the nonmetals, as well as the chemistry of specific elements. Many of these nonmetals are important in biological systems. In many cases, trends in electronegativity enable us to predict the type of bonding and the physical states in compounds involving the nonmetals. We know that electronegativity decreases as we move down a given group and increases as we move from left to right across a period. The nonmetals have higher electronegativities than do metals, and compounds formed between metals and nonmetals are generally ionic in nature because of the large differences in electronegativity between them. The metals form cations, the nonmetals form anions, and the resulting compounds are solids under normal conditions. On the other hand, compounds formed between two or more nonmetals have small differences in electronegativity between the atoms, and covalent bonding—sharing of electrons—results. These substances tend to be molecular in nature and are gases, liquids, or volatile solids at room temperature and pressure. In normal chemical processes, nonmetals do not form monatomic positive ions (cations) because their ionization energies are too high. All monatomic nonmetal ions are anions; examples include the chloride ion, Cl − , the nitride ion, N 3− , and the selenide ion, Se 2− . The common oxidation states that the nonmetals exhibit in their ionic and covalent compounds are shown in Figure 18.19.

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  Study Guide to Accompany Basics for Chemistry

  • Martha Mackin(Author)
  • 2012(Publication Date)
  • Academic Press

    (Publisher)

  Metallic properties are related to low ionization potential, low electron affinity and large atomic size. Nonmetallic properties are related to high ionization potential, high electron affinity and small atomic size. Other periodic arrangements of the elements are described and illustrated. A brief survey of elements by periodic group is included. **Specifics** 1. Definitions for the following terms should be learned: periodic law period group alkali metals alkaline earth metals halogens noble gases main group elements representative elements metals nonmetals semimetals ductile malleable conductors transition elements inner transition elements lanthanides 75 76 Chapter Five actinides ionization energy electron affinity CHAPTER 5 TOPICAL OUTLINE I. History and definition 5.1 Periodic law A. history 1. Dohereiner organized the elements into groups of three elements (triads) that had similar properties. 2. Newland arranged the elements into groups of seven (Newland's octaves) so that the eighth element had properties similar to the first element. · 3. Mendeleev arranged the elements by atomic weight. a) This is the origin of the modern periodic table. b) This classification showed a regular repetition of certain pro-perties . c) Properties of undiscovered elements were successfully predicted based on the positions of blank spaces in the table. d) Because of the existence of isotopes, the arrangement by atomic weight was not completely successful; a few elements are located by their properties and are out of order by atomic weight. 4. When the elements are arranged by atomic number, they are located correctly by their properties. (Moseley determined the atomic numbers of the elements.) -» B. The definition of periodic law which is the basis for the modern periodic table states that the properties of the elements repeat in a regular way when the elements are arranged in order by increasing atomic number.

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  Trophic Interactions Within Aquatic Ecosystems

  • Ahmad Hemami(Author)
  • 2017(Publication Date)
  • CRC Press

    (Publisher)

  We may say elements are single materials that are not composed of separable substances. The number of known elements so far, as they appear in the Mendeleev table (periodic table of elements) is 118, and depending on the way and the magnitude they can combine together, they can compose millions of materials. The Mendeleev table as shown in Figure 3.1 contains various information about all elements. All other materials that we observe, i.e. those not in the Mendeleev table, are Figure 3.1 Mendeleev periodic table of the elements. (Copyright CRC Press.) compounds and are made up of two or more elements chemically bonded together. Going inside the elements has shown that they are all made out of only a few components. In this chapter, we are going to study this matter and see how electricity is related to the inside structure of the materials and how so many materials with various properties can be electrically categorized. 3.2 Material Properties Before getting into the basic structure of all materials, we can easily recognize that there are noticeable differences between various materials as we look around us. Consider, soil, wood, plastic, cloth, a piece of iron, gold, and aluminum. We can define the similarities and the differences between them. All the metals can be categorized as shiny, solid (except mercury that at normal temperature is in the form of liquid), and relatively heavier than many other materials. Moreover, they are conductors of heat. That is, if one side of a reasonably long piece of metal is heated, the heat moves to the other side. This is not true for cloth, wood, or plastic. One more difference between the above-named metals and the rest of the materials is that all the metals are among the elements, whereas others (e.g., cloth, wood, and plastic) are nonelements or compound materials. Elements are those seen in the Mendeleev table. Everything else is a compound, made out of some elements

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  Understanding General Chemistry

  • Atef Korchef(Author)
  • 2022(Publication Date)
  • CRC Press

    (Publisher)

  Chemically, they behave mostly as non-metals. They can form alloys with metals. Readily form glasses React with the halogens to form compounds

  Since metals tend to lose electrons and non-metals tend to gain electrons, metals and non-metals form ionic compounds with each other, such as Fe2 O3 and NaCl.

  Metals can be divided into alkali metals, alkaline earth metals, transition metals, lanthanides and actinides. Lanthanides and actinides form the rare earth elements. Non-metals include halogens and noble gases (Figure 7.5 ).

  FIGURE 7.5 Metals are divided into alkali metals, alkaline earth metals, transition metals, lanthanides and actinides. Non-metals include halogens and noble gases.

  7.3.1 Alkali Metals

  Atoms of the alkali metals present a valence shell (ns) and have one valence electron. The alkali family is found in the first column (Group 1) of the periodic table of elements. They include, among others, lithium (Li), sodium (Na) and potassium (K). Note that alkali metals do not include hydrogen, even though hydrogen belongs to the first group. Hydrogen is a nonmetal. The valence shell of the alkali family is incomplete (ns1 ). They are the most reactive metals. Elements that are reactive bond easily with other elements to make compounds. That is why, in nature, the alkali elements are not found free; they are always bonded with another element.

  7.3.2 Alkaline Earth Metals

  Alkaline earth metals present a valence shell (ns) and have two valence electrons. They are found in Group 2 of the periodic table of elements. The valence shell of the alkaline earth family is completely filled (ns2 ). Alkaline earth metals include, among others, beryllium (Be), magnesium (Mg) and calcium (Ca).

  7.3.3 Transition Metals

  Transition metals are elements where the atom has an incomplete d subshell, or which can give rise to cations with an incomplete d subshell. Transition metals are found from Group 3 to Group 12 in the periodic table of elements. They include iron (Fe), copper (Cu), nickel (Ni), gold (Au) and cobalt (Co), among others. They are good conductors of heat and electricity. They can lose many electrons when they form bonds with other atoms. Many transition metals combine chemically with oxygen to form oxides.

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  Electronic Materials

  Principles and Applied Science

  • Yuriy Poplavko(Author)
  • 2018(Publication Date)
  • Elsevier

    (Publisher)

  Their electronic properties are difficult to explain using existing concepts. The point is that these substances are the intermediate materials between magnetic and nonmagnetic materials as well as between metals and dielectrics, while valence electrons in them are found between the localized and free states. Investigation of these compounds helps to understand their metallic and magnetic properties, specify the conditions of “energy band arrangement” in metal and dielectric states, and understand some peculiarities of electronic states in crystals [9]. Metals with intermediate valence. During investigation of rare earth metal properties, the main attention is focused on a phenomenon known as “intermediate valence” or “heavy fermions.” It is appropriate to bear in mind that all electrons of atoms that form a solid can be divided into two groups: electrons strongly bounded inside atom (in the residue) and electrons that can leave its atom—they either move to another atom (i.e., from atom Na to atom Cl during formation of ionic rock salt crystal, NaCl) or form covalent bonds (such as in germanium crystal). Electrons also might be generalized within crystals, and this occurs with conduction electrons in metals. In all these cases, the conception of atom valence is used, that is, a number of electrons that can be detached and moved away from the atom in the process of solid formation. For example, valence of Na is “+ 1” as in ionic crystal (NaCl) so also in metal (Na). However, there are some known substances in which outward electrons demonstrate a binary, ambivalent nature: keeping partly localized in “native” atom, they also can demonstrate the intention to collectivization. Regarding the systems with unstable valence (or intermediary valence), some compounds of rare-earth metals can be included (those elements that have unfinished 4 f - electron shells)

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