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The Periodic Table

Explore the Periodic Table, groups, valence electrons, metalloids, and more. Discover the unique characteristics and relationships between elements like metals, nonmetals, and metalloids. Gain insights into luster, malleability, and ductility. Learn about the Alkali Metals, Alkaline Earth Metals, Transition Metals, Boron Family, Carbon Family, Nitrogen Family, Oxygen Family, Halogens, Noble Gases, Lanthanides, and Actinides.

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The Periodic Table

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  1. The Periodic Table

  2. The Father of the Periodic Table—Dimitri Mendeleev • Mendeleev was the first scientist to notice the relationship between the elements • Arranged his periodic table by atomic mass • Said properties of unknown elements could be predicted by the properties of elements around the missing element • Moseley later discovered that the periodic nature of the elements was associated with atomic number, not atomic mass

  3. Valence Electrons • Outermost (last shell) electrons in an atom • Electrons available for interactions with valence electrons of other atoms in chemical reactions

  4. Metalloid • Six elements: Boron, Silicon, Germanium, Arsenic, Antimony and Tellurium • Elements found along the stair-step line that separates metals from non-metals. • Chemical elements with properties that are in-between or a mixture of those of metals and nonmetals • Have a metallic appearance but they are brittle and only fair conductors of electricity

  5. The Periodic Table Column = Group or Family 18 columns on the Periodic Table Row = Period 7 rows on the Periodic Table

  6. Metals, Nonmetals, and Semi-metals Hydrogen Only nonmetal on the metal side Nonmetals are on the right of the stair-step Metals are to the left of the stair- step Semi-metals, “metalloids,” touch the stair-step

  7. What is luster, malleable and ductile? • Luster describes the way a surface reflects light…therefore metallic luster would be shiny like a metal object. • Malleable means to be able to press or pound the substance into sheets or different shapes. • Ductile means that the substance can be drawn out into thin wires.

  8. The Groups of the Periodic Table • Group 1: The Alkali Metals • Most reactive metals on the PT • Reactive in water and air thus stored in oil • Rarely found free in nature • Charge of +1: 1 valence electron (1 electron in the outer shell)

  9. The Groups of the Periodic Table Group 2: The Alkaline Earth Metals Still quite reactive React with water to form bases and hydrogen gas Have a silvery luster Good conductors of heat and electricity Charge of +2: 2 valence electrons (2 electrons in outer shell)

  10. T he Groups of the Periodic Table • Groups 3-12: Transition Metals • Found freely and in compounds in nature • Great conductors of electricity • Mixed with paints to achieve bright colors • include radioactive elements 89 through 109 • include Mercury, the only metal that is liquid at room temperature • Have a silvery luster, except Copper and Gold • Charge is usually 2 but can vary—usually 2 valence electrons (2 in outer shell)

  11. T he Groups of the Periodic Table • Group 13: Boron Family • Metallic (except Boron, which is a solid metalloid) • Scarce in nature (except Aluminum, which is the most abundant metallic element • Charge is +3: 3 valence electrons

  12. The Groups of the Periodic Table • Group 14: The Carbon Family • Contains elements that can form unusual bonds (Carbon and Silicon) • Includes a nonmetal (Carbon), two metalloids (Silicon and Germanium) and two metals (Tin and Lead) • Relatively unreactive • Charge is +4 or -4: contains 4 valence electrons

  13. T he Groups of the Periodic Table • Group 15: The Nitrogen Family • Consists of two nonmetals (Nitrogen and Phosphorus), two metalloids (Arsenic and Antimony), and one metal (Bismuth) • Nitrogen is most commonly found as atmospheric gas • Range from very abundant elements (Nitrogen and Phosphorus) to relatively rare elements (Arsenic, Antimony, and Bismuth) • Solids at room temperature, except Nitrogen • Charge is -3: contains 5 valence electrons

  14. The Groups of the Periodic Table • Group 16: The Oxygen Family • Consists of three nonmetals (Oxygen, Sulfur, and Selenium), one metalloid (Tellurium), and one metal (Polonium) • Also known as the Chalcogens • Charge is -2: 6 valence electrons

  15. T he Groups of the Periodic Table • Group 17: The Halogens • Most reactive nonmetals, with Fluorine being the most reactive of all nonmetals • Found in the rocks of Earth's crust and dissolved in sea water • Exist as a gas at room temperature (F2 and Cl2), a liquid (Br2), and a solid (I2 and At) • Charge is -1: 7 valence electrons

  16. T he Groups of the Periodic Table • Group 18: The Noble Gases (The Inert Gases) • Nonreactive • Colorless gases • Nonmetal • Charge is 0: 2 or 8 valence electrons- have a full outer energy level

  17. Special Rows on the PT Lanthanides Actinides

  18. Lanthanides Family • Very reactive; burns easily in air • 15 soft metals • Once called the Rare Earth Elements • Relatively abundant in Earth's crust • Found in Row 6 of the periodic table between Groups 3 and 4 • Occur together in nature, and they are very difficult to separate from each other • Silvery-white metals that tarnish when exposed to air, forming their oxides

  19. Actinides Family • All are radioactive. • 15 very dense metals- tarnish in air. • Actinides combine directly with most nonmetals

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